What is the pH of a solution containing 0.27 M HCOOH and 0.33 M HCOOK? The Ka for HCOOH is 1.7 × 10−4.?
- davidLv 76 months ago
Ka = [H+][HCOO-]/[HCOOH]
1.7x10^-4 = x(0.33+x)/(0.27-x) <<< x is small, "round"
1.7x10^-4 = x(0.33)/(0.27) <<< solve for x
x = [H+] = 1.3909x10^-4 <<< round for sig figs
pH = 3.8567 <<< round for sig figs ... that is your job to finish the problem