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WorksheetsAnalytical Chemistry: Acid-Base and Solubility Equilibrium
Total questions: 15
Worksheet time: 30mins
Name
Class
Date
1.
Calculate the concentration of chloride ions in a saturated lead (II) chloride (Ksp = 2.4 × 10^-4) solution.
a)
2.4 × 10^-4 M
b)
1.2 × 10^-4 M
c)
3.9 × 10^-4 M
d)
7.8 × 10^-4 M
e)
4.8 × 10^-4 M
2.
Which one of the following combinations cannot function as a buffer solution?
a)
NH3 and (NH4 )2SO4
b)
HNO3 and NaNO3
c)
HNO2 and NaNO2
d)
HF and NaF
e)
HCN and KCN
3.
A 2.1 L sample of a 0.23 M NaOH solution is mixed with 1.9 L of a 0.021 M KOH solution. What is the pH of the mixture?
a)
13.4
b)
13.04
c)
11.68
d)
12.84
e)
13.12
4.
Calculate the pH of a 1.6 M KOH solution.
a)
1.6
b)
-0.2
c)
13.8
d)
14.2
e)
0.2
5.
Will a precipitate of magnesium fluoride form when 300. mL of 1.1 x 10^-3 M MgCl2 are added to 500. mL of 1.2 × 10^-3 M NaF? [Ksp (MgF2) = 6.9 × 10^-9]
a)
Yes, Q = Ksp
b)
No, Q < Ksp
c)
Yes, Q > Ksp
d)
No, Q = Ksp
e)
Yes, Q < Ksp
6.
Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 9.2–9.3?
a)
NH3/NH4Cl (Ka= 5.6 × 10^-10)
b)
CH3COONa/CH3COOH (Ka= 1.8 × 10^-5)
c)
NaOCl/HOCl (Ka = 3.2 × 10^-8)
d)
NaNO2/HNO2 (Ka = 4.5 × 10^-4 )
7.
The pH of a 0.6 M solution of a weak acid is 4.0. What percent of the acid has ionized?
a)
3.0E-4
b)
2.0E-4
c)
4.0E-4
d)
1.0E-4
8.
Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 4.6–4.8?
a)
NH3/NH4Cl (Ka = 5.6 × 10^-10 )
b)
NaNO2/HNO2 (Ka = 4.5 × 10^-4)
c)
NaOCl/HOCl (Ka = 3.2 × 10^-8)
d)
CH3COO2Na/CH3COOH (Ka = 1.8 × 10^-5)
9.
What is the pH of a solution prepared by mixing 50.0 mL of 0.300 M HCl with 450.0 mL of 0.400 M HIO3 ? [Ka(HIO3) = 1.6 × 10^-1]
a)
1.52
b)
0.66
c)
0.72
d)
0.89
e)
0.8
10.
Which of the following does not fit the definition of a Brønsted Acid?
a)
H2O
b)
NH4+
c)
CO2
d)
H2PO4–
e)
H3PO4
11.
Which one of the following statements is true for a 0.1 M solution of a weak acid HA?
a)
The pH equals 1.0
b)
The concentration of H+ is slightly less than the concentration of A-.
c)
The concentration of H+ is slightly greater than the concentration of A-.
d)
The concentration of H+ is exactly equal to the concentration of A-.
e)
The pH is less than 1.0.
12.
Which one of the following equations represents the ionization of a weak monoprotic acid in water?
a)
HCN(aq) + OH (aq) ⇌ H2O(l) + CN (aq)
b)
HCN(aq) + NH3(aq) ⇌ NH4CN(aq)
c)
HCN(aq) + OH-(aq) ⇌ H2O(l) + CN-(aq)
d)
HCN(aq) + H2O(l) ⇌ H3O+ (aq) + CN- (aq)
e)
CN-(aq) + H2O(aq) ⇌ HCN(aq) + OH- (aq)
13.
Predict the direction in which the equilibrium will lie for the reaction:<br />H2CO3 + F- ⇌ HCO3- + HF<br />Ka1(H2CO3) = 4.2 × 10^-7 Ka(HF) = 7.1 × 10^-4
a)
to the left
b)
in the middle
c)
to the right
14.
Calculate the pH of a 0.20 M solution of the weak base pyridine. (C5H5N; Kb = 1.7 x 10^-9)
a)
9.37
b)
9.27
c)
9.17
d)
9.47
e)
None of the above
15.
Which one of these equations represents the reaction of a weak acid with a strong base?
a)
OH-(aq) + HCN(aq) ➡ H2O(aq) + CN- (aq)
b)
H+(aq) + CH3NH2 (aq) ➡ CH3NH3+ (aq)
c)
H+(aq) + OH-(aq) ➡ H2O(aq)
d)
HCN(aq) + CH3NH2 (aq) ➡ CH3NH3+ (aq) + CN- (aq)
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