pH of 0.2 mol `L^-1` chloroacetic acid is `1.7`. Find out the degree of dissociation of this chloroacetic acid.

pH of 0.2mol*L^(-1) chloroacetic acid is 1.7. find out the degree of dissociation of this chloroacetic acid.

An aqueous solution of chloroacetic acid of strength 0.2 mol*L^(-1) has pH 1.7. calculate the degree of dissociation of the acid.

The ionisation constant of acetic acid is 1.74xx10^(-5). Calculate the degree of dissociation of acetic acid in its 0.05 (M) solution. Calculate the concentration of acetate ion in the solution and its pH.

In 0.01(M) acetic acid solution, pH = 3.37. What is the degree of ionisation of the acid?

Molar conductivity of "0.025 mol.L"^(-1) methanoic acid is "46 S.cm"^(2)."mol"^(-1) . Calculate its degree of dissociation and dissociation constant. Given : lambda^(@)(HCOO^(-))="54.6 S.cm"^(2)."mol"^(-1), lambda^(@)(H^(+))="349.6 S.cm"^(2)."mol"^(-1) .

Calculate the degree of ionisation of 0.05(M) acetic acid if its pK_(a) value is 4.74. How is the degree of dissociation affected when its solution also contain (1) 0.01(M) in HCl (2) 0.1(M) in HCl?

Determine the pH of 10^(-8) M HCl acid solution. Show that, degree of dissociation of a weak monobasic acid, alpha=1/(1+10^(pk_a-pH)) , where K_a is the dissociation constant of the weak acid at experimental temperature.

The molar conductivities of acetic acid at 298K at the molar concentration of 0.1 is 5.20 S cm^2 mol^(-1) . Calculate the degree of dissociation of acetic acid. Given that lamda_(H^+)^(infty) and lambda_(CH_3COO^-)^(infty) are 349.8 and 40.9 ohm^(-1) cm^2 mol^(-1) respectively.

Concentration of an aqueous solution of weak acid, HA is 0.1 (M) . How many times this acid solution is to be diluted so that the degree of dissociation of HA becomes 2 times that of the initial solution?

The degree of ionisation of a 0.1(M) bromoacetic acid solution is 0.132. calculate the pH of the solution and the pK_(a) of bromoacetic acid.