Transcript Concentration of solutions
Slide 1
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 2
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 3
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 4
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 5
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 6
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 7
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 8
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 9
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 10
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 11
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 12
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 13
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 14
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 15
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 16
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 17
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 18
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 19
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 2
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 3
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 4
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 5
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 6
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 7
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 8
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 9
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 10
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 11
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 12
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 13
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 14
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 15
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 16
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 17
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 18
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4
Slide 19
CONCENTRATION OF
SOLUTIONS
Day 4
CONCENTRATION
A measurement of the amount of solute in a
given amount of solvent or solution (unit of
measurement = molarity)
Kind of like the “strength” of the solution
MOLARITY
Molarity (M)=
mol solute
L solution
MOLARITY
Example #1: If we put 0.500 mol of
sodium hydroxide into 1.00 L of solution,
what is the molarity of the solution?
Molarity= mol solute/L sol’n
M=
=
0.500 mol NaOH
1.00 L
0.500 M NaOH
Example #2: What is the
molarity if we have 80.0 g
NaOH in 1.00 L of solution?
Molarity= mol solute/L sol’n
80.0 g NaOH
1 mol NaOH =2.00 mol
40.0 g NaOH
2.00
M
NaOH
=
2.00
mol
NaOH
M=
1.00 L
MOLARITY
Example #3: How many moles of KOH
are in 0.500 L of 0.100 M KOH?
Molarity= mol solute cross multiply!
1
L sol’n
mol KOH= (0.100 M KOH) (0.500 L)
= 0.0500 mol KOH
MOLARITY
Ex 4: How many grams of KOH
are in 2.75 L of 0.25 M KOH?
Molarity = moles
cross multiply!
L
Moles = Molarity * L
= 0.25 mol/L * 2.75L
= 0.69 moles KOH
0.69 mol KOH
56.097 g KOH = 38.7 g KOH
1 mole KOH
(39)
MOLARITY - DILUTION
Some chemicals are sold as pre-prepared
concentrated solutions (stock solutions).
To be used, stock solutions usually must be
diluted.
ALWAYS ADD ACID
2.) MOLARITY - DILUTION
MSVS = MDVD
• MS – Molarity of stock solution
• VS – Volume of stock solution (L or mL)
• MD – Molarity of dilute solution
• VD – Volume of dilute solution (L or mL)
*In dilution calculations,
the units for volume
must be the same.
2.) MOLARITY - DILUTION
Example #1: How much 12.0 M HCl is
required to make 2.50 L of a 0.500 M
solution?
Ms * Vs = MD * VD
MS VS = MD VD
MS = 12.0 M HCl
VS = ??
VS =
OR M1 V1 = M2 V2
MD = 0.500 M HCl
VD = 2.50 L
(0.500 M HCl) (2.50 L)
(12.0 M HCl)
= 0.104 L HCl
2.) MOLARITY - DILUTION
Example #2: What volume of a 1.50 M
solution can be made using 0.0250 L of
18.0 M H2SO4 ?
MS VS = MD VD
MS VS = MD VD
MS = 18.0 M H2SO4
VS = .0250 L
VD =
MD = 1.50 M H2SO4
VD = ????
(18.0 M H2SO4) (.0250 L)
(1.50 M H2SO4)
= 0.300 L H2SO4