On passing $0.1 \ F$ of electricity through aluminium chloride,the amount of aluminium metal deposited on the cathode is $(Al = 27)$ ............ $g$.

How much charge is required for the deposition of $1$ equivalent of a substance?

Three faradays of electricity are passed through molten $Al_2O_3$,aqueous solution of $CuSO_4$ and molten $NaCl$ taken in different electrolytic cells. The amount of $Al$,$Cu$ and $Na$ deposited at the cathodes will be in the ratio of

One Faraday of electricity when passed through a solution of copper sulphate deposits:

In an experiment,$0.04 \ F$ was passed through $400 \ mL$ of a $1 \ M$ solution of $NaCl$. What would be the $pH$ of the solution after the electrolysis? (Change in volume will be negligible)

On passing $3 \ A$ of electricity for $50 \ minutes$,$1.8 \ g$ of metal deposits. The equivalent mass of the metal is: