Calculate degree of hydrolysis(h) and pH of solution obtained by dissolving `0.1` moles of `CH_(3)COOHNa` in water to get `100L` of solution .Take `K_(a)` of acetic acid `=2xx10^(-5)` at `25^(@)C`.

Calculate degree of hydrolysis and pH of 0.25 NaCN solution at 25^@C . K_a=4.8xx10^(-10)

What is the pH of a buffer solution prepared by dissolving 0.1 mole of sodium acetate and 0.2 mole of acetic acid in enough water to make a dm^(3) of solution? ( K_(a) of acetic acid = 1.8xx10^(-5) ).

Calculate the degree of hydrolysis of 0.1 M solution of acetate at 298 k. Given : K_a=1.8xx10^(-5)

Calculate the degree of hydrolysis of 0.1 M solution of acetate at 298 k. Given : K_a=1.8xx10^(-5)

Calculate the pH of 0.1 (N) acetic acid solution. Given: K_(a) (acetic acid) =1.8xx10^(-5)

When 0.1 mole of NH_(3) is dissolved in water to make 1.0 L of solution, the [OH^(-)] of solution is 1.30xx10^(-3)M. Calculate K_(b) for NH_(3).

When 0.1 mole of NH_(3) is dissolved in water to make 1.0 L of solution, the [OH^(-)] of solution is 1.30xx10^(-3)M. Calculate K_(b) for NH_(3).

Calculate the pH of a buffer solution containing 0.1 mole of acetic acid and 0.15 mole of sodium acetate. K_(c) for acetic acid is 1.75 xx 10^(-5) .