`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)`)

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.

Calculate the hydrogen ion concentration ( "in mol"//dm^3 ) in a solution containing 0.04 mole of acetic acid and 0.05 mole of sodium acetate in 500 mL of solution.Dissociation constant for acetic acid is 1.75xx10^(-6) Report your answer after multiplying by 2xx10^(6)

Calculate the hydrogen ion concentration ( "in mol"//dm^3 ) in a solution containing 0.04 mole of acetic acid and 0.05 mole of sodium acetate in 500 mL of solution.Dissociation constant for acetic acid is 1.75xx10^(-6) Report your answer after multiplying by 2xx10^(6)

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) :

Calculate the pH of 0.1 (N) acetic acid solution. Given: K_(a) (acetic acid) =1.8xx10^(-5)