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

The pH of a buffer solution containing equal moles of acetic acid and sodium acetate is 4.8. (pK_(a) of acetic acid is 4.8) Statement 2: The ionic product of water at 25^@C is 10^(-14)mol^(2)L^(-2) .

The pH of a buffer solution containing equal moles of acetic acid and sodium acetate is 4.8. (pK_(a) of acetic acid is 4.8) Statement 2: The ionic product of water at 25^@C is 10^(-14)mol^(2)L^(-2) .

Assertion (A): The pH of a buffer solution containing equal moles of acetic acid and sodium acetate is 4.8 ( pK_(a) of acetic acid is 4.8). Reasons (R): The ionic product of water at 25^(circ)C is 10^(-14) mol^(2)L^(-2) . The correct answer is

Calculate the pH of a buffer solution containing 0.1 mole of acetic acid and 0.15 mole of sodium acetate. K_(c) for acetic acid is 1.75 xx 10^(-5) .

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

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.