100ml of 0.75 N `NH_(4)OH` is mixed with 100ml of 0.25 N HCl. The `K_(b)` of `NH_(4) OH = 2 xx 10^(-5)` . Hence pH of solution is .

A solution is prepared by mixing 100 ml of 0.1 M NH_(4) OH and 200 ml of 0.2 M NH_(4) Cl . pK_(b) of NH_(4) OH is 4.8 . Then the pH of the solution is

100 ml of 0.15 M HCl is mixed with 100 ml of 0.05 M HCl, is the pH of the resulting solution?

A solution consist of 0.2 M NH_(4)OH and 0.2 M NH_(4)Cl . If K_(b) of NH_(4)OH is 1.8 xx 10^(-5) , the [OH^(-)] of the resulting is

5 mL of 0.4 N NaOH is mixed with 20 mL of 0.1 N HCl. The pH of the resulting solution will be

5 mL of 0.4 N NaOH is mixed with 20 mL of 0.1 N HCl The pH of the resulting solution will be

5 mL of 0.4N NaOH is mixed with 20 mL of 0.1N HCl. The pH of the resulting solution will be :

A solution consists of 0.2 M NH_4 OH and 0.2 M NH_4Cl . If K_b of NH_4 OH is 1. 8 xx 10 ^(-5) , the [OH^(-) ] of the resulting solution is

K_(b) for NH_(4)OH is 1.81xx10^(-5) . The pH of 0.01 M NH_(4)Cl solution at 25^(@)C is :