Calculate the pH of `0.05M` sodium acetate solution, if the `pK_(a)` of acetic acid is `4.74`.

pH of 0.05(M) calcium acetate solution (pK_a=4.74) is -

Determine the pH of 0.1 M acetic acid solution . ( pK_(a) of acetic acid is 4.75) Is there any OH^(-) ion present in this solution of acetic acid ? Answer with reason .

What will be the pH of 0.1 M ammonium acetate solution ? pK_a=pK_b=4.74

When 0.2M solution of acetic acid is neutralised with 0.2M NaOH in 500 mL of water, the pH of the resulting solution will be: [pK_(a) of acetic acid = 4.74]

When 0.2M solution of acetic acid is neutralised with 0.2M NaOH in 500 mL of water, the pH of the resulting solution will be: [pK_(a) of acetic acid = 4.74]

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)

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 )

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 )-