Review sheet for Acids and Bases and Equilibrium Quiz – AP Chemistry
1. 10 mL of a base of 𝑝𝐻 9 can be converted to a solution of 𝑝𝐻 8 by ________________
2. What is the hydrogen and hydroxide ion concentration, 𝑝𝐻 and 𝑝𝑂𝐻 of a weak acid HA of
molarity 0.02, whose dissociation constant is 5 × 10−7
3. 50 Milliliters of 0.5 M sulfuric acid and 25 Milliliters of 2.5 M Sodium Hydroxide are mixed
together, the molarity of the resultant solution, hydrogen ion, hydroxide ion concentration, 𝑝𝐻
and 𝑝𝑂𝐻 are
4. 𝐻2 𝐶2 𝑂4+ 2 𝐻2 𝑂  2 𝐻3 𝑂+ + 𝐶2 𝑂42−
For reaction above, what is the equilibrium constant? Use the data given below.
𝐻2 𝐶2 𝑂4 + 𝐻2 𝑂  𝐻3 𝑂+ + 𝐻𝐶2 𝐻𝑂4−
K1 = 5
𝐻𝐶2 𝐻𝑂4− + 𝐻2 𝑂  𝐻3 𝑂 + + 𝐶2 𝑂42−
K2 = 10
In the above examples identify conjugate acid- base pairs.
5. The volume of 1 M Nitric acid required to neutralize 25 milliliters of 0.25 M Calcium
hydroxide assuming completing dissociation.
6. The dissociation constant of a weak base is 5.0 × 10−9 . What is the hydrogen and hydroxide
ion concentration, 𝑝𝐻 and 𝑝𝑂𝐻 of the base whose molarity is 0.03
7. Write all the possible Conjugate acid – base pairs in the given equations.
𝐻2 𝐶2 𝑂4 (aq)+ 𝐻2 𝑂(𝑙)  𝐻3 𝑂+ (𝑎𝑞) + 𝐻𝐶2 𝑂4− (𝑎𝑞)
𝐻𝐶2 𝑂4− (aq)+ 𝐻2 𝑂(𝑙)  𝐻3 𝑂 + (𝑎𝑞) + 𝐶2 𝑂42− (aq)
𝐻2 𝑂 (l) + 𝐻2 𝑂 (l) ⇄ 𝐻3 𝑂+ (aq) + 𝑂𝐻 − (aq)
8. The value of equilibrium constant for the reaction can be altered by
𝑃𝐶𝑙3 (g) + 𝐶𝑙2(g) ⇄ 𝑃𝐶𝑙5 (g) + energy
9. 100 milliliters of a weak acid is titrated with NaOH, a) Refer to your textbook or online
resource for the selection of indicators and identify the indicators that best suit for the titration.
B) 𝑝𝐾𝑎 of the acids is approximately C) the point at which the number of moles of acid is equal
to the number of moles of base d) the point at which 𝑝𝐻 is close to that the strong base added, e)
the point at which the concentrations of weak acid and its conjugate is equal is
10. Approximate 𝑝𝐻 of these mixtures is 1) 𝑁𝐻3 and 𝑁𝐻4 𝐶𝑙 2) 𝐻3 𝑃𝑂4 and 𝑁𝑎𝐻2 𝑃𝑂4
3) 𝐻𝐶𝑙 and 𝑁𝑎𝐶𝑙 4) 𝑁𝐻3 and 𝐻𝐶2 𝐻3 𝑂2 (acetic acid)
11. In this equilibrium 𝐻2 𝐶2 𝑂4 (aq)+ 𝐻2 𝑂(𝑙)  𝐻3 𝑂+ (𝑎𝑞) + 𝐻𝐶2 𝑂4− (𝑎𝑞), the strongest base is
12. 2 𝑋(𝑔) + 𝑌(𝑔) ⇄ 2𝑍(𝑔) When 0.40 mole of 𝑋 and 0.60 mole of 𝑌 are placed initially
in a 5 liter container and at equilibrium 0.3 mole of 𝑍 was found, Calculate equilibrium constant.
13. Write the formulas of all strong acids and strong bases.
14. Write the 𝑝𝐻 of aqueous solutions ( is it equal to 7 or greater than 7 or less than 7), the
hydrolysis equations, identify the parent acids, bases and mention is it cationic or anionic
hydrolysis of the following salts. 1. 𝐴𝑙(𝑁𝑂3 )3 2. 𝐾2 𝐶𝑂3 3. 𝐶𝑎𝐶𝑙2 4. 𝐿𝑖𝑁𝑂3 5. 𝐾𝐵𝑟 6. 𝑁𝐻4 𝐶𝑙
7. 𝐻𝐶2 𝐻3 𝑂2 8. 𝑁𝑎𝐹 9. 𝑁𝑎𝑁𝑂3 10. 𝑁𝑎𝐶𝑁 11. 𝑁𝑎𝐻𝑆𝑂4 12. 𝐶𝑎(𝑂𝐶𝑙)2
15. Write the conjugate acid and base of 𝑁𝐻3 𝑎𝑛𝑑 𝐻𝐶𝑙
16. 𝑝𝐻 of a solution is 3.2, the hydroxide and hydroxyl ion concentrations are
17. Write the conjugate acid and base of 𝐻2 𝑂 and 𝐻𝑆𝑂4−
18. 2 𝑋(𝑔) + 𝑌(𝑔) ⇄ 2𝑍(𝑔) the equilibrium constant for the reaction is 25, then the
1
equilibrium constant for the reaction 𝑍(𝑔) ⇄ 𝑋(𝑔) + 2 𝑌 is
19. 2 𝑋(𝑔) + 𝑌(𝑔) ⇄ 2𝑍(𝑔) for the equilibrium, reducing the volume of the container
________________ reaction is favored.
20. In the Haber process for the manufacture of Ammonia, the favorable conditions for the
formation of Ammonia are
21. 2 𝑋(𝑔) + 𝑌(𝑔) ⇄ 2𝑍(𝑔) , 4 moles of X and 6 moles of Y are placed in 1 liter container
and at equilibrium 3 moles of Z was found, calculate the equilibrium constant.
22. Calculate the molarity of 𝐶𝑙 − ion that precipitates 𝑃𝑏𝐶𝑙2 from a solution of 0.05 M
𝑃𝑏(𝑁𝑂3 )2 and the solubility product constant of 𝑃𝑏𝐶𝑙2 is 1.6 × 10−5
23. In a saturated solution of 𝑀(𝑂𝐻)3 the concentration of 𝑂𝐻 − is 3.0 × 10−6 , then the
solubility product constant of 𝑀(𝑂𝐻)3 at the same temperature is
24. Write the net ionic equation for the neutralization and precipitation reaction between sulfuric
acid and Barium hydroxide. Calculate the original molarity of Barium Hydroxide solution and
calculate the concentration of Barium ions in the solution at the equivalence point after30
milliliters of 0.1 M sulfuric acid is added. After the equivalence point addition of 1 more
milliliter of Sulfuric acid reduces the concentration of Barium ions, Justify your answer.
(The original volume of Barium hydroxide used is 25 Milliliter).
25. A solution contains 40.00 mL of 0.400 M NH4Cl(aq), The ammonium ion reacts with water
according to the equation NH4+(aq) + H2O(l) ⇄ NH3(aq) + H3O+(aq). Calculate the value of the
equilibrium constant for the reaction of the ammonium ion with water. (At 25 oC, the value of Kb
for NH3 is 1.8 x 10-5).
A solution is prepared by mixing 40.0 mL of 0.400 M NH3(aq) with 40.0 mL of 0.400 M
NH4Cl(aq). Is the solution acidic, basic, or neutral? Justify your answer