How much `CH_3COONa` should be added to 1 litre of 0.01 M ` CH_3 COOH` to make . A buffer of pH = 4.1 ?
` (K_a " for " CH_3COOH = 1.8 xx 10 ^(-5))`

The weight of CH_(3)COONa needed to add in 1 litre N/10 CH_(3)COOH to obtain a buffer solution of pH value 4 is ( Given K_(a) = 1.8 xx10^(-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 value of 0.01 M CH_3COOH if it is 5% dissociated.

What amount of solid acetate should be added into 1 litre of the 0.1 M CH_(3)COOH solution so that the resulting solution has pH almost equal to pK_(a) (CH_(3)COOH) = 4.74 .

What will be the value of pH of 0.01 "mol dm"^(-3)CH_(3)COOH(K_(1)=1.74xx10^(-5)) ?

What is [H^(+)] in mol//L of a solution that is 0.20 M in CH_(3)COONa and 0.1 M in CH_(3)COOH ? K_(a) for CH_(3)COOH is 1.8xx10^(-5) ?

The pH of a mixture of 0.01 M HCI and 0.1 M CH_3COOH is approximately

The pH of a solution obtained by mixing 100 ml of 0.2 M CH_3COOH with 100 ml of 0.2 N NaOH will be (pK_a "for " CH_3COOH=4.74 and log 2 =0.301)

Calculate the pH of each of the following solution (i) 100 ml of 0.1 M CH_(3)COOH mixed with 100 ml of 0.1 M NaOH. (ii) 100 ml of 0.1 M CH_(3)COOH mixed with 50 ml of 0.1 m NaOH (iii) 50 ml of 0.1 M CH_(3)COOH mixed with 100 ml of 0.1 M NaOH. K_(a)(CH_(3)COOH)=1.8xx10^(-5)

What is the concentration of CH_(3)COOH which can be added to 0.5M HCOOH solution so that dissociation of both is same. K_(CH_(3)COOH) = 1.8 xx 10^(-5), K_(HCOOH) = 2.4 xx 10^(-4)