Why does the conductivity of a solution decrease with dilution? f

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Electrochemistry

Short Answer Type

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

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2. Can you store copper sulphate solutions in a Zinc pot?

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3. Consult the table of standard electrode potentials and suggest three substance that can oxidize ferrous ions under suitable conditions.

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4. Calculate the potential of hydrogen electrode in contact with a solution whose pH is 10.

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Long Answer Type

5. Calculate the emf of the cell in which the following reaction takes place:
Ni(s) + 2Ag⁺ (0.002 M)

\to

Ni²⁺ (0.160 M) + 2Ag(s)
Given that

{E^{o}}_{Cell} = 1.05 V

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6. The cell in which the following reaction occurs:
2Fe³⁺ (aq) + 2I^–(aq)

\to

2Fe²⁺ (aq) + I₂(s) has E⁰_cell = 0.236 V at 298 K. Calculate the standerd Gibbs energy and the equilibrium constance of the cell reaction.

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Short Answer Type

7. Why does the conductivity of a solution decrease with dilution?

Answer:

The conductivity of a solution is directly proportional to number of ions present in a unit volume of the solution because current is carried forward by the ions. With dilution number of ions in unit volume decreases so that conductivity also decreases. Hence with dilution conductivity decreases.

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

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Long Answer Type

9. 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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Short Answer Type

10. 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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