Electrochemistry

Question

The potential of a hydrogen electrode in a solution of unknown [H⁺] is 0.29 V at 298 k measured against a standard hydrogen electrode. Calculate the pH of the solution.

Solution

The both electrode are same thus there

E_{cell}^{0}

=0
Since the potential of the hydrogen electrode measured against standard hydrogen electrode is a positive value, the electrode is acting as the anode. If the unknown [H⁺] be x, the Nernst equation takes the form

E_{cell} = E °_{cell} - \frac{0.0592}{2} \log \frac{x^{2}}{1^{2}}

Since both electrodes are the same,

E °_{cell} = 0 .

∴

0.29 V = 0 - \frac{0.0592 V}{2} \times 2 \log x

0.29 V = - 0.0592 V \times \log x

Since

- logx = - \log [H^{+}] = pH

0.029 V = 0.0592 V \times pH

pH = \frac{0.29}{0.0592} = 4.9 .

Some More Questions From Electrochemistry Chapter

How would you determine the standard electrode potential of the system Mg²⁺/Mg?

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The molar conductivity of 0.025 mol L^–1methanoic acid is 46.1 S cm² mol^–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H⁺) = 349.6 S cm²mol^–1 and λ° (HCOO^– ) = 54.6 s cm² mol^–1.

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Electrochemistry

The potential of a hydrogen electrode in a solution of unknown [H⁺] is 0.29 V at 298 k measured against a standard hydrogen electrode. Calculate the pH of the solution.

Some More Questions From Electrochemistry Chapter

How would you determine the standard electrode potential of the system Mg²⁺/Mg?

Can you store copper sulphate solutions in a Zinc pot?

Why does the conductivity of a solution decrease with dilution?

Suggest a way to determine the Λ°_m value of water.

The molar conductivity of 0.025 mol L^–1methanoic acid is 46.1 S cm² mol^–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H⁺) = 349.6 S cm²mol^–1 and λ° (HCOO^– ) = 54.6 s cm² mol^–1.

If the current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons flow through the wire?

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For Daily Free Study Material Join wiredfaculty

Electrochemistry

The potential of a hydrogen electrode in a solution of unknown [H+] is 0.29 V at 298 k measured against a standard hydrogen electrode. Calculate the pH of the solution.

Some More Questions From Electrochemistry Chapter

How would you determine the standard electrode potential of the system Mg2+/Mg?

Can you store copper sulphate solutions in a Zinc pot?

Why does the conductivity of a solution decrease with dilution?

Suggest a way to determine the Λ°m value of water.

The molar conductivity of 0.025 mol L–1 methanoic acid is 46.1 S cm2 mol–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H+) = 349.6 S cm2 mol–1 and λ° (HCOO– ) = 54.6 s cm2 mol–1.

If the current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons flow through the wire?

Mock Test Series

NCERT Sample Papers

Entrance Exams Preparation

The potential of a hydrogen electrode in a solution of unknown [H⁺] is 0.29 V at 298 k measured against a standard hydrogen electrode. Calculate the pH of the solution.

How would you determine the standard electrode potential of the system Mg²⁺/Mg?

Suggest a way to determine the Λ°_m value of water.

The molar conductivity of 0.025 mol L^–1methanoic acid is 46.1 S cm² mol^–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H⁺) = 349.6 S cm²mol^–1 and λ° (HCOO^– ) = 54.6 s cm² mol^–1.