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Dichloroacetic acid has an acid dissociation constant of k0a = 3.32*10-2 mol/kg at 250 c calculate...

Dichloroacetic acid has an acid dissociation constant of k⁰_a = 3.32*10^-2 mol/kg at 25⁰ c calculate the degree of dissociation and pHof 0.01 mol/kg solution

taking all activity coefficients equal to 1 and compute necessary activity coefficients from the devies equation

Expert Solution

CHCl₂COOH H⁺ + CHCl₂COO^-

0.01 0 0 - intial stage

0.01-0.01 0.01 0.01

is degree of dissociation

K = [H⁺][CHCl₂COO^-]/CHCl₂COOH

3.32*10^-2 = (0.01)²/(0.01-0.01)

² + 3.32-3.32

By solving the above quadratic equation

= 0.8048

[H⁺] = 0.01x 0.8048

=8.0 x 10^-3

p^H = -log(8.0x10^-3)

= 2.1

Davies equation

Ionic strength of solutiom (CHCl₂COOH) I = 1/2(C_H⁺(z_H⁺)² + C_CHCl2COO^- (z_CHCl2COO^-)²)

z= charge on ion

C_H⁺ = C_CHCl2COO^- = 8.0 x 10^-3

z_H⁺ = z_CHCl2COO^- = 1

I = 1/2(8.0*10^-3(1)² + 1/2(8.0*10^-3(1)²)

= 8.0*10^-3

-logf = 0.5x1x1{(8.0*10^-3/ 1+ 8.0*10^-3)-0.05x8.0*10^-3}

= 0.03435

molal activity coefficient (f) = 1.0823

queen_honey_blossom answered 2 years ago

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Dichloroacetic acid has an acid dissociation constant of k0a = 3.32*10-2 mol/kg at 250 c calculate...

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