What will be the hydrogen ion concentration of a solution obtained by mixing 500ml of 0.2 M acetic acid and 500ml of 0.4 M sodium acetate ? `(K_(a)CH_(3)COOH)=1.8 xx 10^(-5))`

What will be the hydrogen ion concentration of a solution obtained by mixing 500 ml of 0.20 M acetic acid 500 ml of 0.30 M sodium acetate (K_(a) = 1.75 xx 10^(-5))

What will be the hydrogen ion concentration of a solution obtained by mixing 500 ml of 0.20 M acetic acid 500 ml of 0.30 M sodium acetate (K_(a) = 1.75 xx 10^(-5))

Calculate the pH of solution prepared by mixing 40 ml of 0.1 M acetic acid with 40 ml of 0.1 M sodium acetate, Given K_a = 10 ^(-5)

The hydrogen ion concentration and pH of the solution made by mixing 100 mL of 1.0 M HNO_(3) with 100 mL of 0.8 M KOH, are

The hydrogen ion concentration and pH of the solution made by mixing 100 mL of 1.0 m HNO_(3) with 100 mL of 0.8 M KOH, are

Calculate the pH of solution prepared by mixing 50.0 mL of 0.200 M HC_2H_3O_2 and 50.0 mL of 0.100 M NaOH. [Ka(CH_3COOH)=1.8 xx 10^(-5)]

Calculate the concentration of H_3O^+ ions in a mixture of 0.02 M acetic acid and 0.1 M sodium acetate. K_alpha for acetic acid is 1.8 xx 10^(-5) .

Calculate the pH value of 0.15 M solution of acetic acid. K_(CH_3COOH)=1.8xx10^(-5)

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)