In a voltaic cell, a salt bridge is needed to allow the motion of choose. Between the terminals. In the salt bridge, choose. Move toward the anode and choose. Move toward the cathode.

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21-07-2022
Biology

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In a voltaic cell, a salt bridge is needed to allow the motion of choose. Between the terminals. In the salt bridge, choose. Move toward the anode and choose. Move toward the cathode.

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Tutorconsortium330 Tutorconsortium330 · Answer 1 · 2022-08-02T19:28:05+02:00

In a voltaic cell, a salt bridge is needed to allow the motion of ions between the terminals. In the salt bridge, anions move toward the anode and cations move toward the cathode.

What is a voltaic cell?

A voltaic cell is an electrochemical device that harnesses the power of a chemical process to generate electrical energy. A voltaic cell's key components are:

Anode, an electrode where oxidation takes place. Anions move toward the anode.
Cathode, an electrode where reduction takes place. Cations move toward the cathode.
A salt bridge is an electrolyte chamber required to finish the circuit in a voltaic cell.
Half-cells are containers that serve as a barrier between the oxidation and reduction reactions.
The external circuit, which typically has a load attached to it, is used to carry electron flow between the voltaic cell's electrodes.
A load is a component of a circuit that uses an electron flow to carry out a certain task.

Working of a voltaic cell:

When an electrode is dipped into the electrolyte at the electrode and electrolyte contact surface in a voltaic cell, the electrode's atoms tend to produce positive ions in the electrolytic solution while leaving the electrode's electrons unaffected. The electrode thus acquires a negative charge.

Additionally, the electrolytic solution's positive ions have a propensity to deposit on the electrode, giving it a positive charge. The electrodes get positively or negatively charged in relation to the electrolyte as a result of the two opposite processes. As a result, there is a potential difference between the electrode and electrolyte. The term "electrode potential" refers to this potential difference.

Now, the electrode where reduction occurs is known as the cathode and turns positive in relation to the electrolytic solution, whereas the electrode where oxidation occurs is known as the anode and has a negative potential in relation to the electrolytic solution. This caused a potential difference to form between the voltaic cell's two electrodes. Cell Potential is the name given to this potential differential.

The voltaic cell's potential is sometimes referred to as its electromotive force (EMF) when no current is being drawn from it. Electrons begin to flow from the anode (negative electrode) to the cathode (positive electrode) when an external circuit is connected to the voltaic cell. As a result, in the external circuit, the normal current flows from the positive terminal to the negative terminal.

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