[" The ionization constant of a mono basic "],[" acid is "5times10^(-2)" .The "pH" of "0.01M" acid "],[" solution is "]

The ionisatioln constant of a mono basic acid is 5 xx 10^(-2) . The pH of 0.01 M acid solution is

The dissociation constant of a monobasic acid is 1.0xx10^(-9) . The pH of its 0.1 M aqueus solution is:

The dissociation constant of a weak monobasic acid K_a is 1 xx 10^-5 . The pH of 0.1 M of that acid would be

The dissociation constant of a weak monobasic acid K_(a) is 1xx 10^(-5) . The pH of 0.1 M of that acid would be

The dissociation constant of a substituted benzoic acid at 25^(@)C is 1.0 xx 10^(-4) . The pH of 0.01M solution of its salt is :

If the ionization constant of hypochlorous acid (HOCl) is 2.5xx10^(-5) , the pH of 1.0 M of its solution is (log5=0.7)

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)

The ionization constant of chloroacetic acid is 1.35xx10^(-3) . What will be the pH of 0.1 M acid and its 0.1M sodium salt solution?

The ionization constant of chloroacetic acid is 1.35xx10^(-3) . What will be the pH of 0.1 M acid and its 0.1M sodium salt solution?