Question

The potential of a hydrogen electrode at $pH = 10$ is

• A. $- 0.59\, V$
• B. $0.00\, V$
• C. $0.59\, V$
• D. $-0.059$

Hint:

A reference potential of 0 volts and is used as the basis for measuring the standard electrode potentials of other half-cells.

Answer 1

The Correct Option is A

The correct answer is Option A) \(- 0.59\, V\)

\(H^{+}(p H=10) \mid H_{2}(1\) atm \() \mid P t(s)\)
Reaction : \(2 H^{+}\left(p^{H}=10\right)+2 e^- \rightarrow H_{2}(1\) atm \()\)
\(E=E^{0}-\frac{0.0591}{2} \log \left(\frac{p_{H_{2}}}{\left[H^{+}\right]^{2}}\right)\)
\(=0-\frac{0.0591}{2} \log \frac{1}{\left(10^{-10}\right)^{2}}\)
\(=-\frac{0.0591}{2} \times 2 \log \frac{1}{10^{-10}}\)
\(=-0.0591 \times 10=-0.591\)
i.e. \(E=-0.591\, V\)

Discover More from Chapter: Standard Hydrogen Electrode

Answer 2

The correct answer is Option A) \(- 0.59\, V\)

Real Life Applications

Some real-life examples of the potential of the hydrogen electrode 
1. To measure the pH of a solution. 
2. It can be used to make a number of different electroanalytical measurements, such as the determination of the concentration of an analyte in a solution. 
3. It is used in fuel cells to convert the chemical energy of oxygen and hydrogen into electrical energy. 

Question can also be asked as

1. What is the potential of a hydrogen electrode in a basic solution? 
2. What is the potential of a hydrogen electrode in a pH 10 solution? 
3. How does the potential of a hydrogen electrode change with pH?
4. What is the relationship between pH and the potential of a hydrogen electrode? 

Answer 3

The correct answer is Option A) \(- 0.59\, V\)

A hydrogen electrode is an electrode used in electrochemical measurements to establish a standard reference potential. The standard hydrogen electrode (SHE) is a specific implementation of the hydrogen electrode at standard conditions (1 bar of hydrogen gas, 25 degrees Celsius, and pH 0). It is assigned a reference potential of 0 volts and is used as the basis for measuring the standard electrode potentials of other half-cells.

Working of Standard Hydrogen Electrode

• The half-cell is called anode where the process of oxidation in a Galvanic cell occurs. They have a negative potential.
• The other half-cell is called cathode where reduction takes place. Cathode has a positive potential.
• Between the cathode and anode, a potential difference is created.
• When the switch is ON, then the electrons start to move from the negative electrode to the positive electrodes
• In the Galvanic cell, the current flows from the opposite direction to that of the electron flow.
• The cell potential is the potential difference between the two electrodes (and anode) of a galvanic cell. The unit of cell potential is volts.
• When no current is drawn through the cell, the force applied is called the cell electromotive force.

Related Topics
Hydrogen	Standard Electrode Potential	Electrodes
Cell Potential	Electrochemistry Questions	Reduction Potential