Consider a 0.05 M solution of a week acid. What will be the pH of the acid at 298K? [`K_a = 1.98xx10^-4` at 298K]

pH of a 0.01 M aq. Solution of potassium propanoate is 8 at 298 K. The Ka of propanoic acid at 298 K is

1 ml of 0.1 M aq. solution a weak monoacidic base is diluted to 100 ml. The pH of the resulting solution at 298 K is (Given pK_(b) of the base at 298 K = 5)

1 ml of a 10^(-5) M aq. solution of NaOH is diluted to 1L. The pH of the resulting solution at 298 K is approximately

Calculate the pH of a 0.2M solution of hydrocyanic acid (HCN). Ionisation constant (K_a) of HCN at 298K is 7.2xx10^(-10)

Equilibrium constant of a reaction is 10, what will be the value of Delta G^(@) (in kcal mol^(-1) ) at 298 K?