A weak monoprotic acid of 0.1M ,ionizes to 1% in solution.What will be the pH of solution

A weak monobasic acid is 1% ionized in 0.1 M solution at 25^@ C. The percentage of ionization in its 0.025 M solution is :

50 ml of 0.05 M sodium hydroxide is mixed with 50 ml 0.1 of M acetic acid solution. What will be the pH resulting solution if K_(a) (CH_(3)COOH) = 2 xx 10^(-5)

A monoprotic acid in a 0.1 M solution ionizes to 0.001% . Its ionisation constant is

A solution of weak acid HA was titrated with base NaOH. The equivalent point was reached when 40 mL. Of 0.1 M NaOH has been added. Now 20 mL of 0.1 M HCl were added to titrated solution, the pH was found to be 5.0 What will be the pH of the solution obtained by mixing 20 mL of 0.2 M NaOH and 20 mL of 0.2 M HA?

The degree of ionisation of a 0.1 M bromoacetic acid solution is 0.132. Calculate the pH of the solution and the rhoK_a bromoacetic acid.

HA is a weak acid. The pH of 0.1 M HA solution is 2. What is the degree of dissociation (alpha) of HA ?

Upon titrating a solution of weak monoprotic acid with a weak monoacidic base solution at equivalent point:

The equivalent point in a titration of 40.0mL of a sodium of a weak monoprotic acid occurs when 35.0mL of a 0.10M NaOH solutio has been added. The pH of the solution is 5.5 after the addition of 20.0mL of NaOH solution. What is the dissociation constant of the acid ?

Solution of a monobasic acid has a pH=5. If one mL of it is diluted to 1 litre, what will be the pH of the resulting solution ?

calculate [H^(o+)] and [overset(Θ)OH] in a 0.1M solution of weak monoacitic base which is 2.0% ionised. What is the pH of solution.