Calculate pH of a buffer solution that contains 0.1M `NH_(4)OH(K_(b)=10^(-5))` and 0.1 M `NH_(4)Cl.`

What [NH_4^(+) ] in a solution that contains 0.02M NH_3 (K_b =1.8 xx 10^(-5) ) and 0.01 M KOH ?

Calculate pH of a 1.0xx10^(-8) M solution of HCl.

The pH of a buffer solution formed by mixing 30ml of 0.1 M NH_(4) OH and 30ml os 1M NH_(4) Cl solution is 8.6. The pK _(b) of NH-(4) OH is

The pH of a buffer solution made by mixing 25 mL of 0.02 M NH_(4)OH and 25 mL of 0.2 M NH_(4)CI at 25 ^(circ) is ( p^(K_(b)) of NH_(4)OH = 4.8 )

Calculate the pH of a solution which contains 100 ml of 0.1 H HCl and 9.9 ml of 1.0 M NaOH.

pH of an aqueous solution of NH_(4)CI is

Calculate the pH of the solution in which 0.2M NH_(4)Cl and 0.1M NH_(3) are present. The pK_(b) of ammonia solution is 4.75 .

If the pH of a buffer solution containing 0.1 M of monoacidic base and 0.01 M of its salt is 10.5, the pK_(a) of conjugate acid is