Assume that you want to construct a voltaic cell that uses the...

Question

Assume that you want to construct a voltaic cell that uses the following half-reactions: A2+1aq2 + 2 e- ¡ A1s2 Ered ° = -0.10 V B2+1aq2 + 2 e- ¡ B1s2 E°red = -1.10 V You begin with the incomplete cell pictured here in which the electrodes are immersed in water.

(a) What additions must you make to the cell for it to generate a standard emf?

Diagram of a galvanic cell setup with electrodes C and D, a voltmeter, and a salt bridge.

(a) What additions must you make to the cell for it to generate a standard emf?

Accepted Answer

Identify the half-reactions and their standard reduction potentials: $$A^{2+} + 2e$$^- \rightarrow A (E_{red}^0 = -0.10 V) and $$B^{2+} + 2e$$^- \rightarrow B (E_{red}^0 = -1.10 V).. Determine which half-reaction will occur at the anode and which will occur at the cathode. The half-reaction with the higher reduction potential will occur at the cathode (reduction), and the one with the lower reduction potential will occur at the anode (oxidation).. Assign the electrodes: Electrode C will be the anode (oxidation of B to $$B^{2+}$$), and Electrode D will be the cathode (reduction of $$A^{2+} to A).. $$Add the appropriate solutions to each beaker: Add a solution of $$B^{2+}$$ ions to the beaker with Electrode C and a solution of $$A^{2+}$$ ions to the beaker with Electrode D.. Ensure the salt bridge is properly set up to allow the flow of ions between the two solutions, maintaining electrical neutrality.

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주요 개념

Voltaic Cell

Standard Electrode Potential

Salt Bridge