Calculate the pH of a 0.360 M solution of sodium acetate, CH3COONa. (Ka = 1.7 x

Question

Calculate the pH of a 0.360 M solution of sodium acetate, CH3COONa. (Ka = 1.7 x 10-5)

Explanation / Answer

sodium acetate is a strong salt CH3COONa => CH3COO- + Na+ Sodium acetate is a strong electrolyte CH3COONa ----> CH3COO- + Na+ CH3COO- + H2O CH3COOH + OH- start 0.38 change -x .. . . . . . .. . .. . . . . . . . +x. . .. . . +x at equilibrium 0.38-x. . . . . . . .. . . . . . . .x. . . .. .. . x the constant of this equilibrium also called hydrolysis constant or Kb is Kb = Kw/Ka = 1.0 x 10^-14 / 1.8 x 10^-5 = 5.6 x 10^-10 = x^2 / 0.38-x x = [OH-]=1.46 x 10^-5 M pOH = 4.8 pH = 14 - 4.8 = 9.2

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