ACID AND BASE EQUILIBRIA
1. Identify which species is /are Bronsted-Lowry acids and bases in the following reactions
a. NH4+ + HSO3- ⇌ NH3 + H2SO4
b. NH2- + H2O ⇌ NH3 + OH-
2. a. Calculate the percent ionization of a 0.20 M solution of the monoprotic acetylsalicylic acid (aspirin)
for which
Ka = 3.0 x 104-.
b. The pH of gastric juice in the stomach is 1.00. After swallowing 0.20 M of acetylsalicylic acid,
calculate the percent ionization of the aspirin in the stomach under these conditions.
3. Determine whether aqueous solutions of each of these salts are acidic, basic, or neutral:
a. Ba(CH3COO)2, b. NH4Cl, c. CH3NH3Br, d. KNO3, e. Al(ClO4)3.
4. If 10 mL of 0.6 M HClO solutions is titrated with 0.3 M KOH solution, calculate the pH of solution
when the volume of KOH added is as provided below. Take Ka of HClO to be 2.9 x 10-8.
a) 0 mL
b. 4 mL
c. 9 mL
d. 12 mL
e. 22.5 mL
1. Identify which species is /are Bronsted-Lowry acids and bases in the following reactions
a. NH4+ + HSO3- ⇌ NH3 + H2SO4
b. NH2- + H2O ⇌ NH3 + OH-
2. a. Calculate the percent ionization of a 0.20 M solution of the monoprotic acetylsalicylic acid (aspirin)
for which
Ka = 3.0 x 104-.
b. The pH of gastric juice in the stomach is 1.00. After swallowing 0.20 M of acetylsalicylic acid,
calculate the percent ionization of the aspirin in the stomach under these conditions.
3. Determine whether aqueous solutions of each of these salts are acidic, basic, or neutral:
a. Ba(CH3COO)2, b. NH4Cl, c. CH3NH3Br, d. KNO3, e. Al(ClO4)3.
4. If 10 mL of 0.6 M HClO solutions is titrated with 0.3 M KOH solution, calculate the pH of solution
when the volume of KOH added is as provided below. Take Ka of HClO to be 2.9 x 10-8.
a) 0 mL
b. 4 mL
c. 9 mL
d. 12 mL
e. 22.5 mL
