Question

Calculate the pH of the solution that results from diluting .50 mol HCO2H and .10 mol NaHCO2 in water to a final volume of 750 mL (Ka of HCO2H = 1.8 x 10^-4)

Answer 1

Upon solvation, formic acid will form:

\(HCOOH_{\;(aq.)} + H_2O\) \(\rightleftharpoons\) \(H_3O^++ HCOO^{\;-}\)

so, write an equilibrium expression, and find \([H_3O^+]\).

then use: pH=-log\([H_3O^+]\), to find the pH.