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Calculate the pH of a buffer that has 0.30 M ammonia and 0.38 M ammonium chloride...

Calculate the pH of a buffer that has 0.30 M ammonia and 0.38 M ammonium chloride before and after 0.04M M nitric acid is added. Write the equilibrium and buffering reactions. Kb(ammonia) = 1.7 x 10 -5

Please show all work thank you!

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Answer #1

POH = Pkb + log[NH4Cl]/[NH3]

Pkb = -logKb

          = -log1.7*10-5

         = 4.769

POH   = 4.769 + log0.38/0.3

             = 4.769 + 0.1026 = 4.8716

PH     = 14-POH

           = 14-4.8716 = 9.1284

by the addition of 0.04 M of HNO3

conc of NH3 = 0.3-0.04 = 0.26M

conc of NH4Cl = 0.38+0.04 = 0.42M

POH = PKb + log[NH4Cl]/[NH3]

        = 4.769+ log0.42/0.26

         = 4.769+0.2089 = 4.9779

PH = 14-POH

        = 14-4.9779 = 9.0221

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