`0.025 M CH_3COOH` is dissociated 9.5%. Hence the pH of the solution is

A solution contains 0.09 HC1, 0.09 M CHC1_(2)COOH , and 0.1M CH_(3)COOH . The pH of this solution is one. Calculate K_(a) for CHC1_(2)COOH . (Given K_(a)CH_(3)COOH = 10^(-5))

100 ml of 0.2 M CH_3COOH is titrated with 0.2 M NaOH solution. The pH of of the solution at equivalent point will be ( pKa of CH_3COOH=4.76 )

The pH of a 0.1 M CH_(3)COOH which is 2% ionised in aqueous 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?

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 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?

Which of the following solutions when added to 1L of a 0.1 M CH_3COOH or in the pH of the solution K_a=1.8xx10^(-5) for CH_3COOH ?