A buffer solution is made up of acetic acid `[pK_(a)=5]` having conc.=1.5M and sodium acetate having conc.=0.15 M. What is the number `OH^(-)` ions present in 1 litre solution?

A buffer solution contains 0.1 M of acetic acid and 0.1 M of sodium acetate. What will be its pH ? ( pK_(a) of acetic acid is 4.75)

The pH of buffer solution containing 4 xx 10^(-3) and 0.4 mole of acetic acid (pK_(a) = 4.76) and sodium acetate respectively will be

A buffer solution is prepared by mixing 10 mL of 1.0 M acetic acid and 20 mL of 0.5 M sodium acetate and then diluted to 100 mL with distilled water, The pH of the buffer solution is ( pK_(a) of acetic acid is 4.76 )

The pH of a buffer solution containing 0.1M acetic acid and 0.1 M sodium acetate (pKa of a acetic acid is 4.74) is

A buffer solution contains 0.1 M each of acetic acid and sodium acetate. The pH of the buffer solution is (pK_(a)(CH_(3)COOH)=4.75) :

1xx10^(-3) mol of HCl is added to a buffer solution made up of 0.01 (M) acetic acid and 0.01(M) sodium acetate. The final pH of the buffer will be ( pK_(a) of acetic acid is 4.75 at 25^(@)C )-

1xx10^(-3) mole of HCl is added to a buffer solution made up of 0.01 M acetic acid and 0.01 M sodium acetate. The final pH of the buffer will be (given, pK_a of acetic acid is 4.75 at 25^@ C)

One litre of buffer solution contains 0.1 mole of acetic acid add 1 mole of sodium acetate. Find its pH if pK_(a) of CH_(3)COOH is 4.8.