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_(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_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

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

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 )

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