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))`

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) .

The pH of a buffer solution of 0.1 M CH_(3)COOH and 0.01 M CH_(3)COONa is (pK_(a)(CH_(3)COOH)=4.745) :

write the Henderson-Hasslbalch equation for an acidic buffer, calculate the pH of an acidic buffer containing 0.1M CH_3COOH and 0.5M CH_3COONa[Ka for CH_3COOH is 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

The pH of a buffer solution of 0.1 M CH_(3)COOH and 0.1 MCH_(3)COONa is (pK_(a)CH_(3)COOH =4.745)

The pH of a solution resulting from the addition of 12.5mL of 0.1M HCl to 50mL of a solution containing 0.15M CH_(3)COOH & 0.2M CH_(3)COONa will be (Given : pK_(a) of CH_(3)COOH=4.74 )