OH – From the pH we can calculate the hydrogen ion concentration. Knowing hydrogen ion concentration and the ionic product of water we can calculate the concentration of hydroxyl ions. Thus we have: [H + ] = antilog (–pH) = antilog (– . ) = .
× – [OH – ] = K w / [H + ] = × – / . × – = . × – The concentration of the corresponding hydrazinium ion is also the same as that of hydroxyl ion. The concentration of both these ions is very small so the concentration of the undissociated base can be taken equal to .004M.
Thus, K b = [NH NH + ][OH – ] / [NH NH ] = ( . × – ) / . = . × – p K b = –log K b = –log( .
× – ) = . . Problem . Calculate the pH of the solution in which .2M NH Cl and .1M NH are present.
The pK b of ammonia solution is . . NH + H O NH + + OH – The ionization constant of NH , K b = antilog (–p K b ) i.e. K b = – .
= . × – M NH + H O NH + + OH – Initial concentration (M) . . Change to reach equilibrium (M) –x +x +x At equilibrium (M) .
– x . + x x K b = [NH + ][OH – ] / [NH ] = ( . + x)(x) / ( . – x) = .
× – As K b is small, we can neglect x in comparison to .1M and .2M. Thus, [OH – ] = x = . × – Therefore, [H + ] = . × – pH = – log[H + ] = .
. . . Relation between K a and K b As seen earlier in this chapter, K a and K b represent the strength