5. A corrosion potential of -0.229 V versus SCE was measured for a corroding alloy. What is the potential versus SHE? Ag/AgCl (saturated)? Cu/saturated CuS04? Saturated Calomel?
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A corrosion potential of -0.23 V vs saturated calomel electrode (SCE) was measured for a corroding alloy. What is the potential versus standard hydrogen electrode (SHE)? Ag/AgCl (saturated) (SSC)? Cu/CuSO4 (saturated) (CCS)?
Sri K.
14-2. Convert the following potentials. The Ag | AgCl and calomel reference electrodes are saturated with KCl. (a) 0.523 V versus S.H.E. = ? versus Ag | AgCl (b) -0.111 V versus Ag | AgCl = ? versus S.H.E. (c) -0.222 V versus S.C.E. = ? versus S.H.E. (d) 0.023 V versus Ag | AgCl = ? versus S.C.E. (e) -0.023 V versus S.C.E. = ? versus Ag | AgCl
Ivan K.
Reference Electrodes The E° value for the following reaction is 0.446 V relative to the standard hydrogen electrode (SHE): Ag2CrO4(s) + 2e- → 2Ag(s) + CrO42-(aq) A chemist wishes to determine the concentration of CrO42- electrochemically. A cell is constructed consisting of a saturated calomel electrode (SCE; which has a reduction potential of 0.242 V relative to the SHE) and a silver wire coated with Ag2CrO4 and suspended in a CrO42- solution. What is the potential of this cell at 25°C when [CrO42-] = 1.00 M? 0.446 V The Saturated Calomel Electrode (SCE) is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCl. This description is not actually needed to do this problem but is worth knowing anyway. The important thing is to visualize a Galvanic cell having the silver + chromate reaction in one half-cell versus another half-cell of the given potential of the SCE and to combine the half-cell potentials correctly. Calculate ΔG for the full-cell reaction at 25°C when [CrO42-] = 1.00 M? What is the potential of this cell at 25°C when [CrO42-] = 6.50×10-9 M? 0.686 V For a solution of unknown [CrO42-], the measured potential for the cell at 25°C is 0.388 V. What is [CrO42-] (in mol/L)? 91.2 M You have not been told which direction the current flows through the cell but consider this: A saturated K2CrO4 solution is about 3.6 M (at 25°C). Even the most soluble chromate salts will not exceed about 7 M. What does this mean in terms of the possible direction of the redox reactions occuring in the cell? (i.e. Could the polarity of the cell be reversed at some achievable chromate concentration?)
Adi S.
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