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.

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)

4g of NaOH was dissolved in one litre of a solution containing one mole of acetic acid and one mole of sodium acetete. Find the pH of the resulting solution ( K_(a) of acetic acid is 1.8xx10^(-3) )

4g of NaOH was dissolved in one litre of a solution containing one mole of acetic acid and one mole of sodium acetete. Find the pH of the resulting solution ( K_(a) of acetic acid is 1.8xx10^(-3) )

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) .

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) :

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

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