Question

The potential of hydrogen electrode at $25^\circ {\text{C}}$ will be: $({{\text{P}}_{{{\text{H}}_2}}} = 1{\text{ atm, concentration of }}{{\text{H}}^ + }{\text{ = 0}}{\text{.1M)}}$
A.) 0.00 V
B.) -0.059 V
C.) 0.118 V
D.) 0.059 V

Answer 1

We know that Nernst equation is used to get the value of electrode potential. It relates, cell potential, temperature, reaction quotient and standard cell potential to each other.

Complete step by step answer:
We have been given the temperature to be ${\text{25}}^\circ {\text{C}}$ i.e. ${\text{25}}^\circ {\text{C + 273 = 298K}}$. Also, ${{\text{P}}_{{{\text{H}}_2}}} = 1{\text{ atm}}$and ${\text{[}}{{\text{H}}^ + }{\text{] = 0}}{\text{.1M}}$.

Reaction occurring on hydrogen electrode is –
${\text{2}}{{\text{H}}^ + }{\text{ + 2}}{{\text{e}}^ - }{\text{ }} \to {\text{ }}{{\text{H}}_2}$.
At ${\text{25}}^\circ {\text{C}}$, Nernst equation is given as - ${{\text{E}}_{{\text{cell }}}}{\text{ = }}{{\text{E}}^0}{\text{ - }}\dfrac{{0.059}}{2}{\text{log}}\dfrac{{{{\text{P}}_{{{\text{H}}_2}}}}}{{[{{\text{H}}^ + }]}}$

Substituting given values in above equation we get,
${{\text{E}}_{{\text{cell }}}}{\text{ = 0 - 0}}{\text{.059 log}}\dfrac{1}{{(0.1)}}$
(standard electrode potential of hydrogen electrode is taken as 0. Hence, ${{\text{E}}^0}{\text{ = 0}}$.)

{{\text{E}}_{{\text{cell }}}}{\text{ = 0}}{\text{-0.059 log {10}}} \\\ {\text{ = - 0}}{\text{.059 V}} \\\ \end{gathered} $$ Hence, the potential of hydrogen electrode at is $${\text{ - 0}}{\text{.059 V}}$$. _**So, option B is correct.**_ **Additional information:** Standard Hydrogen Electrode is used as a reference electrode when calculating the standard electrode potential of a half cell. Platinum metal is generally used to construct hydrogen electrodes. Often to calculate the cell potential of an electrochemical cell at any given temperature, pressure, and reactant concentration Nernst equation is used. The potential difference between the metal and solution is known as electrode potential. It is a measure of tendency of an electrode in a half cell to gain or lose electrons. Whereas, standard electrode potential is the measure of electrode potential at equilibrium conditions. In other words, the electrode potential of a given electrode measured at STP is called a standard electrode potential. It is represented by $${{\text{E}}^0}_{{\text{cell}}}$$. **Note:** At STP, $${\text{Temperature = 298 K}}$$, $${\text{Pressure = 1 atm}}$$ and $${\text{Concentration = 1}}{\text{ M}}$$. Standard hydrogen electrode is used as a reference or a parameter to measure electrode potentials of other metals.