1. Are the aqueous solutions of the following acidic, basic or neutral in terms of their acidity? If they are either acidic or basic, write a reaction equation that explains this property.

a) NH₃

b) NH₄Cl

c) NaCN

d) NaCl

e) HNO₃

f) CH₃ OH ( a non electrolyte)

g) NaOH

h) AcOH

2. What is the pH of a 0.56 M solution of NaOAc?

3. What is the pH of a 0.23 M solution of NH₄Cl?

 (answer = 4.95)

4. Define the following terms a)amphoteric b) hydrolysis c) strong electrolyte d) weak acid e) buffer solution

5. What is the pH of a solution that is .03 M in NH₃ and 0.45 M in NH₄ Cl? K_b of NH₃ is 1.8x10 ^-5 .

 (answer = 8.1)

6. Calculate the value of the equilibrium constants for the following reactions from the value of Kb = 1.8x10^-5 for NH₃ and K_w.

a) NH₄ ⁺ (aq) + OH ^-(aq) = NH₃ (aq) + H₂O(l)

b) NH₄ ⁺ (aq) = H ⁺ (aq) + NH₃ (aq)

c) NH₃ (aq) + H ⁺ (aq) = NH₄ ⁺ (aq)

7. Define the following terms and give an example of each using acetic acid or acetic acid derivitives.

a) hydrolysis b) strong electrolyte c) weak acid

d) buffer solution e) conjugate base of an acid

8. Calculate the % ionization of acetic acid in a 0.2 M solution of acetic acid.