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Determine the pH of the following solutions. (a) a 0.48 M CH3COOH solution (b) a solution...

Determine the pH of the following solutions.

(a) a 0.48 M CH₃COOH solution

(b) a solution that is 0.48 M CH₃COOH and 0.22 M CH₃COONa

Expert Solution

a. CH3COOH -----------------> CH3COO^- (aq) + H^+ (aq)

I 0.48 0 0

C -x +x +x

E 0.48-x +x +x

ka = [CH3COO^-][H^+]/[CH3COOH]

1.8*10^-5 = x*x/0.48-x

1.8*10^-5*(0.48-x) = x^2

x = 0.00293

[H^+] = x = 0.00293M

PH = -log[H^+]

= -log0.00293

= 2.5331

b. [CH3COOH] = 0.48M

[CH3COONa] = 0.22M

PH = Pka + log[CH3COONa]/[CH3COOH}

= 4.75 + log0.22/0.48

= 4.75-0.3388

= 4.4112 >>>answer

queen_honey_blossom answered 2 years ago

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