EXERCISE-I (Conceptual Questions)

The molar conductivitites  $\wedge {°}_{\mathrm{NaOAC}}$ and  $\wedge {°}_{\mathrm{HCl}}$ at infinite dilution in water at  $\text{25}°\text{C}$ are 91.0 and 426.2 S  ${\text{cm}}^{\text{2}}/\text{mol}$ respectively. To calculate  $\wedge {°}_{\text{HOAC}},$  the additional value required is –

Given electrode potentials are 

${\mathrm{Fe}}^{3+}+{\mathrm{e}}^{-}\to {\mathrm{Fe}}^{+2};{\mathrm{E}}^0=0.771 \mathrm{V}$

${\mathrm{I}}_2+2{\mathrm{e}}^{-}\to 2{\mathrm{I}}^{-};{\mathrm{E}}^0=0.536 \mathrm{V}$

${\mathrm{E}}_{\mathrm{cell}}^0$ for the reaction

$2{\mathrm{Fe}}^{3+}+2{\mathrm{I}}^{-}\to 2{\mathrm{Fe}}^{2+}+{\mathrm{I}}_2$ is

How much will the reduction potential of a hydrogen electrode change when its solution initially at $\mathrm{pH}=0$ is neutralised to $\mathrm{pH}=7$ ?

Assume that partial pressure of hydrogen gas= 1 atm in the reaction.

Two electrolytic cells, one containing acidified ferrous chloride and another acidified ferric chloride, are connected in series. The ratio of iron deposited at cathodes in the two cells when electricity is passed through the cells will be

When lead storage battery is charged :

Capacity of solvent to neutralise charge on ionic compound is called :-

${\mathrm{Al}}_2{\mathrm{O}}_3$ is reduced by electrolysis at low potentials and high currents. If $4.0\times {10}^4$ amperes of current is passed through molten ${\mathrm{Al}}_2{\mathrm{O}}_3$ for $6$ hours, what mass of aluminum is produced (Assume $100\%$ current efficiency, atomic mass of $\mathrm{Al}=27 \mathrm{g}/\mathrm{mol}$) ?