Answer Happy

A) Calculate the pH of a 0.012 M acetic acid,
HC2H3O2, solution. Its
Ka = 1.8 x 10-5.
B)Calculate the pH of a 0.012 M sodium acetate,
NaC2H3O2, solution. For acetate,
the Kb = 5.6 x 10-10.
C)Calculate the pH of a solution that is both 0.24 M acetic
acid, HC2H3O2, and 0.12 M sodium
acetate, NaC2H3O2. For acetic
acid, the Ka = 1.8 x 10-5.
D)Calculate the pH of a solution that is both 0.36 M ammonia,
NH3, and 0.36 M ammonium chloride, NH4Cl. For
ammonia, the Kb = 1.8 x 10-5.
E)Calculate the pH of a solution prepared by disolving 1.60 g of
sodium acetate CH3COONa. in 53.5 mL of .20 M acetic acid CH3COON
(aq). Assume the volume change upon dissolving the sodium acetate
is Ka of CH3COOH is 1.75 x 10^-5.