Which of the following acid-base reactions should go more or less to completion?

(a) HClO4(aq) + OCl-(aq) ➝ ClO4-(aq) + HOCl(aq)

 (b) HF(aq) + I-(aq) ➝ HI(aq) + F-(aq)

   (c) H2SO3(aq) + SO42-(aq) ➝ H2SO4(aq) + SO32-(aq)

    (d) H2S(aq) + 2 Cl-(aq) ➝ S2-(aq) + 2 HCl(aq)

    (e) All of these reactions would go to completion, giving high yields of products.

NaHCO3 can be used to neutralize strong bases, such as NaOH. What conclusion can be drawn from the fact that the following acid-base reaction proceeds to the right as written?

                    HCO3-(aq) + OH-(aq) ➝ CO32-(aq) + H2O(l)

          (a) HCO3- is a stronger acid than H2O

         (b) HCO3- is a stronger base than CO32-

         (c) HCO3- is a stronger base than OH-

         (d) CO32- is a stronger base than OH-

         (e) H2O is a stronger acid than HCO3-

Which of the following isn’t a conjugate acid/base pair?

         (a) NH4+(aq) and NH3(aq)                      (b) H2O(l) and OH-(aq)

          (c) H3O+(aq) and OH-(aq)            (d) NH3(aq) and NH2-(aq)

Which of the following is the strongest Brønsted acid?

(a) NH4+ 

(b) HCl

 (c) HNO3

 (d) HSO4-

 (e) HClO4
 

 Which of the following solutions would be the best buffer when a small amount of NaOH is added to the solution?

(a) a 1.0 L solution prepared by adding 0.10 mol of carbonic acid and 0.10 mol of sodium bicarbonate.

(b) a 1.0 L solution prepared by adding 0.20 mol of carbonic acid and 0.20 mol of sodium bicarbonate.

(c) a 1.0 L solution prepared by adding 0.10 mol of hydrochloric acid and 0.10 mol of sodium hydroxide.

(d) a 1.0 L solution prepared by adding 0.20 mol of hydrochloric acid and 0.20 mol of sodium hydroxide.

 (e) all of these solutions would have the same buffer capacity.

 How would you increase the buffering capacity of a buffer made by adding NaHCO2 to an aqueous solution of HCO2H?

         (a) increase the concentration of HCO2H.

         (b) increase the concentration of NaHCO2.

          (c) increase the concentrations of both HCO2H and NaHCO2.

         (d) increase the ratio of the concentration of HCO2H to NaHCO2.

         (e) increase the ratio of the concentration of NaHCO2 to HCO2H.

For a weak diprotic acid, H2A, for which Ka1 = 2.1 x 10-7 and Ka2 = 4.3 x 10-13 the A2- ion concentration at equilibrium will be:

         (a) approximately equal to the initial concentration of H2A.

          (b) roughly equal to Ka2.

          (c) roughly equal to the HA- concentration.

         (d) much larger than the HA- concentration.

         (e) approximately equal to the H3O+ concentration