Question

The potential of hydrogen electrode is $- 118.5mV.$ The ${H^ + }$ concentration of the solution is:
A. $0.01M$
B. $2M$
C. ${10^{^{ - 4}}}M$
D. $1M$

Answer 1

The basis of the thermodynamics of oxidation reduction potential is formed by a Redox electrode which is the standard hydrogen electrode . it can be used to compare the potential of any other electrodes at the same temperature as that of the standard hydrogen electrode.

Formula used:
{E_{cell}} = \dfrac{{0.0591}}{n}\log \left\\{ {{H^ + }} \right\\}

Complete step by step answer:
Given $E = 118.5mV = 118.5 \times {10^{ - 3}}$
We will determine this with the help of Nernst equation.
Nernst equation is the relationship between electrode potential, cell potential and the concentration of reacting species
We know that,
{E_{cell}} = \dfrac{{0.0591}}{n}\log \left\\{ {{H^ + }} \right\\}
Here,
$n = 1$ , number of electrons involved in the reaction
On substituting the value of electrode potential of hydrogen electrode
So, \log \left\\{ {{H^ + }} \right\\} = \dfrac{{ - 118.5 \times {{10}^{ - 3}}}}{{0.0591}}
$\Rightarrow$ \log \left\\{ {{H^ + }} \right\\} = - 2.0051
$\Rightarrow$ \left\\{ {{H^ + }} \right\\} = 0.001M
Hence from the above calculations we find out that the concentration of hydronium ions in the solution is \left\\{ {{H^ + }} \right\\} = 0.001M
Hence, the correct answer is (A).

Additional Information: Hydrogen electrode is based on the redox half cell
$2{H_{aq}}^ + + 2{e^ - } \to {H_2}\;(g)$
The standard hydrogen electrode consists of a platinised platinum electrode dipped in 1 molar solution of hydronium ions and pure hydrogen gas maintained at a pressure of 1 atmosphere is bubbled through the solution containing platinised platinum electrode . It can act as Both anode and cathode because it is a half reaction cell . Its electrode potential is zero.

Note: Its absolute electrode potential is estimated to be $4.44 \pm 0.02V\;a + {25^ \circ }C$ , but to form a basis for comparison with all other electrode reactions, hydrogen is standard electrode potential $\left( {{E^ \circ }} \right)$ is declared to be Zero Volts at any temperature. In Nernst equation , the term involving log is the same as the expression for equilibrium constant when there is a minus sign between the two terms on the right hand side .