Find the pH of a buffer solution having equal volumes of `0.2MNH_(4)OH and 0.2M NH_(4)Cl (K_(b)` for base `=1.0xx10^(-5)`)

A buffer solution has equal volume of 0.20 M NH_(4)OH and 0.02 MNH_(4)Cl : The pK_(b) of the base is 5. The pH is

A buffer solution has equal volume of 0.20 M NH_(4)OH and 0.02 MNH_(4)Cl : The pK_(b) of the base is 5. The pH is

A buffer solution has equal volumes of 0.2 M NH_(4)OH and 0.02 M NH_(4) CI The pk_(b) of the base is 5. The pH is

The pH of a buffer solution of 0.1 M NH_(4)OH [ pK_(a)=4.0] and 0.1 M NH_(4)Cl is

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) .