what is the pH of a 0.025 M aqueous solution of sodium propionate, NaC3H5O2? What is the concentration of propionic acid in the solution?

Answer 1

This is a hydrolysis problem. The sodium propionate ion (which I'll call Pr^-) hydrolyzes.
Pr^- + HOH ==> HPr + OH^-
Set up an ICE chart and substitute into the Kb expression for Pr^-. (HPr is propionic acid).
Kb = (Kw/Ka) = (HPr)(OH^-)/(Pr^-).
(HPr_ = x = (OH^-). (Pr^-) = 0.025M from the problem. Solve for x and convert to pH. Post your work if you get stuck.