1 M solution of `CH_(3)COOH` is diluted to x times so that pH of solution is doubled. Calculate x
Given `K_(a)=1.8xx10^(-5)`

Calculate the change in pH when a 0.1 M solution of CH_3COOH in water at 25^@C is diluted to a final concentration of 0.01 M . [K_a=1.85xx10^(-5)]

What is the pH of 1 M solution of acetic acid ? To what volume one litre of this solution be diluted so that pH of the resulting solution will be twice of the original value ? (K_(a)=1.8xx10^(-5))

What is the pH of 1 M solution of acetic acid ? To what volume one litre of this solution be diluted so that pH of the resulting solution will be twice of the original value ? (K_(a)=1.8xx10^(-5))

To what volume must one litre of 1MC H_3COOH solution be diluted so that the pH of resulting solution becomes twice the original value. [Given: K_a=1.8xx10^-5]

What amount of CH_(3)COONa is to be added to one litre of 0.1(M) CH_(3)COOH solution so that the pH becomes 4.0? [K_(a)=1.8xx10^(-3)] .