Acid and Base Review Game
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Transcript Acid and Base Review Game
Acid and Base
Review Game
Chemistry
Name the Acid
HNO2
Nitrous Acid
H2SO4
Sulfuric Acid
HCl
Hydrochloric Acid
HBr
Hydrobromic Acid
HClO
Hypochlorous Acid
Name the Base
NaOH
Sodium Hydroxide
Ca(OH)2
Calcium Hydroxide
Mg(OH)2
Magnesium Hydroxide
KOH
Potassium Hydroxide
Write the Formula
Nitric Acid
HNO3
Hydroiodidic Acid
HI
Phosphoric Acid
H3PO4
Acetic Acid
HC2H3O2
Write the Formula
Sodium carbonate
Na2CO3
Barium hydroxide
Ba(OH)2
Lithium hydroxide
LiOH
Arrhenius
What is the definition of an
acid?
A substance which produces H+ when put in water
What is the definition of a
base?
A substance which produces OH- when put in water
If a soap has a hydrogen
ion concentration of
-6
2.0 x 10 M, what is the pH
of the solution? The pOH?
Is it an acid or a base?
[H+] = 2 x 10-6M pH = -log(2 x 10-6) = 5.7
pOH = 14 – 5.7 = 8.3
Acid because pH < 7
What is the hydrogen ion
concentration and hydroxide
ion concentration of a solution
with a pH of 2.3? Is the
substance an acid or base?
[H+] = 10-2.3 = 0.005 M
pOH = 14 – 2.3 = 11.7
[OH-] = 10-11.7 = 2 x 10-12 M
Acid because pH < 7
What is the hydrogen ion
concentration of a sample of
phosphoric acid that has a pH of
4.9? What is the concentration
of phosphoric acid?
[H+] = 10-4.9 = 1.3 x 10-5M
Since there are 3 H’s in each H3PO4 … the concentration of phosphoric
acid would be a third of the concentration of H+
1.3 x 10-5/3 = 4.2 x 10-6 M
Neutralization Reaction
What is the
neutralization reaction
for nitrous acid reacting
with potassium
hydroxide?
HNO2 + KOH KNO2 + H2O
Neutralization Reaction
Write the complete
balanced equation for
the neutralization of
phosphoric acid with
calcium hydroxide
2H3PO4 + 3Ca(OH)2 Ca3(PO4)2 + 6H2O
How many grams of copper
(II) sulfate pentahydrate will
be needed to make 75 mL
of a 0.250 M solution?
CM = n/V
.25 = n/0.075
n = 0.01875 mol x 249.5 = 4.7 g
How many kilograms of
sucrose C12H22O11 will
be needed to make 3.50
L of a 1.15 M solution?
CM = n/v
1.15 = n/3.5
n = 4.025 mol x 342 = 1376.55 g / 1000 = 1.38 kg
What is the pH of a
solution made with
0.15 grams of barium
hydroxide in 4500 mL
of water?
What is the molar
concentration of a solution
that contains 0.0750 moles
of NaHCO3 in a volume of
115 mL
CM = n/v
CM = 0.075/.115 = 0.65 M
A solution has 3.00 moles of
solute in 2.00 L of solution,
what is its molar
concentration? How many
moles would there be in 350
mL of solution?
CM = n/V
CM = 3/2 = 1.5M
1.5 = n/0.35
n = 0.53 mol
Describe in your own words
how you would prepare 1.00L
of a 0.85 M solution of formic
acid HCO2H?
CM = n/v
0.85 = n/1
n = 0.85 mol x 46 = 39.1 g
Take 39.1 grams of formic acid and dissolve in a little bit of
water. Put into a 1.00 L volumetric flask and fill to the line with
water
What is the molarity of a
sulfuric acid solution which
contains 5.4 grams of sulfuric
acid in 250 mL of water?
What is the normality?
5.4g/98 = 0.055 mol
CM = 0.055/0.25 = 0.22 M
N = (eq)M = 2 x 0.22 = 0.44 N
What is the molarity of a
potassium hydroxide solution
which contains 0.94 moles of
potassium hydroxide in 450
mL of water? What is the
normality?
CM = 0.94/0.45 = 2.1 M
N = (eq)M = 1 x 2.1 = 2.1 N
In the titration of 35 mL of liquid
drain cleaner containing NaOH,
50 mL of 0.4M HCl must be
added to reach the equivalence
point. What is the molarity of the
base in the cleaner?
NaVa = NbVb
(0.4)(50) = Nb(35)
Nb = 0.57 N / 1 = 0.57 M
Calculate how many
milliliters of 0.25 M
Ba(OH)2 must be added to
titrate 46 mL of 0.40 M
HClO4
NaVa = NbVb
0.4(46) = 0.5Vb
Vb = 36.8 mL
A 15.5 mL sample of 0.215 M
KOH was titrated with an acetic
acid solution, It took 21.2 mL of
the acid to reach the equivalence
point. What is the molarity of the
acetic acid?
(0.215)(15.5) = Na(21.2)
Na = 0.157 N / 1 = 0.157 M
What is the molarity
of a solution of
phosphoric acid with
a pH of 2.65?
10-2.65 = 0.0022M / 3 = 7.62 x 10-4 M
A 20 mL sample of an HCl
solution was titrated with
27.4 mL of a standard
solution of Ba(OH)2. The
concentration of the
standard is 0.0154 M. What
is the molarity of the HCl?
(0.0308)(27.4) = Na(20)
Na = 0.042N / 1 = 0.042M
Buffer
What is a buffer?
A solution that resists changes in pH
Buffer
What are buffers
made of? Where can
you find them?
Weak acid and its conjugate base
Weak base and its conjugate acid
You can find them in your BLOOD
I want to dilute 20 mL of a 6M
solution of acetic acid to a
3.8M solution of acetic acid.
How much water should I add
to the 6M acetic acid to
achieve this?
6(20) = 3.8V
V = 31.6 mL
ADD 11.6 mL of water
I mix 20 mL of 4.5M
NaCl with 40 mL of
water. What is the new
concentration of the
NaCl?
4.5(20) = M(60)
M = 1.5 M
A 450 mL solution of 1.5 M
HCl is sat out over night. 150
mL of the water evaporated.
What is the new
concentration of the HCl?
1.5 (450) = M (300)
2.25 M
What does the term
“strong acid” mean?
Strong acid means that the acid
dissociates completely in water
I used 50 grams of
potassium chromate to
make a 1.4M solution.
What is the volume of the
solution?
50 g K2CrO4 / 194 = 0.26 mol
1.4 = .26/v
V = 0.184 L
What is the pH of a
solution made by putting
6.0 grams of phosphoric
acid in 250 L of water?
6 g H3PO4 / 98 = 0.0612 mol
[H3PO4] = 0.0612 / 250 = 2.45 x 10-4
[H+] = 3(2.45 x 10-4) = 7.35 x 10-4
pH = -log(7.35 x 10-4) = 3.13
What is the pH of a solution
made by putting 3.25 grams
of strontium hydroxide in
5000 L of water?
3.25 g Sr(OH)2 / 121.6 = 0.0267 mol
[Sr(OH)2] = 0.0267/ 5000 = 5.34 x 10-6M
[OH-] = 2(5.34 x 10-6) = 1.07 x 10-5 M
pOH = -log(1.07 x 10-5) = 4.97
pH = 14 – 4.97 = 9.03