Ch.19 - Electrochemistry

McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook

McMurry 8th Edition

Ch.19 - Electrochemistry

Problem 55

Chapter 19, Problem 55

What is the function of a salt bridge in a galvanic cell?

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A salt bridge is a crucial component in a galvanic cell, which is an electrochemical cell that generates electrical energy from spontaneous redox reactions.

The primary function of a salt bridge is to maintain electrical neutrality within the internal circuit, preventing the cell from rapidly reaching equilibrium and stopping the flow of electrons.

It does this by allowing the flow of ions between the two half-cells, which balances the charge as electrons move through the external circuit.

Typically, a salt bridge is made of a gel or a porous material soaked in a salt solution, such as KCl or NaNO₃, which does not react with the components of the cell.

By allowing ions to flow, the salt bridge completes the circuit and enables the galvanic cell to continue producing electricity efficiently.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Galvanic Cell

A galvanic cell is an electrochemical cell that converts chemical energy into electrical energy through spontaneous redox reactions. It consists of two half-cells, each containing an electrode and an electrolyte. The flow of electrons from the anode to the cathode generates an electric current, which can be harnessed for work.

Salt Bridge

A salt bridge is a device used in galvanic cells to maintain electrical neutrality by allowing the flow of ions between the two half-cells. It typically contains a gel or solution of a salt that does not react with the cell components. By facilitating ion movement, the salt bridge prevents charge buildup that would otherwise halt the reaction.

Electrolyte

An electrolyte is a substance that dissociates into ions when dissolved in a solvent, allowing it to conduct electricity. In galvanic cells, electrolytes are crucial as they provide the medium for ion exchange between the anode and cathode. The choice of electrolyte can affect the cell's voltage and overall efficiency.

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Related Practice

Textbook Question

An H₂/H⁺ half-cell (anode) and an Ag⁺/Ag half cell (cathode) are connected by a wire and a salt bridge. (b) Write balanced equations for the electrode and overall cell reactions.

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Textbook Question

An H₂/H⁺ half-cell (anode) and an Ag⁺/Ag half cell (cathode) are connected by a wire and a salt bridge. (a) Sketch the cell, indicating the direction of electron and ion flow.

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Textbook Question

Write balanced net ionic equations for the following reactions in basic solution. (c)

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Textbook Question

Write the shorthand notation for a galvanic cell that uses the following cell reaction. Include inert electrodes if necessary.2 Fe1s2 + Cr2O72-1aq2 + 14 H+1aq2¡2 Fe3+1aq2 + 2 Cr3+1aq2 + 7 H2O1l2

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Textbook Question

Write balanced net ionic equations for the following reactions in basic solution. (b)