You are supplied with two acid solutions, one of which contains HCOOH `(pK_b=3.75)` and the other `CH_3COOH(pK_a=4.74)` and their respective salts to prepare a 100 mL buffer solution having pH=4. Which acid and its salt would you choose for the purpose ? Give reason

You are supplied with HCOOH (pK_(a)=3.74), CH_(3)COOH (pK_(a)=4.74) and NaOH solutions. To prepare a buffer solution of pH=3.8, which acid will you select? Give reason.

Then pK_a of a certain weak acid is 4.0. What should be the [salt] ratio if we have to prepare a buffer with pH=5 using the acid and one of the salts?

The ratio of volumes of 0.1(N) CH_3COOH to 0.1(N) CH_3COONa required to prepare a buffer solution of pH 5.74 is (given : pK_a of CH_3COOH is 4.74_-

The ratio of volumes of CH_3COOH 0.1 (N) to CH_3COONa 0.1 (N) required to prepare a buffer solution of pH5.74 is (given: pKa of CH_3COOH is 4.74)

You are asked to prepare a 100 mL buffer solution of pH=5.0. for this purpose, you are supplied with acetic acid (pK_(a)=4.74) , benzoic acid (pK_(a)=4.20) , formic acid (pK_(a)=3.75) and their sodium salts. Which one of the acids will you use to prepare the most effective buffer?

pK_(a) of a weak acid (HA) and p K_(b) of a weak base (BOH) are 3.2 and 3.4 respectively . The pH of their salt (AB) solution is -

Between two solutions of pH 2 and 6 respectively which one is more and how many times more acidic than the other? Define with examples acidic and alkaline buffer.