A silver-silver bromide wire is sometimes used as a reference electrode when Cl- -free conditions must be maintained. Write the cell notation and calculate the potential (at 30°C) of an Ag/AgBr reference electrode if it is immersed in a 3.5M solution of KBr. (Use concentrations, not activities in your calculation.)
The half cell notation for the Ag/AgBr electrode is
Br-(3.5M)/AgBr(s)/Ag(s)
Cell potential can be calculated using Nernst equation
E= E0-2.303RT{log[(Red)/(Oxd)]}/nF,
E= E0-2.303RT{log[Br-]}/nF
R = 8.314 j/K, T = 273+30 = 303K, n = 1 for Ag/AgBr electrode, F = 96500C (faraday constant), E0 = 0.0713 V (ref. Chem. Educ., 1969, 46 (11), p 741)
sustituting these values into Nernst equation
E = 0.0713-0.0601log(3.5)
E = 0.0385 V
A silver-silver bromide wire is sometimes used as a reference electrode when Cl- -free conditions must...
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?
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=
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