In the following question two statements (Assertion) A and...

In the following question two statements (Assertion) A and Reason (R) are given. Mark a. if $\mathrm{A}$ and $\mathrm{R}$ both are correct and $\mathrm{R}$ is the correct explanation of $\mathrm{A}$; b. if $A$ and $R$ both are correct but $R$ is not the correct explanation of A; c. $\mathrm{A}$ is true but $\mathrm{R}$ is false; d. A is false but $\mathrm{R}$ is true, e. A and $R$ both are false. (A): When an aqueous solution of $\mathrm{NaNO}_{3}$ is electrolysed, sodium is liberated at the cathode. $(\mathbf{R}): \mathrm{Na}^{+}$ions are discharged at cathode and $\mathrm{NO}_{3}^{-}$ at the anode.

In the following question two statements (Assertion) A and Reason (R) are given. Mark
a. if $\mathrm{A}$ and $\mathrm{R}$ both are correct and $\mathrm{R}$ is the correct explanation of $\mathrm{A}$;
b. if $A$ and $R$ both are correct but $R$ is not the correct explanation of A;
c. $\mathrm{A}$ is true but $\mathrm{R}$ is false;
d. A is false but $\mathrm{R}$ is true,
e. A and $R$ both are false.
(A): When an aqueous solution of $\mathrm{NaNO}_{3}$ is electrolysed, sodium is liberated at the cathode.
$(\mathbf{R}): \mathrm{Na}^{+}$ions are discharged at cathode and $\mathrm{NO}_{3}^{-}$ at the anode.

Key Concepts

Standard Electrode Potentials

Standard electrode potentials indicate the intrinsic tendency of a chemical species to be reduced or oxidized under standard conditions. They are critical in predicting which species will be preferentially discharged during electrolysis. Differences in these potentials explain why certain ions do not deposit as metals, even if they are present, when water is also available.

Reduction and Oxidation Mechanisms at Electrodes

These mechanisms account for the reactions that occur at the cathode (reduction) and the anode (oxidation) during electrolysis. Understanding these mechanisms is key to predicting the products of electrolysis, as they rely on both the nature of the electrolyte and the reactivity of water, particularly in distinguishing between the direct discharge of ions and the participation of solvent molecules.

Electrolysis of Aqueous Solutions

This concept refers to the process where an electric current is passed through an aqueous ionic solution, causing chemical reactions at the electrodes. In these systems, water itself can participate in the redox reactions, often leading to the production of hydrogen or oxygen gas rather than the deposition or evolution of the constituent ions from the salt.

Discharge Order at Electrodes

Discharge order describes the preferential reduction or oxidation of species present in the solution based on their tendencies measured by standard electrode potentials. In aqueous media, even if metal ions are present, water often undergoes reduction or oxidation first because of its more favorable electrode potentials, guiding which species are actually discharged at the cathode and anode.

Transcript

Please give Ace some feedback