A hydrogen electrode placed in a solution containing `CH_(3)COOK` and `CH_(3)COOH` in the ration `a:b` and `b:a` has electrode potential values of `-1.59` and `+1.0V,` respectively. Calculate `pK_(a)` of `CH_(3)COOH.`

A hydrogen electrode placed in a buffer solution of CH_(3)COONa and CH_(3)COOH in the ratios of x:y and y:x has electrode potential values E_(1) volts and E_(2) volts, respectively at 25^(@)C The pK_(a) values of acetic acid is (E_(1) and E_(2) are oxidation potential)

The hydrogen electrode when placed in a buffer solution of CH_3COONa and CH_3COOH in the ratio x:y and y: x has oxidation electrode potential E_ and E_ volts respectively at 25^(@) C (pH_2 =1 atm) . pK_a for CH_3COOH will be :

The hydrogen electrode when placed in a buffer solution of CH_(3)COONa and CH_(3)COOH in the ratio x:y and y:x has oxidation electrode potetnial E_(1) and E_(2) volts respectively at 25^(@)C (P_(H_(2))=1 " atm").pK_(a) for CH_(3)COOH will be

Write an equilibrium equation for a solution containing CH_(3)COOH and CH_(3)COONa . What effect does CH_(3)COONa have on a solution of CH_(3)COOH ?

In a solution containing 0.02M CH_(3)COOH and 0.01M C_(6)H_(5)COOH . If K_(CH_(3)COOH) and K_(C_(6)H_(5)COOH) are 1.8xx10^(-5) and 6.4xx10^(-5) respectively, then calculate the pH of solution.

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?

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?

A solution is 1M in CH_(3)COONa . and 0.1M in CH_(3)COOH . if pK_(a) of CH_(3)COOH is 4.8 , what is the pH of the solution?