Question

Acetic acid, CH₃CO₂H, is the solute that gives vinegar its characteristic odor and sour taste.

Part A: Calculate the pH of 1.16 M CH₃CO₂H.

Part B: Calculate the concentration of H₃O + in 1.16 M CH₃CO₂H

Part C: Calculate the concentration of CH₃CO₂^- in 1.16 M CH₃CO₂H .

Part D: Calculate the concentration of CH₃CO₂H in 1.16 M CH₃CO₂H.

Part E: Calculate the concentration of OH^- in 1.16 M CH₃CO₂H.

Part F: Calculate the pH of 0.0104 M CH₃CO₂H.

Part G: Calculate the concentration of H₃O+ in 0.0104 M CH₃CO₂H

Part H: Calculate the concentration of CH₃CO₂^- in 0.0104 M CH₃CO₂H.

Part I: Calculate the concentration of CH₃CO₂Hin 0.0104 M CH₃CO₂H.

Part J: Calculate the concentration of OH- in 0.0104 M CH₃CO₂H

Answer 1

Part A: Calculate the pH of 1.16 M CH3CO2H.

pH of CH3COOH = 1/2(pka-logC)

    = 1/2(4.74-log1.16)

    = 2.34

Part B: Calculate the concentration of H3O + in 1.16 M CH3CO2H

[h3o+] = 10^-pH

         = 10^-2.34

          = 0.0046 M

Part C: Calculate the concentration of CH3CO2- in 1.16 M CH3CO2H .

   [CH3COO-] = [H3O+] = 0.0046 M

Part D: Calculate the concentration of CH3CO2H in 1.16 M CH3CO2H.

   [ch3cooh] = 1.16-0.0046 = 1.1554 M

Part E: Calculate the concentration of OH- in 1.16 M CH3CO2H.

   [OH-] = 10^-14/(0.0046) = 2.174*10^-12 M

Part F: Calculate the pH of 0.0104 M CH3CO2H.

pH of CH3COOH = 1/2(pka-logC)

    = 1/2(4.74-log0.0104)

    = 3.36

Part G: Calculate the concentration of H3O+ in 0.0104 M CH3CO2H

[h3o+] = 10^-pH

         = 10^-3.36

   = 0.000436 M

Part H: Calculate the concentration of CH3CO2- in 0.0104 M CH3CO2H.

   [CH3COO-] = [h3o+] = 0.000436 M

Part I: Calculate the concentration of CH3CO2Hin 0.0104 M CH3CO2H.

[ch3cooh] = 0.0104-0.000436 = 0.009964 M

Part J: Calculate the concentration of OH- in 0.0104 M CH3CO2H

[OH-] = 10^-14/0.000436

       = 2.3*10^-11 M