Indicate the correct expression of the Nernst equation for an AgCl/Ag electrode. (1). EAgCI/CI= E AgCI/CI+ (RT / F) In aa CI Ag (2). Egal/a= E Agc/a - (RT/F) In a (3). EAC/C = E Agcl/a - (RT/2F) In a/a Ag (4). EAC/C = E AC/a - (RT/F) In a / a Ag* cr
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- What is the schematic representation of a cell with a saturated calomel electrode as the reference electrode and a silver indicator electrode to measure the p-function of [CrO4²-]? SCE | Ag2CrO4(sat'd), CrO42-(x M)| Ag O SCE || Ag2 CrO4(s), CrO4²-(x M)| Ag SCE ||Ag2 CrO4(sat'd), CrO4²-(x M) | Ag SCE || Ag2CrO4(s), CrO4²-(x M) | AgCalculate the potential of a calomel electrode (Hg Hg2Cl2, mercurous chloride) in a solution: 1 of NaCl at 1 mol.L´ ; 2 saturated of NaCl (solubility of NaCl in water at 298 K: 4.8 mol.L-¹) 0.789 V; KS(H92Cl2) 1.7×10-17. Data: el (Hg₂+ /Hg) -1 - The answer : 1) e = 0.294 V; 2) e = 0.254 VA 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:
- Write the cell reactios and electrode half reactios and calculate the standardpotetial for each of the following cells (i) Zn/ZnSO4(aq)//AgNO3(aq)/pt (ii)Pt/Fe3+(aq),Fe2+(aq)//S4+(aq),Sn2+(aq)/ptThe described electrochemical cell (concentration cell) was set up: Cu|CuSO4 (c1) // CuSO4 (c2)|Cu Determine which electrode is the positive terminal (+) of the cell and calculate the cell potential E (electromotive force, EMF) for the given concentrations of the electrolyte CuSO4 in the cell (25oC): c1 = 0.01 mol dm-3, c2 = 1×10-4 mol dm-313.28 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?
- The cell 2- SCE// Ag₂ CrO4 (sat'd), CrO4 ²- (xM) /Ag is employed for the determination of pCrO4-. ESCE = 0.244 V at 25 OC The half reaction at indicator electrode Ag₂ CrO4 (s) + 2e- 2 Ag (s) + CrO₂2- E0=+0.446 V 4 a) Calculate pCrO4 when the cell potential is 0.402 V b) What type of indicator electrode is Ag in this case?The standard potential of the cell calomel || nonesuch composed of a calomel electrode and a nonesuch electrode is -1978 mV at 25oC. Find the standard potential of the nonesuch electrode at 25oC.[-1.710] The answer is enclosed in the bracket, I would like to know how it was obtained. Thank you!u = (2)²) id (spheri Date чис Subject Month Year. 58 3.9 Discuss the mechanism by which the potential of a platinum electrode becomes poised by immer- sion into a solution of Fe(II) and Fe(III) in 1 M HCl. Approximately how much charge is required to shift the electrode potential by 100 mV? Why does the potential become uncertain at low concentra- tions of Fe(II) and Fe(III), even if the ratio of their concentrations is held near unity? Does this ex- perimental fact reflect thermodynamic considerations? How well do your answers to these issues apply to the establishment of potential at an ion-selective electrode? فصل دوم مراجع استاد
- Pt (s)) | H2 (g, 1.00 bar) | HCI (5.00E-4 M) || KCI(0.100 M) | Hg() | H&2C1215) The anode in the above cell can actually be considered a standard hydrogen electrode if concentrations were standardized. That would make the cathode an ion selective electrode. What analyte would the electrode be detecting? And what component of the cathode would you replace by the solution containing the unknown concentrations of analyte?(H 15.2) Convert the following potentials. The Ag | AgCl and calomel reference electrodes are saturated with KCI, therefore EºAgCl = 0.199V, ESCE = 0.244V. a. 0.523 V vs. SHE = ? vs. Ag | AgCl b. -0.111 V vs. Ag | AgCl = ? vs. SHE -0.222 V vs. SCE = ? vs. SHE d. 0.023 V vs. Ag | AgCl = ? vs. SCE -0.023 V vs. SCE = ? vs. Ag | AgCl C. e.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.
