Determine the pH of the following solutions. (a) a 0.36 M CH3COOH solution (b) a solution...

Determine the pH of the following solutions.

(a) a 0.36 M CH3COOH solution

(b) a solution that is 0.36 M CH3COOH and 0.22 M CH3COONa

Expert Solution

Determine the pH of the following solutions.
(a) a 0.36 M CH3COOH solution
       CH3COOH + H2O <--> CH3COO- + H3O+
I            0.36 -          0        0
C            -x   -                +x       +x
E           0.36-x    -           x        x

Ka = [CH3COO-][H3O+]/[CH3COOH]
1.8 x 10^-5 = (x²)/(0.36-x) (since, x is very small, we can 0.36 -x ~ 0.36)
x² = 0.36 x 1.8 x 10^-5
   = 6.48 x 10^-6
x = 2.55 x 10^-3 M
Therefore, [H₃O⁺] = 2.55 x 10^-3 M
pH = -log[H₃O⁺]
   = -log(2.55 x 10^-3 M)
   = 2.59

pH = 2.59

(b) a solution that is 0.36 M CH₃COOH and 0.22 M CH₃COONa
       CH3COOH + H2O <--> CH3COO- + H₃O⁺
I        0.36 M         -              0.22M      0
C            -x           -        +x           +x
E        0.36 M-x    -           0.22+x        x

Ka = 1.8 x 10^-5 = [(x)(0.22+x)/(0.36-x)] (since, x is very small, we can take (0.22 + x)~ 0.22 and (0.36-x) ~ 0.36)
   1.8 x 10^-5 = [(x)(0.22)/(0.36)]
   2.95 x 10^-5 = x
   Therefore [H₃O⁺] = 2.95 x 10^-5 M
   pH = -log[H₃O⁺]
       = -log(2.95 x 10^-5 M )
       = 4.53

   pH = 4.53

queen_honey_blossom answered 2 years ago

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