/10.7 Careful measurements of the potential of the cell Pt|H2(g,p°) |NaOH(aq, 0.0100 mol kg*1), NaCI(aq,0.01125 mol kg-l) |AGČI(s)|Ag have been reported (C.P. Bezboruah, M.F.G.F.C. Camoes, A.K. Covington, and J.V. Dobson, J. Chem. Sóc. Faraday Trans. I; 69, 949 (1973)). Among the data is the following information: 0/°C 20.0 25.0 30.0 E/V 1.04774 1.04864 1.04942 Calculate pK, at these temperatures and the standard enthalpy and entropy of the autoprotolysis of water at 25.0°C. the tyne

/10.7 Careful measurements of the potential of the cell Pt|H2(g,p°) |NaOH(aq, 0.0100 mol kg*1), NaCI(aq,0.01125 mol kg-l) |AGČI(s)|Ag have been reported (C.P. Bezboruah, M.F.G.F.C. Camoes, A.K. Covington, and J.V. Dobson, J. Chem. Sóc. Faraday Trans. I; 69, 949 (1973)). Among the data is the following information: 0/°C 20.0 25.0 30.0 E/V 1.04774 1.04864 1.04942 Calculate pK, at these temperatures and the standard enthalpy and entropy of the autoprotolysis of water at 25.0°C. the tyne

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.23QAP

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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.
16.4 Careful measurements of the potential of the cell Pt|H,(g,p®)| NaOH(aq,0.0100 molkg"),NaCI(aq, 0.011 25 mol kg")|AgCl(s)|Ag(s) have been reported. Among the data is the following information: 20.0 25.0 30.0 EcaV 1.04774 1.04864 1.04942 Calculate pK, at these temperatures and the standard enthalpy and entropy of the autoprotolysis of water at 25.0°C. Recall that K, is the equilibrium constant for the autoprotolysis of liquid water.
Careful measurements of the potential of the cell Pt|H2(g.pe)|NaOH(aq,0.0100 mol kg-4),NaCl(aq, 0.011 25 mol kg-1)|AgC(s)|Ag(s) have been reported. Among the data is the following information: 0/°C 20.0 25.0 30.0 Ecell/V 1.04774 1.04864 1.04942 Calculate pKw at these temperatures and the standard enthalpy and entropy of the autoprotolysis of water at 25.0 °C. Recall that Kw, is the equilibrium constant for the autoprotolysis of liquid water.
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?
a. Calculate for the process AgIO3(s) +eAg(s) + 103 PIO3 = Ag+ /Ag E = b. Use the shorthand notation to describe a cell consisting of a saturated calomel reference electrode and a silver indicator electrode that could be used to measure PIO3. (Enter saturated calomel electrode as SCE. Omit states of matter.) (x M), II (sat'd)| c. Develop an equation that relates the potential of the cell in (b) to pIO3. (At 25°C, the potential of the saturated calomel electrode versus the standard hydrogen electrode is 0.244 V. Enter cell potencial as Ecell-) = 0.799 V, Ksp (AgIO₂) = 3.1 x 10-8) V d. Calculate pIO; if the cell in (b) has a potential of 0.321 V. PIO3 =
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?
Marked out of 3.00 Choose the best answer Ecell for Pt|H2 (p-1 atm)lH*(m)||Cl|H92C2IH9|Pt is 0.398 V at 1.0 atm and 306.4 K. Eo for the normal calomel electrode is 0.28V. Calculate the pH of solution (without activity) a. 3.88087 b. 1.94096 C. -1.63185 d. 2.02350 e. 0.95627
Give answer all questions with explanation please
Please complete Table A1.
For the following Cell. Pt | H2 (g, p°) | HCI (aq, b) | Hg2 Cl2 (s) | Hg (1) The EMF at 25°C as a function of molality are tabulate below. Using DHLL, determine standard electrode potential of the cell and calculate the mean activity coefficient y+ of HCl for all molalities. C / mmol / kg 2.009625 3.846125 6.300375 9.617250 13.68425 E / V 0.48064 0.45464 0.43496 0.41816 0.40424
Chemistry التاريخ - Ex:write the reaction cell ? then calculate AG", AH, AS for the following Fe/Fe (1M) // Brz (tata), BF (14). /pt.
15 The electromotive force of the cell: Pt | H,(1 atm) | HCI | Hg,CI, | Hg; is 0.686 V at 300 K. The pH of the HCI solution is; ( Hg,CI, + 2e E° = 0.2802 V) * 2Hg + 2CI %3D 5.85 O 4.27 O 2.49 6.87 О 3.43