The Kb of weak base B is 1.0 x 10-6. A solution contains 0.75 M B and 0.25 M HB+Cl- (the salt of B with HCl). What is the pH of the solution after 0.05 mol NaOH is added to 1.0 L of the above solution?

pH of the given solution is 8.7.

Explanation:

For the buffer mixture, initial pOH will be given as follows.

         pOH =

                 =

                 =

                 = 5.523

When 0.05 mol NaOH is added to this buffer solution then concentration of species present will be as follows.

   0.05 mol      0.25           0.75           0

      0              0.20      (0.75 + 0.25)   0.05

Hence, the volume of solution will be 1 liter.

      [BOH] = ,           [Salt] =

So,  pOH = [/tex]

                = 6 - 0.69

                = 5.30

Now, we will calculate the pH as follows.

            pH = 14 - 5.30

                  = 8.7

Thus, we can conclude that pH of the given solution is 8.7.

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