The hydrogen electrode is dipped in a solution of pH=3 at 25^∘ C. The potential of the cell woul

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The hydrogen electrode is dipped in a solution of pH=3 at...

The hydrogen electrode is dipped in a solution of $\mathrm{pH}=3$ at $25^{\circ} \mathrm{C}$. The potential of the cell would be (value of $2.303 \mathrm{RT} / \mathrm{F}$ is $0.059 \mathrm{~V}$ ) a. $+1.77 \mathrm{~V}$ b. $+0.177 \mathrm{~V}$ c. $-0.87 \mathrm{~V}$ d. $-0.177 \mathrm{~V}$

The hydrogen electrode is dipped in a solution of $\mathrm{pH}=3$ at $25^{\circ} \mathrm{C}$. The potential of the cell would be (value of $2.303 \mathrm{RT} / \mathrm{F}$ is $0.059 \mathrm{~V}$ )
a. $+1.77 \mathrm{~V}$
b. $+0.177 \mathrm{~V}$
c. $-0.87 \mathrm{~V}$
d. $-0.177 \mathrm{~V}$

Key Concepts

Electrode Potential

Electrode potential is the voltage associated with a specific electrode in an electrochemical cell. It is determined by both the intrinsic properties of the electrode reaction and the conditions of the system, such as ion concentration and temperature. Understanding electrode potential is critical for analyzing and predicting the behavior of galvanic and electrolytic cells.

Standard Hydrogen Electrode

The standard hydrogen electrode (SHE) is a reference electrode based on the half-cell reaction involving hydrogen gas and hydrogen ions. It is assigned a potential of zero volts under standard conditions, and it serves as the baseline for measuring the electrode potentials of other half-cells, making it essential in electrochemistry.

Nernst Equation

The Nernst equation relates the electrode potential of a half-cell to the standard electrode potential, temperature, number of electrons transferred, and the reaction quotient. It allows for the calculation of electrode potentials under non-standard conditions by incorporating the activities (or concentrations) of the reactants and products involved in the redox reaction.

pH and Hydrogen Ion Concentration

pH is a measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration. In electrochemical cells involving hydrogen electrodes, the pH directly influences the concentration of H+ ions in solution, which in turn affects the electrode potential as described by the Nernst equation.

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