The conductivity of 0.001028 mol `L^(-1)` acetic acid is `4.95 xx 10^-5`S `cm^-1`. Calculate its dissociation constant if `A_m^@` for acetic acid is 390.5 S cm^2 mol^(-1).

Conductivity of 0.00241M acetic acid is 7.896xx10^-5 S cm^-1 . Calculate its molar conductivity and if Lambda^@ for acetic acid is 390.5 S cm^2 mol^-1 . What is its dissociation constant?

Conductivity of 0.00241 M acetic acid is 7.896 x 10^(-5) S cm^(-1). Calculate its molar conductivity. If A°_m for acetic acid is 390.5 S cm^2 mol^(-1) , what is its dissociation constant?

The molar conductivity of 0.025 mol L^-1 methanoic acid is 46.1 S cm^2 mol^-1 . Calculate its degree of dissociation and dissociation constant. Given (H^+) = 349.6 S cm^2 mol^-1 and (HCOO ) = 54.6 S cm^2 mol^(-1).

The conductivity of 0.20 MKCl solution at 298 K is 0.0248 S cm^-1 . Calculate its molar conductivity.

The conductivity of 0.001 mol L^-1 solution of CH_3COOH is 3.905xx10^-5 S cm^-1 . Calculate the molar conductivity and degree of dissociation Give that lambda^@(H^+)=349.65 S cm^2 mol^-1 and lambda^@(CH_2COO^-40.9 S cm^2 mol^-1 .

The conductivity of 0.35M NaCl solution at 298K is 0.025 S/cm. Calculate its molar conductivity .

The conductivity of a saturated solution of AgBr at 25^@C is 8.5xx10^-7 S cm^-1 . If the limiting molar ionic conductance of Ag^+ and Br^- ions are 62 and 78 S cm^2 mol^-1 , then calculate the solubility product of AgBr.

The density of a 2.05 M acetic acid in water is 1.02gcm^-3 . Calculate the molality of the solution.

The freezing point of solution containing 0.2 g of acetic acid in 20.0 g of benzene is lowered by 0.45^(@)C . Calculate the degree of association of acetic acid in benzene. (K_(f)=5.12 K^(@) mol^(-1) kg^(-1))

The density of 2.05 M acetic acid in water is 1.02 g/ml . Calculate the molality of solution.