The equivalent conductances of two strong electrolytes at infinite dilution in H₂O (where ions move freely through a solution) at 25^oC are given below:
$$ \wedge _{C{H_3}COONa}^o$$ = 91.0 S cm²/equiv
$$ \wedge _{HCl}^o$$ = 426.2 S cm²/equiv
What additional information/quantity one needs to calculate $$ \wedge ^o$$ of an aqueous solution of acetic acid?

The cell, Zn | Zn²⁺ (1M) || Cu²⁺ (1M) | Cu($$E_{cell}^o$$ = 1.10V) was allowed to be completely discharged at 298 K. The relative concentration of Zn²⁺ to Cu²⁺ $$\left[ {{{\left[ {Z{n^{2 + }}} \right]} \over {\left[ {C{u^{2 + }}} \right]}}} \right]$$ is

Given the data at 25^oC,
Ag + I^- $$\to$$ AgI + e^- , E^o = 0.152 V
Ag $$\to$$ Ag⁺ + e^-, E^o = -0.800 V
What is the value of log K_sp for AgI? (2.303 RT/F = 0.059 V)

Resistance of a conductivity cell filled with a solution of an electrolyte of concentration 0.1 M is 100$$\Omega $$. The conductivity of this solution is 1.29 S m^–1. Resistance of the same cell when filled with 0.2 M of the same solution is 520 $$\Omega $$, The molar conductivity of 0.02 M solution of the electrolyte will be