`HCOOH` and `CH_(3)COOH` solutions have equal `pH.` If `K_(1)//K_(2)` is `4`, the ratio of their molar concentration will be

Both HCOOH and CH_(3)COOH solutions have equal pH. If K_(1) // K_(2) ( ration of acid ionisation constants ) of these acids is 4, their molar concentration ratio will be

A solution is 10 M in CH_(3)COONa and 1 M in CH_(3)COOH . If pK_(a) of CH_(3)COOH is 4.8 , what is the pH of the solution?

At a certain temp, the dissociation constants of HCOOH and CH_(3)COOH are 1.8 times 10^(-4) and 1.8 times 10^(-5) respectively. The molarity of an CH_(3)COOH solution in which H^(+) concentration is the same as in a 0.001 M HCOOH solution is

A solutions is 10 M in CH_(3)COONa and 1 M in CH_(3)COOH . If pK_(a) of CH_(3)COOH is 4.8 , what is the pH of the solution?

Determine the pH of an aqueous 1.0(M) CH_(3)COOH solution. If 1L of this acid solution is diluted with distilled water, then calculate the volume of the dilute solution for a two-fold increase in the pH of the solution? [K_(a)(CH_(3)COOH)=1.8xx10^(-5)] .