What would be the `pH` of `0.1` molar sodium acetate solution. Given that the dissociation constant of acetic acid is `1.8xx10^(-5)`? `(log1.8=0.26)`

The molar conductivity of acetic acid solution at infinite dilution is 390.7 Omega^(-1)cm^(2)mol^(-1) . Calculate the molar conductivity of 0.01M acetic acid solution, given that the dissociation of acetic acid is 1.8xx10^(-5) .

Calculate t the H^(+) ion concentration in 0.10 M acetic acid solution. Given that the dissociation constant of acetic acid in water is 1.8xx10^(-5)

Calculate the H^+ ion concentration in 0.10 M acetic acid solution- Given that the dissociation constant of acetic acid in water is 1.8 xx 10^(-6) .

Calculate the pH of 0.01 M Solution of CH_3 COOH . The dissociation constant of the acid is 1.8 xx 10 ^(-5)

Calculate the degree of ionisation and [H_3O^(+) ] of a 0.15 M CH_3COOH solution. The dissociation constant of acetic acid is 1.8 xx 10^(-5)

Calculate the pH of 0.05M sodium acetate solution, if the pK_(a) of acetic acid is 4.74 .

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)

Acetic acid gets 1.3% ionised in its decimolar solution.What is be the ionisation constant of acetic acid?

Calculate the pH of 0.10 M solution of NH_4CI . The dissociation constant (K_b) "of" NH_3 "is" 1.8 xx 10^(-5) .

Calculate the concentration of H_3O^(+) in a mixture of 0.03 M acetic acid and 0.1 M sodium acetate. Ionisation constant for acetic acid is 1.8 xx 10^(-5)