Answer:
A salt bridge is an essential component of a voltaic cell in maintaining the electrical neutrality of the cell and facilitating the flow of ions. When a voltaic cell operates, the oxidation and reduction reactions occur in separate half-cells. These cells are physically separated from each other to prevent the direct transfer of electrons between them. Instead, the electrons flow through an external circuit, creating an electric current.
During this process, the reduction half-cell accumulates negative charge, while the oxidation half-cell accumulates positive charge. Without a salt bridge, this accumulation of charge would eventually lead to a buildup of electrostatic repulsion. This would stop the flow of electrons and prevent the cell from functioning.
The salt bridge prevents this by providing a pathway for the flow of ions between the two half-cells. Specifically, it contains a solution of an electrolyte, a substance that dissociates into ions when dissolved in water. The positively charged ions from the electrolyte move into the reduction half-cell to neutralize the accumulating negative charge. On the other hand, the negatively charged ions move into the oxidation half-cell to neutralize the accumulating positive charge. This flow of ions ensures that the cell remains electrically neutral and allows the cell to continue operating.
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Therefore, the salt bridge helps maintain the electrochemical balance of the cell. It also facilitates the flow of ions necessary for the generation of electrical energy.
Step-by-step explanation: