A solution of `0.1M NaZ` has `pH = 8.90`. The `K_(a)` of `HZ` is

A solution of 0.1 M NaZ has PH = 8.90 . The K_a of HZ is.

0.01M solution of H_(2)A has pH equal to 4. If k_(a1) for the acid is 4.45 xx 10^(-7) , the concentration of HA^(-) ion in solution would be

The freezing point of 0.20M solution of weak acid HA is 272.5K . The molality of the solution is 0.263mol Kg^(-1) . Find the pH of the solution on adding 0.20M solution of NaOH . Given: K_(f) of water = 1.86 Km^(-1)

The freezing point of 0.20 M solution of week acid HA is 272.5 K . The molality of the solution is 0.263 "mol" kg^(-1) . Find the pH of the solution on adding 0.25 M sodium acetate solution. K_(f) of water = 1.86 K m^(-1)

The freezing point of 0.20 M solution of week acid HA is 272.5 K . The molality of the solution is 0.263 "mol" kg^(-1) . Find the pH of the solution on adding 0.25 M sodium acetate solution. K_(f) of water = 1.86 K m^(-1)

The freezing point of 0.20 M solution of week acid HA is 272.5 K . The molality of the solution is 0.263 "mol" kg^(-1) . Find the pH of the solution on adding 0.25 M sodium acetate solution. K_(f) of water = 1.86 K m^(-1)

Calculate pH of resultant solution of 0.1 M HA + 0.1 M HB [K_a (HA) =2 xx 10^(-5), K_a (HB)=4 xx 10^(-5)]

The pH of 0.05M aqueous solution of diethy 1 amine is 12.0 . Caluclate K_(b) .

The pH of 0.05M aqueous solution of diethy 1 amine is 12.0 . Caluclate K_(b) .