Calculate the concentration and the pH in a .10 M solution of sodium acetate, Na(CH3CO2). Equilibrium...

Calculate the concentration and the pH in a .10 M solution of sodium acetate, Na(CH3CO2). Equilibrium constant of acetic is 1.8*10^-5.

Expert Solution

The dissociation of 0.10 sodium acetate CH3COONa yields 0.10 M acetate ion and 0.10 M Na⁺ ion.

CH₃COO^- (aq) + H₂O (l) <------------> CH₃COOH (aq) + OH^- (aq)

I(M) 0.10 - 0 0

C -x +x +x

Eq (0.10-x) x x

K_b = K_w/K_a = 5.55*10^-10 = (x)(x) / (0.10-x)

By solving - x = [OH^-] = 7.453*10^-6 M

Thus - pOH = -log [OH^-] = -log (7.453*10^-6 ) = 5.12

Hence - pH = 14 - 5.12 = 8.88

queen_honey_blossom answered 7 months ago

calculate the ph of .010 M sodium acetate

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