Calculate the `pH` of a buffer by mixing `0.15` mole of `NH_(4)OH` and `0.25` mole of `NH_(4)CI` in a `1000mL` solution `K_(b)` for `NH_(4)OH = 2.0 xx 10^(-5)`

Calculate the pH of a buffer by mixing 0.15 mole of NH_(4)OH and 0.25 mole of NH_(4)Cl in a 1000mL solution K_(b) for NH_(4)OH = 2.0 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) .

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) .

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 buffer solution containing 0.2 mole of NH_4Cl and 0.1 mole of NH_4OH per litre. K_b for NH_4OH=1.85xx10^(-5) .

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

One litre of a buffer solution is prepared by dissolving 0.6 mole. of NH_3 and 0.4 mole of NH_4CI . What is the pH of the solution ? For NH_3K_b = 1.8 xx 10^(-5) . What is the pH of the buffer after addition of 0.1 mole of of HCI ?