[" Solution of "0.1NNH_(4)OH" and "0.1N],[NH_(4)Cl" has "pH9.25" ,then find out "],[pK_(b)" of "NH_(4)OH]

Solution of 0.1 N NH_(4)OH and 0.1 N NH_(4)Cl has pH 9.25 , then find out pK_(b) of NH_(4)OH .

Solution of 0.1 N NH_(4)OH and 0.1 N NH_(4)Cl has pH 9.25 , then find out K_(b) of NH_(4)OH .

Solution of 0.1 N NH_4 OH and 0.1 N NH_4CI has pH 9.25 . Then find out pK_b "of" NH_4OH

Solution of 0.1 N NH_4OH and 0.1 NH_4Cl has has pH 9.25 Then pK_b of NH_4OH is

Solution of 0.1 N NH_4 OH and 0.1 N NH_4 Cl "has " P^(H) 9.25 . Then P^(K_b) of NH_4 OH is

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

Calculate pH of the buffer solution containing 0.15 mole of NH_(4)OH " and " 0.25 mole of NH_(4)Cl. K_(b) " for " NH_(4)OH " is " 1.98 xx 10^(-5) .

Calculate pH of the buffer solution containing 0.15 mole of NH_(4)OH " and " 0.25 mole of NH_(4)Cl. K_(b) " for " NH_(4)OH " is " 1.98 xx 10^(-5) .

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