What is the pH of a solution that results when 0.010mol HNO3 is added to 500.ml of a solution that is 0.10M in aqueous ammonia and 0.55 M in ammonium nitrate. assume no volume change. (The Kb for NH3 =1.8 * 10-5 )

Answer : The  

pH of a solution is, 8.56

Explanation : Given,

Concentration of ammonia (base) = 0.10 M

Concentration of ammonium nitrate (salt) = 0.55 M

First we have to calculate the value of .

The expression used for the calculation of is,

Now put the value of in this expression, we get:

Now we have to calculate the pOH of buffer.

Using Henderson Hesselbach equation :

Now put all the given values in this expression, we get:

The pOH of buffer is 5.44

Now we have to calculate the pH of a solution.

Thus, the pH of a solution is, 8.56

its b it was a compound