Chloroacetic acid has a dissociation constant of ka =0.000138 calculate the degree of dissociation for 0.0825m solution of this acid using the Debye -Huckel limiting law 

A weak acid has a dissociation constant of Ka = 0.025.

(a) Calculate the degree of dissociation for a 0.094 m solution of this acid using the Debye-Huckel limiting law.

(b) Calculate the degree of dissociation for a 0.094 m solution of this acid that is also 0.200 m KCl from the Debye-Huckel limiting law using an iterative calculation until the answer is constant in the second decimal place.

(c) Repeat the calculation (b) using the value of \(\gamma\pm\) = 0.718 for KCl.

This problem is from the Engel-Reid Physical Chemistry textbook, 3rd edition. Problem 10.5. Chegg does not have solutions for this chapter...

a) Trichloroacetic acid, CCl₃COOH, has an acid dissociation constant of 2.0 × 10^-1 at 25 °C. Calculate the pH of a 0.0420 M trichloroacetic acid solution. (The correct answer is 1.45 but I would like to see the work)

ph = ______

b) Trichloroacetic acid, CCl₃COOH, has an acid dissociation constant of 2.0 × 10^-1 at 25 °C. How many times greater is the H₃O⁺concentration in this solution than in a 0.0420 M acetic acid (K_a = 1.8×10^-5)? (The correct answer is 41 but I would like to see the work)