The standard oxidation potential of $N i / N i^{2 +}$ electrode is $0.236 V$ . If this is combined with a hydrogen electrode in acid solution, at what pH of the solution, will the measured emf be zero at $25^{o} C$ ? Assume $[N i^{2 +}] = 1$ M and pressure of hydrogen is kept at 1 atm.

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Solution

Given,
$E_{N i / N i^{2 +}}^{0} = 0.236 V$
$E_{H^{+} / H_{2}}^{0} = 0, E_{H^{+} / H_{2}} = - 0.236 V, to make E_{c e l l} = 0 So, 2 H^{+} + 2 e^{-} \to H_{2}$ $∴ E_{H^{+} / H_{2}, P t} = 0 - \frac{0.059}{2} l o g \frac{1}{{[H^{+}]}^{2}} = - 0.236$ $we know, p H = l o g \frac{1}{[H^{+}]} = \frac{0.236}{0.059} = 4$

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Similar questions

The standard oxidation potential of $N i | N i^{2 +}$ electrode = 0.236 V. If this is combined with a hydrogen electrode in acid solution, at what pH of the solution will the measured emf be zero at 25 ºC. Assume $[N i^{2 +}]$ = 1M.

Q. The standard oxidation potential of

N i / N i^{2 +} (N i^{2 +} = 1 M)

electrode is

0.236 V

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(P_{H_{2}} = 1 a t m)

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at which the measured e.m.f. of the solution will be zero at

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^{o}

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Q. The standard oxidation potential of

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0.236 V

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Given

[N i^{+ 2}] = 1 M, \frac{R T}{F} = 0.059 V

Q. What is the electrode potential in (in V) of the following electrode at

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The standard oxidation potential of Ni/Ni2+ electrode is 0.236V. If this is combined with a hydrogen electrode in acid solution, at what pH of the solution, will the measured emf be zero at 25oC ? Assume [Ni2+]=1 M and pressure of hydrogen is kept at 1 atm.

Given, E0Ni/Ni2+=0.236 V E0H+/H2=0,EH+/H2=−0.236 V,to make Ecell=0So,2H++2e−→H2∴EH+/H2,Pt=0−0.0592log1[H+]2=−0.236we know, pH=log1[H+]=0.2360.059=4

The standard oxidation potential of $N i / N i^{2 +}$ electrode is $0.236 V$ . If this is combined with a hydrogen electrode in acid solution, at what pH of the solution, will the measured emf be zero at $25^{o} C$ ? Assume $[N i^{2 +}] = 1$ M and pressure of hydrogen is kept at 1 atm.