What is the pH of a solution that is 1.3 M NH3? ( Ka=5.70 x 10^-10...

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What is the pH of a solution that is 1.3 M NH3? ( Ka=5.70 x10^-10 for NH4+).

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4.2 Ratings (739 Votes)

Since Ka*Kb = 10-14

Thus, Kb = 10-14/(5.7*10-10) = 1.75*10-5

The reaction taking place is :

                      NH3 + H2O ----> NH4+ + OH-

Initial                1.3                   0           0

Eqb                1.3-x                  x           x

Thus, Kb = [NH4+]*[OH-]/[NH3] = x*x/(1.3-x) = 1.75*10-5

Solving we get :

x = [OH] = 4.76*10-3 M

Thus, pOH = -log([OH-]) = 2.32

Thus, pH = 14- pOH = 11.68


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