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- Which of the following statements is/are correct for coulometry? I. Coulometric methods count the electrons used in a chemical reaction to measure the analyte. II. Coulometry uses constant current or constant potential conditions. III. An advantage of coulometric methods is low reproducibility and a disadvantage is low sensitivity. IV. Coulometric titrations are constant potential methods. V. Constant potential methods using a three-electrode cell are more selective than constant-current methods.By how many volts will the potential of an ideal Mg2+ ion selective electrode (ISE) change if the electrode is removed from a 1.0 x 10-4 M solution of MgCl2 and placed in 1.0 x 10-3 M MgCl2? 28 mL of 0.1M Ce4+ is mixed with 50 mL of 0.05M Fe2+. The solution potential is monitored with a Pt indicator electrode and an Ag/AgCl reference electrode. Calculate the potential of the Pt electrode and the cell potential. An ion selective electrode for NO2- has the following values of Log k for the listed interferents. Interferent Logk F- -3.1 SO42- -4.1 I- -1.2 NO3- -3.3 Which ion…Which of the following statements is/are correct for coulometry? I. Coulometric methods count the electrons used in a chemical reaction to measure the analyte. II. Coulometry uses constant current or constant potential conditions. III. An advantage of coulometric methods is low reproducibility and a disadvantage is low sensitivity. IV. Coulometric titrations are constant potential methods. V. Constant potential methods using a three-electrode cell are more selective than constant-current methods. A). I, II and V B). I, II, IV and V C). I, III and IV D.) II, IV and V
- 1) Since E0 (Fe3 + / Fe2 +) = + 0.77 V, E0 (Fe2 + / Feo) = - 0.44 V and E0 (MnO4- / Mn2 +) = +1.51 VFe / Fe3 + (0.01M) // pH = 3; MnO4- (0.10M); Mn2 + (0.01M) / PtWrite down the anode, cathode and total battery reactions of the battery. Calculate the cell potential at a temperature of 25 degrees Celsius and the equilibrium constant of the spontaneous reaction in the cell with the Gibbs Free Energy Change.Consider mixing 25mL of V (III) 0.0361 mol / L and V (II) 0.0904 mol / L solution with 10 mL of a 0.0835 mol / L and Cr (II) solution of Cr (III) ) 0.119 mol / L. (Data: E ° (Cr3 + / Cr2 +) = - 0.407 V; E ° (V3 + / V2 +) = -0.225 V). a) Calculate the cell potential and write the schematic representation of the cell. b) Determine the equilibrium constant.Given the standard reduction potentials (Eo ’) for ubiquinone (Q) Q + 2H+ + 2e- ---> QH2 E o ’ = 0.04V FMN + 2H+ + 2e- ---> FMNH2 E o ’ = -0.22V Calculate the standard ΔEo ’ for the oxidation of FMNH2 by Q. Make sure to show each half reaction and the overall redox reaction. From the reactants in your derived redox reaction, indicate the oxidant and reductant
- Calculate the emf at 298.15 K generated by the oxidation of Fe2+ by O2 in acidic solution, according to the following reaction: O2(g) + 4H+(aq) + 4Fe2+(aq) ⟶ 4Fe3+(aq) + 2H2O(l) when [H+] = 0.003 M, [Fe3+] = 2.5 x 10 – 4 M, and [Fe2+] = 0.18 M. Also, write the complete (oxidation/reduction) half-reactions.1) Since E0 (Fe3 + / Fe2 +) = + 0.77 V, E0 (Fe2 + / Feo) = - 0.44 V and E0 (MnO4- / Mn2 +) = +1.51 VFe / Fe3 + (0.01M) // pH = 3; MnO4- (0.10M); Mn2 + (0.01M) / PtWrite down the anode, cathode and total battery reactions of the battery. Calculate the cell potential at 25 oC and the equilibrium constant of the spontaneous reaction in the cell using the Gibbs Free Energy Change.2. Calculate the equilibrium constant at 25°C for the reactionH2 + 2Fe 3+→ 2H+ + Fe2+E° H+|H2 = 0.00 V and E° Fe3+|Fe2+ = 0.771 V 3. Given the standard of the Cu2+/Cu and the Cu+/Cu couples are +0.340 V and +0.522 V,respectively, evaluate E°(Cu2+/ Cu+)
- Calculate potentials after the addition of a) 25.00 mL; b) Veq; c) 50.00 mL of 0.0800 M Sn4+ to 50.00 mL of 0.100 M V2+ V 3+ + e V 2+ E 0 = -0.255V Sn4+ + 2e Sn2+ E 0 = 0.154VA bare silver wire electrode is dipped into a solution 0.05M in KNO3 (supporting electrolyte) and saturated in AgBr (Ksp = 5.0 x 10-13), and connected to the back of an mV/pH meter along with a saturated calomel reference electrode. Calculate the potential of the silver indicator electrode. Calculate the cell potential.In a voltammogram, which of the following statements is correct 2 a. The limiting current i, is used for quantitative analysis b. The half-wave potential E₁/2 is used for quantitative analysis c. The limiting current i depends on the identity of the analyte d. The half-wave potential E1/2 dependens on the analyte concentration A 0.20 g sample of primary standard Na₂C₂O4 (134 g/mol) needed 37.22 mL of of KMnO4 solution to reach the end point. What is the molarity of KMnO4 reagent a. 0.14 M b. 0.016 M C. 0.65 M d. 0.0014 M In the glucose sensor, the component diffuses through the inner layer of the electrode is the J a. gluconic acid b. hydrogen peroxide c. glucose d. glucose oxidase
