0.2 M solution of `Ba(OH)_2` is found to be 90% ionised at `25^@C`. Find the pH of the solution at that temperature.

An acid of pH 5 is diluted 1000 times. What is the pH of final solution? A 0.05 M solution of acetic acid is found to be 1.9% ionised at 25^@C . Calculate pH of the solution.

0.2 M solution of a weak acid HA is 1 % ionised 25^(@)C . K_(a) for the acid is equal to

Ksp of M(OH)_(2) is 5 xx 10^(-16) at 25^(0)C . The pH of its saturated solution at 25^(0)C is

An acid of pH 5 is diluted 1000 times. What is the pH of final solution? A 0.05 M solution of acetic acid is found to be 1.9% ionised at 25^@C . Calculate K_a of acid.

0.1 molal aqueous solution of an electrolyte AB_(3) is 90% ionised. The boiling point of the solution at 1 atm is ( K_(b(H_(2)O)) = 0.52 kg " mol"^(-1) )

0.1 molal aqueous solution of an electrolyte AB_(3) is 90% ionised. The boiling point of the solution at 1 atm is ( K_(b(H_(2)O)) = 0.52 kg " mol"^(-1) )

At T (K ) , it the ionisation constant of ammonia in solution is 2.5 xx 10^(-5) the pH of 0.01 M ammonia solution and the ionisation constant of its conjugate acid respectively at that temperature are (log 2= 0.30)

A solution was prepared by dissolving 0.0005 mol of Ba(OH)_(2) in 100 mL of the solution. If the base is assumed to ionise completely, the pOH of the solution will be