A)
Ag-------------> Ag+ Cl-
E= 0.222 - 0.059 log(1.29)
E = 0.2154 V
B)
0.266 = 0.222 - 0.059 log(Cl-)
[Cl-] = 0.1795
activity of Cl- = 0.1795
Calculate the cell potential (E) for the half-reaction of a silver-silver chloride reference electrode (E =...
Write the half-reaction for the silver-silver chloride reference electrode. Include physical states. half-reaction: - Write the half-reaction for the saturated calomel reference electrode. Include physical states half-reaction: What is the potential of the cell silver-silver chloride electrode || saturated calomel electrode given that the potential for the AglAgCI electrode in a saturated KCl solution is +0.197 V and the potential for a saturated calomel electrode is +0.241 V? Write the half-reaction for the silver-silver chloride reference electrode. Include physical states....
Write the half-reaction for the silver-silver chloride reference electrode. Include physical states. half-reaction: Write the half-reaction for the saturated calomel reference electrode. Include physical states. half-reaction: What is the potential of the cell silver-silver chloride electrode || saturated calomel electrode given that the potential for the Ag AgCl electrode in a saturated KCl solution is +0.197 V and the potential for a saturated calomel electrode is +0.241 V? E=
1. Write the half‑reaction for the silver-silver chloride reference electrode. Include physical states. 2. Write the half‑reaction for the saturated calomel reference electrode. Include physical states. 3. What is the potential of the cell: silver–silver chloride electrode || saturated calomel electrode given that the potential for the Ag∣∣AgCl electrode in a saturated KCl solution is +0.197 V and the potential for a saturated calomel electrode is +0.241 V?
Convert each of the potentials. The silver-silver chloride and calomel reference electrodes are saturated with KCl, resulting in cell potentials of +0.197 V and +0.241 V with respect to the standard hydrogen electrode (S.H.E.), respectively If an electrode has a potential of 0.695 V with respect to a standard hydrogen electrode (S.H.E.), what is the potential with respect to a silver-silver chloride electrode? E= V If an electrode has a potential of-0.131 V with respect to a silver-silver chloride electrode,...
Convert each of the potentials. The silver–silver chloride and calomel reference electrodes are saturated with KCl, resulting in cell potentials of +0.197 V and +0.241 V with respect to the standard hydrogen electrode (S.H.E.), respectively. If an electrode has a potential of 0.686 V with respect to a standard hydrogen electrode (S.H.E.), what is the potential with respect to a silver–silver chloride electrode? E= If an electrode has a potential of −0.118 V with respect to a silver–silver chloride electrode,...
Convert the following voltages Assume the silver-siIver chloride and calomel reference electrodes are saturated with KCl, giving cell potentials of +0.197 V and +0 241 respective y If an electrode has a potential of 0.337 V with respect to a standard hydrogen electrode (S H E ), what is the potential with respect to a silver-silver chloride electrode? If an electrode has a potential of -0 088 V with respect to a silver-silver chloride electrode, what is the potential with...
Convert each of the potentials. The silver-silver chloride and calomel reference electrodes are saturated with KCl, resulting in cell potentials of +0.197 V and +0.241 V with respect to the standard hydrogen electrode (S.H.E.), respectively. If an electrode has a potential of 0.496 V with respect to a standard hydrogen electrode (S.H.E.), what is the potential with respect to a silver–silver chloride electrode? If an electrode has a potential of −0.147 V with respect to a silver–silver chloride electrode, what...
The half-cell potential of Ag/AgCl reference electrode provides a source of constant potential because: A. junction potential is negligible B. the Ag/AgCl half-reaction contains only solids C. B and C D. the [Ag+] of the filling solution is 0.010 M E. the [Ag+] of the filling solution is 0.010 M
A voltaic cell consists of two half-cells. One half-cell contains a chromium electrode immersed in 1.00 M Cr(NO3)3 solution. The second half-cell contains a cobalt electrode immersed in 1.00 M Co(NO3)2 solution. Cobalt plates out on the cobalt electrode as the voltaic cell runs. The beginning voltage of the cell is +0.467 V at 25°C. The standard electrode potential (standard reduction potential) of chromium at 25°C is −0.744 V. (a) Write a balanced half-reaction equation for the reaction occurring at...
One half-cell in a voltaic cell is constructed from a silver wire electrode in a AgNO3 solution of unknown concentration. The other half-cell consists of a zinc electrode in a 1.9 M solution of Zn(NO3)2. A potential of 1.48 V is measured for this cell. Use this information to calculate the concentration of Ag (aq). E® Zn/Zn2+ = -0.763 V Eº Ag/Ag+ = 0.7994 V Concentration = Submit Answer Try Another Version 6 item attempts remaining