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- Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.For each of the following reactions, determine the overall balanced electrochemical reaction, its standard electric potential, and the standard Gibbs energy of the reaction. aCo+F2Co2++2F bZn+Fe2+Zn2++Fe c Zn+Fe3+Zn2++Fe d Hg2++HgHg22+The cell Ag|AgCl(sat'd)||H+(a=x)glass electrode has a potential of -0.2094V when tne solution in the right hand compartment is a buffer of pH 4.006. The following potential are obtained when the buffer is replaced with unknowns:(a)-0.2806V and (b)-0.2132V. Calculate the pH and the hydrogen ion activity of each unknown.(c)Assuming an uncertainty of 0.001V in the junction potential,what is range of hydrogen ion activities within which the true value might be expected to lie?
- A bromine ion selective electrode has a selectivity coefficient K Br-, OH- = 0.05. What will be the change (absolute value in mV, NO UNITS, one figure after decimal point examples 3.3 or 33.0) in electrode potential when in 4.0 x 10-5 M Br" aqueous solution pH 6.0 is raised to pH 9.8 at constant temperature of 25 °C? Give answer as an absolute value in mV, NO UNITS, one figure after decimal point, examples 3.3 and 33.0 Answer:A 0.10 M FeSO:(aq) solution is electrolyzed between a magnesium cathode and a platinum anode with a current density of 1.0 mA cm-2. The hydrogen overpotential is 0.65 V. What will be the concentration of Fe2+ ions when evolution of H2 just begins at the cathode? Assume all activity coefficients are unity. (E°(Fe2*/Fe) = -0.44V)1. (a) Calculate Eo’ for the process:AgI03(s) + e- ⇔ Ag(s) + I0 3-(b) Use the shorthand notation to describe a cell consisting of a saturated calomel reference electrodeand a silver indicator electrode that could be used to measure pIO3.(c) Develop an equation that relates the potential of the cell in (b) to pIO3.(d) Calculate plO3 if the cell in (b) has a potential of 0.294 V.
- 13.28 For the cell Pt,|Fe²*(a = 2.00), Fe**(a = 1.20):|I"(a = 0.100)|1½(s)|Ptg %3D %3D R (a) write the cell reaction; (b) calculate E298 assuming the net liquid-junction potential is negligible. (c) Which terminal is at the higher potential? (d) When the cell is connected to a load, into which terminal do electrons flow from the load?Calculate the standard cell potential at 25°C for the following cell reaction from standard free energies of formation: 2AI(:) + ЗHg2* (ад) —» 2AB (аq) + ЗHg() Standard Free Energy of Formation Ion AG; (kJ/mol) Al+ (ag) -485.0 Zn²+ (ag) -147.0 Co+ (aq) -54.4 Ni²+ (aq) -45.6 2+ (ag) -24.39 Cu²+ (aq) 65.52 Hg²+ (aq) 164.4 Fe?+ (ag) -78.87 V Standard cell potential =3 . For cell schematic notation Zn(s) | ZnCl2 (1.0 M )| | CuSO4 ( 2.0 M ) | Cu(s) (standard reduction potential E˚Zn(II)/Zn = -1.3 V E˚Cu(II)/Cu = 0.80 V T=25 ˚C R = 8.314 J ) (a ) Calculate Ecell of the above cell in volts. (b) Is this cell being used as a battery or electrolytic cell ? Is the overall cell reaction a spontaneous one ? (c ) Write the reactions at the anode and cathode respectively. ( d) Calculate the equilibrium constant K for the reaction Zn 2+ (aq) + Cu (s ) = Cu 2+ ( aq ) + Zn (s) ( e ) What is the purpose to construct the following cell in Quant Analysis ? Please explain. Ag(s) | AgCl(s), KCl (1.0 M ) | | Cu 2+ ( aqueous ) | Cu(s)
- Propagation of uncertainty. In an extremely accurate measurement of the Faraday constant, a pure silver anode was oxidized to Ag1 with a constant current of 0.203 639 0 (60.000 000 4) A for 18 000.075 (60.010) s to give a mass loss of 4.097 900 (60.000 003) g from the anode. Given that the atomic mass of Ag is 107.868 2 (60.000 2), find the value of the Faraday constant and its uncertainty.What reactions occur during the electrolysis of aqueous Nal between Pt electrodes? & of Na | Nat = -2.71 V E of Pt | 12, 1 = 0.53 V E of Pt | H₂O, H₂, OH = -0.83 V E of Pt | H₂O, O2, H+ = 1.23 V H₂(g) evolves at the cathode, O2(g) evolves at the anode Na(s) deposits at the cathode, 12(s) deposits at the anode H₂(g) evolves at the cathode, 12(s) deposits at the anode Na(s) deposits at the cathode, O2(g) evolves at the anodeA fluoride ion-selective electrode has a selectivity coefficient Kot F, OH- = 0.1. What will be the change in electrode potential when the pH of 1.0 X 10-4 M solution of F is raised from pH = 5.5 to pH= 11.5. The potential of an ion-selective electrode is 0.05916 E= constant + B log(IA]sample + E KAI'[!) where: z = -1 for fluoride ion and assume B = 1. Express your answer in units of Volt. Do not write down the unit.