To calculate the acid dissociation constant Ka of a 0.1 M solution of acetic acid, we can use the following steps:1. Convert the pKa value to Ka:pKa = -log Ka 4.74 = -log Ka Ka = 10^-4.74 Ka 1.8 x 10^-5 2. Calculate the concentration of H+ ions using the given pH value:pH = -log [H+] 3.7 = -log [H+] [H+] = 10^-3.7 [H+] 2.0 x 10^-4 M3. Use the Ka expression to find the concentration of acetate ions A- :Ka = [H+][A-]/[HA]1.8 x 10^-5 = 2.0 x 10^-4 A- / 0.1 - A- 4. Solve for A-:A- 9.0 x 10^-4 M5. Calculate the concentration of undissociated acetic acid HA remaining in the solution:[HA] = 0.1 M - A-[HA] 0.1 - 9.0 x 10^-4 [HA] 0.0991 M6. Verify the Ka value using the calculated concentrations of H+, A-, and HA:Ka = [H+][A-]/[HA]Ka 2.0 x 10^-4 9.0 x 10^-4 / 0.0991 Ka 1.8 x 10^-5 The acid dissociation constant Ka of the 0.1 M solution of acetic acid is approximately 1.8 x 10^-5 .