Problem: A voltaic cell is constructed with two silver-silver chloride electrodes, each of which is based on the following half-reaction:AgCl(s) + e-  →  Ag(s) + Cl- (aq).The two cell compartments have [Cl- ] = 1.51×10−2 M and [Cl- ] = 2.60 M , respectively.For the cathode compartment, predict whether [Cl- ] will increase, decrease, or stay the same as the cell operates.

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We are asked to determine if the [Cl-] will increase, decrease or stay the same in the cathode department in the voltaic cell given.


We have to determine the anode (oxidation) and cathode (reduction) reactions in the concentration cell.

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Problem Details

A voltaic cell is constructed with two silver-silver chloride electrodes, each of which is based on the following half-reaction:
AgCl(s) + e-  →  Ag(s) + Cl- (aq).
The two cell compartments have [Cl- ] = 1.51×10−2 M and [Cl- ] = 2.60 M , respectively.

For the cathode compartment, predict whether [Cl- ] will increase, decrease, or stay the same as the cell operates.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Nernst Equation concept. You can view video lessons to learn The Nernst Equation. Or if you need more The Nernst Equation practice, you can also practice The Nernst Equation practice problems.

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Based on our data, we think this problem is relevant for Professor Wilson & Tran's class at Saint Louis Community College.