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Standard X

Chemistry

Electrolysis and Electrolytes

The passage o...

Question

The passage of current through a solution of certain electrolyte results in the evolution of $H_{2}$ at cathode and $C l_{2}$ at anode. What could be the solution?

Water

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H_{2} S O_{4}

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Aqueous

N a C l

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Aqueous

C u C l_{2}

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Solution

The correct option is A Aqueous $N a C l$
The reduction potential of $H^{+} > N a^{+}$
$∴ H^{+}$ gets reduced.
Reduction potential of $C l^{-} < O H^{-}$
i.e. oxidation potential of $C l^{-} > O H^{-}$
$∴ C l^{-}$ gets oxidised at the anode

Hence, option $C$ is correct.

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Similar questions

The passage of current through a solution of certain electrolyte results in the formation of hydrogen at cathode and chlorine at anode. The solution is:

Q. The passage of current liberates

H_{2}

at cathode and

C l_{2}

at anode. The solution is_______________.

Q. Assertion :The electrolysis of NaCl solution gives

H_{2}

(g) at cathode and

C l_{2}

(g) at anode. Reason:

C l_{2}

has higher oxidation potential than

H_{2} O

Q. An aqueous solution of NaCl on electrolysis gives

H_{2}

(g),

C l_{2}

(g) and NaOH according to reaction,

2 C l^{-} (a q) + 2 H_{2} O \to 2 O H^{-} (a q) + H_{2} (g) + C l_{2} (g)

A direct current of 25 ampere with a current efficiency of 62% is passed through 20 litre of NaCl solution (20% by mass) Write down the reactions taking place at the electrodes.
The redox changes are : Cathode:

2 C l^{-} \to C l_{2} + 2 e

Anode :

2 e + 2 H_{2} O \to 2 O H^{-} + H_{2}

Which of the following statements are correct?

a) The electrolysis of aqueous NaCl produces hydrogen gas at the cathode and chlorine gas at the anode .

b) The electrolysis of a $C u S O_{4}$ solution using Pt electrodes causes the liberation of $O_{2}$ at the anode and the deposition of copper at the cathode .

c) Oxygen and hydrogen are produced at the anode and cathode during the electrolysis of dilute aqueous solution of $H_{2} S O_{4}$ .

d) All electrolytic reactions are redox reactions .

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The passage of current through a solution of certain electrolyte results in the evolution of H2 at cathode and Cl2 at anode. What could be the solution?

The correct option is A Aqueous NaClThe reduction potential of H+>Na+∴H+ gets reduced.Reduction potential of Cl−<OH−i.e. oxidation potential of Cl−>OH−∴Cl− gets oxidised at the anodeHence, option C is correct.

The passage of current through a solution of certain electrolyte results in the evolution of $H_{2}$ at cathode and $C l_{2}$ at anode. What could be the solution?

The correct option is A Aqueous $N a C l$
The reduction potential of $H^{+} > N a^{+}$
$∴ H^{+}$ gets reduced.
Reduction potential of $C l^{-} < O H^{-}$
i.e. oxidation potential of $C l^{-} > O H^{-}$
$∴ C l^{-}$ gets oxidised at the anode

Hence, option $C$ is correct.