Transcript Slide 1

Arrhenius Definitions:
+
H
Acids: liberate
ions in
solution.
Bases: liberate OH ions
in solution.
An acid-base
reaction in which
water is formed is
called a
neutralization.
Brӧnsted- Lowry
Definitions:
Acids: proton donors
Bases: proton acceptors
What volume of 0.20 M NaOH must
be added to 25.0 mL of 0.15 M
HC2H3O2 to neutralize the acid?
25.0 mL acetic acid
1
0.15 mol
1 mole NaOH
1000.0mL
1 mole acetic acid
1000.0 mL
0.20 mol NaOH
=19 mL NaOH
Volume of acid
present
Molarity of
acid
Mole ratio
MaVa(1/Mb)= Vb
Upside down
molarity of
= volume
base…1/Mb of base
needed
MaVa = MbVb
Ba(OH)2
What volume of 0.20 M NaOH must
be added to 25.0 mL of 0.15 M
HC2H3O2 to neutralize the acid?
25.0 mL acetic acid
1
Ba(OH)2
1 mole NaOH
0.15 mol
1000.0mL
1 mole acetic acid
2
1000.0 mL
Ba(OH)2
0.20 mol NaOH
= 19 mL NaOH
Volume of acid
present
Molarity of
acid
Mole ratio
MaVa(1/Mb)= Vb
9.4 mLBa(OH)2
Upside down
molarity of
= volume
base…1/Mb of base
needed
MaVa = 2MbVb
(If base has 2 hydroxides/formula)
MaVa = MbVb
(for one to one mole ratio neutralizations)
MaVa = 2MbVb
(for neutralizations involving bases with 2
hydoxides per FU)
2MaVa = MbVb
(for neutralizations involving diprotic acids)
What is the molarity of an H2SO4
solution if a volume of 22.3 mL of LiOH
(with a concentration of 0.75 M) is
needed to neutralize 100.0 mL of it?
2MaVa = MbVb
2Ma(100.0 mL) = (0.75 M)(22.3mL)
Ma = 0.084 M