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Give the cell diagram for the reaction below.
Cd + 2 Fe3+ ---->Cd2+ + 2 Fe2+
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- The following cell was found to have a potential of —0.492 V: Ag|AgCl(sat’d)||HA(0.200 M),NaA(0.300 M)|H2(1.00 atm),Pt Calculate the dissociation constant of HA, neglecting the junction potential.Give the cell diagram for the reaction below using | and || when applicable.Cd + 2 Fe3+ ---->Cd2+ + 2 Fe2+Explain why ionic attractions are weaker in media with high dielectric constants, e. g.,water and aqueous buffers.
- Write the half-reaction and calculate the electrode potential of a. a platinum electrode in 0.0566 M K4Fe(CN)6 and 0.00813 M K3Fe(CN)6 b.a platinum electrode in a solution buffered at pH 6.00 and saturated withH2(g) at 1.00 atmIn a polarographic experiment of a 60 mL of 0.08 M Cu2+solution, a limitingcurrent was left on for 15 minutes. If the average current during the time of theexperiment is 6.0 μA, what fraction of the copper is removed from the solution? TheFaraday constant is 96485 C/mol of electron.Given a cell: 2 Ag+(aq) + Cu(s) ----> 2Ag (s) + Cu2+ (aq), E(cell) = 0.346 V, E0(cell) = E0cathode - E0anode = 0.800 V - 0.340 V = 0.460 V, I. calculate the concentration of Cu2+ given that of Ag+ is 1.0 x 10-5M Cu2+M= Keq =
- Given a cell: 2 Ag+(aq) + Cu(s) ----> 2Ag (s) + Cu2+ (aq), E(cell) = 0.346 V, E0(cell) = E0cathode - E0anode = 0.800 V - 0.340 V = 0.460 V, I. calculate the concentration of Cu2+ given that of Ag+ is 1.0 x 10-5MThe following cell was employed for the determination of pCrO4: SCE // CrO4 2-(xM) / Ag2CrO4 (s) / Ag (s) Find the pCrO4 if the cell potential is - 0.402 V (E0 Ag/Ag2CrO4 = - 0.316 V ; E SCE = 0.241 V)Many applications of electrochemistry have been in chemical analysis.Suppose a Fe|Fe2+ concentration cell is set-up in which the [Fe2+] = 1.0 x10¯2 M in one compartment but the concentration in the othercompartment is unknown. The Ecell was measured at 0.024V when thehalf-cells were connected.(i) Without doing a numerical calculation, is the unknown more orless concentrated than the 1.0 x 10¯2 M solution? Justify youranswer
- Many applications of electrochemistry have been in chemical analysis.Suppose a Fe|Fe2+ concentration cell is set-up in which the [Fe2+] = 1.0 x10¯2 M in one compartment but the concentration in the othercompartment is unknown. The Ecell was measured at 0.024V when thehalf-cells were connected.(i) Without doing a numerical calculation, is the unknown more orless concentrated than the 1.0 x 10¯2 M solution? Justify youranswer(ii) Calculate the unknown concentration.(iii) Does your calculated answer agree with your original answer?Why?What is the voltage associated with the 2-electron reduction of Cu2+ to Cu at the cathode and the 2-electron oxidation of Fe to Fe2+ at the anode under standard conditions?A concentration cell was made using a silver metal electrode in a saturated solution of AgCl for the anode half cell, and a silver metal electrode in 1.00 M Ag⁺ for the cathode half cell. E for the cell was 0.288 V at 25°C. Calculate the Ksp for AgCl. (Note: For purposes of this exercise, carry out the calculation to three significant figures.)