Name:____________________________________ AP Chemistry Review Acids and Bases
_____1. Which of the following best describes the pH of a 0.01-molar solution of HBrO?
(For HBrO, Ka = 2 × 10-9)
(A) Less than or equal to 2
(D) Between 7 and 11
(B) Between 2 and 7
(C) 7
(E) Greater than or equal to 11
_____2. A 1-molar solution of a very weak monoprotic acid has a pH of 5. What is the value of Ka for
the acid?
(A) Ka = 1 × 10-10
(B) Ka = 1 × 10-7
(C) Ka = 1 × 10-5
(D) Ka = 1 × 10-2
(E) Ka = 1 × 10-1
_____3. The concentrations of which of the following species will be increased when HCl is added to a
solution of HC2H3O2 in water?
i. H+
ii. C2H3O2iii. HC2H3O2
(A) I only
(D) II and III only
(B) I and II only
(E) I, II and III
(C) I and III only
_____4. The first acid dissociation constant for tartaric acid, H2C4H4O6, is 1.0 × 10-3. What is the base
dissociation constant for HC4H4O6-?
(A) Kb= 1.0 × 10-13 (B) Kb= 1.0 × 10-11 (C) Kb= 1.0 × 10-7 (D) Kb= 1.0 × 10-4 (E) Kb= 1.0 × 10-1
_____5. If 0.630 grams of HNO3 (molecular weight 63.0) are placed in 1 liter of distilled water at 25°C,
what will be the pH of the solution? (Assume that the volume of the solution is unchanged by
the addition of HNO3.)
(A) 0.01
(B) 0.1
(C) 1
(D) 2
(E) 3
Questions 6-8
A solution of a weak monoprotic acid is titrated with a solution of a strong base, KOH. Consider
the points labeled (A) through (E) on the titration curve that results as shown below.
_____6. The point at which the moles of the added strong base are equal to the moles of the weak acid.
_____7. The point at which the pH is closest to that of the strong base being added
_____8. The point at which the pH of the mixture is equal to the pKa of the acid.
9. a. A 0.100M solution of NH3 is prepared in a 125mL flask. What is the pH of the solution if Kb of
ammonia is 1.79 x 10-5?
b. A different solution is prepared containing 0.100-molar NH4Cl with 0.200-molar solution of NH3.
What is the pH of this new solution ? The value of Kb for ammonia is 1.79 × 10-5.
10. A sample of 40.0 milliliters of a 0.100 molar HC2H3O2 solution is titrated with a 0.150 molar
NaOH solution. The Ka value for acetic acid is1.8×10-5.
(a) What volume of NaOH is used in the titration in order to reach the equivalence point?
(b) What is the molar concentration of C2H3O2- at the equivalence point?
(c) What is the pH of the solution at the equivalence point?