The pH of a solution containing 0.1 M `CH_3COONa and 0.1 M (C_2H_5COO)_2` Ba will be `K_a(CH_3COOH)=2xx10^(-5). K_a(C_2H_5COOH)=1.5xx10^(-5)`:

Calculate the pH of a solution containing 0.1 M CH_(3)COOH and 0.15 M CH_(3)COO^(-) . (K_(a) "of" CH_(3)COOH=1.8xx10^(-5))

Calculate the pH of a solution containing 0.1 M CH_(3)COOH and 0.15 M CH_(3)COO^(-) . (K_(a) "of" CH_(3)COOH=1.8xx10^(-5))

The pH of solution, containing 0.1N HCl and 0.1N CH_(3)COOH(K_(a)=2xx10^(-5)) is

The pH of solution, containing 0.1N HCl and 0.1N CH_(3)COOH(K_(a)=2xx10^(-5)) is

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.

Determine the pH of a buffer solution consisting of 0.01(M) CH_(3)COOH and 0.03(M)" "CH_(3)COONa. Given: K_(a)(CH_(3)COOH)=1.8xx10^(-5) .

calculate the pH of a solution which is 0.1 m in CH_3COOH and .5 M in CH_3COONa . k_a for CH_3COOH is 1.8xx10^-6 .

Calcualte the pH of solution when 100 mL, 0.1 M CH_(3)COOH and 100 mL, 0.1 M HCOOH are mixed together. ("Given : "K_(a)(CH_(3)COOH)=2xx10^(-5)), K_(a)(HCOOH)=6xx10^(-5)