The conductivity of a 0.05 M solution of a weak monobasic acid is `10^(-3) 5 cm^(-1)`, If `lambda_(m)^(oo)` for weak acid `500 5cm^(2) "mol"^(-1)`, calculate Ka of weak monobasic acid :

The conductivity of a 0.05 M solution of a weak monobasic acid is 10^(-3) S cm^(-1) , If lambda_(m)^(oo) for weak acid 500 Scm^(2) "mol"^(-1) , calculate Ka of weak monobasic acid :

At 15^@C 0.05 N solution of a weak monobasic acid is 3.5% ionised. Calculate k_a

Molar conductivity of a 0.01 M solution of a weak monobasic acids HA is 156cm^(2)mol^(-1) at 298 K. What is the pH of this solution if lamda_(m)^(@) of HA 390S cm^(2)mol^(-1)

The pH of 0.1 M solution of weak mono protic acid is 4.0. Calculate its [H^(+)] and Ka .

If the equivalent conductance of (M/20) solution of a weak monobasic acid is 25.0 S cm^2 eq^(-1) and at infinite dilution is 500 Scm^2eq^(-1) , then the dissociation constant of the acid is

The equivalent conductance of M//32 solution of a weak monobasic acid is 6.0 mho cm^(2) eq^(–1) and at infinite dilution is 200 mho cm^(2) eq^(–1) . The dissociation constant of this acid is:

The equivalent conductance of M//32 solution of a weak monobasic acid is 6.0 mho cm^(2) eq^(–1) and at infinite dilution is 200 mho cm^(2) eq^(–1) . The dissociation constant of this acid is:

The pH of a 2 M solution of a weak monobasic acid (HA) is 4. What is the value of the Van’t Hoff factor?