Molar conductivity of a monobasic acid HA having molar concentration equal to $C$ is $\lambda$ and the limiting molar conductivity is ${\lambda }_{\infty }$. The dissociation constant of the acid is

Q. The slope of the graph $\frac{{\Lambda }_v^2}{{\Lambda }_{\infty }({\Lambda }_{\infty }-{\Lambda }_v)}vs.\frac{1}{c}$, if ${\Lambda }_v$ and ${\Lambda }_{\infty }$ are molar conductivity of weak electrolyte having dissociation constant $K_a$ at concentration c and zero respectively is:

Q. Molar conductance of a $0.2$ M solution of a weak acid, $HA$ is $2.8\times {10}^{-2}$ $S{m}^2$ $mo{l}^{-1}$. If the limiting molar conductance of $HA$ is $560$ S $m^2$ $mo{l}^{-1}$, the dissociation constant of the acid is:

Q.

The molar conductivity of 0.025 mol L−1 methanoic acid is

46.1 S cm2 mol⁻¹.

Calculate its degree of dissociation and dissociation constant. Given λ ^°(H⁺)

= 349.6 S cm² mol⁻¹ and λ ^°(HCOO−) = 54.6 S cm² mol

Q. The molar conductivity of $0.009\text{M}$ aqueous solution of a weak acid (HA) is $0.005{\text{S m}}^2{\text{mol}}^{-1}$ and limiting molar conductivity of $HA$ is $0.05{\text{S m}}^2{\text{mol}}^{-1}$ at $298\text{K}$. Assuming activity to be unity, the acid dissociation constant $K_a$ of $HA$ at this temperature is:

Q. Limiting molar conductivity of $N{H}_{4}OH(i.e,{\Lambda }_m^{\circ }(N{H}_{4}OH\left)\right)$ is equal to :