O Macmillan LearningIron was electrolytically plated onto a platinum gauze electrode from a solution containing 270 g/L FeSO4 ·7H₂O,50 g/L HNO3, and 6 g/L NaCl at −1.3 V vs. Ag|AgCl. Prior to deposition, the platinum electrode weighed 0.4612 g. After13.74 C were passed through the circuit, the elecrode weighed 0.4649 g. In addition to the reduction of iron, the reduction of H+to H2 also occurs during the electrolysis. What percentage of the charge was used in the reduction of iron?charge used in iron reduction:%Chapter 17 Ho

The amount of iron deposited can be calculated by subtracting the initial weight of the electrode…

Answered: O Macmillan Learning Iron was…

Appl Of Ms Excel In Analytical Chemistry

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Chapter10: Potentiometry And Redox Titrations

Section: Chapter Questions

Problem 3P

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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.
A conductivity cell filled with a 0.01 M KCl solution was found to have a resistance of 189 ohms at 25oC. When filled with 0.01 M HCl solution, the cell gave a resistance of 64.8 ohms at the same temperature. At 25oC, the conductivity of 0.01 M KCl solution was 1.4088 x 10-3 S cm-1. Calculate (a) the cell constant and (b) the conductivity of the HCl solution. answer is [0.266; 4.105 x 10-3] please explain. thank you!
(c)Ions that react with Ag+ like SCN- can be determined electrogravimetricallyby deposition on a silver working anode:Ag(s) + SCN- ≤ AgSCN(s) + eA silver anode with initial mass of 12.4730 g was used to electrolyse 85.00 mL of asolution of 0.0245 M KSCN. At the end of the experiment, the anode weighed12.5767 g. How long did the experiment take, if a current of 100 mA was used?
Calculate the potential of the copper electrode immersed in a 0.0750 M NaCI solution saturated with CuC12 (EOCU + / Cu = 0.521 V; Kç CuC12 = 1.9 x 10-7)
Calibration of a glass electrode gave a reading of 129.7 mV with a saturated potassium hydrogen tartrate buffer standard ( pH = 3.557), and a reading of -98.7 mV with a 0.008695 m potassium dihydrogen phosphate, 0.0343 m disodium hydrogen phosphate buffer standard (pH = 7.400), both measured at 30 °C. What is the observed slope (mV/pH unit) of the calibration curve? slopeobserved = mV/pH What is the theoretical slope at 30 °C? slope heoretical mV/pH What is the pH of an unknown that gives a reading of 18.5 mV with this electrode at 30 °C? pH =
A potassium ion-selective electrode is used to measure the concentration of potassium ion in a solution that contains 6.0 x 10-3 M cesium (activity). The electrode responds equally to either ion (KK.C = 1). If the potential versus a reference electrode is -18.3 mV for a 5.0 x 10-3 M KCI solution and +20.9 mV in the sample solution, what is the activity of K+ in the sample? Assume Nernstian response
Electrochemical solutions of MY and MX2 were prepared by successive dilutions and their resistances were measured all from a conductivity cell. The following values were obtained at 25ºC. C(mol/L) 0,001 0,050 R para MX2/Ω 1669 37,14 R para MY/ Ω 4242 561 Knowing that this is a strong and weak electrolyte, answer:a) Which is the strong electrolyte and which is the weak electrolyte? Justify your answerb) Knowing that λ(Y2-)= 10.66 mS m2 mol -1 and λ(X-)=3.01 mS m2 mol-1 estimate the equilibrium constant of the weak electrolyte and the degree of ionization of an aqueous solution of this electrolyte a 0.050 mol/L at 25ºC. Conductivity cell data: molar conductivity=158.39 S cm2 mol-1 and R=4.62 for KCL 0.3 mol/L in the same cell in which the above electrolyte measurements were performed at 25ºC.
A platinum electrode is immersed into a solution of 10 mol m-3 KNO3 and poised at -1 V. (1) Sketch how the concentration of potassium ions, [K+], change as a function of distance, x, from the electrode surface. (Calculate the extent to which the electrical double layer protrudes from the electrode surface, assuming a water solvent (\epsi r = 78.1) at 25 deg C I
At 25C, you conduct a titration of 20.00 mL of a 0.0400 M AgNO3 solution with a 0.050 M NaI solution within the following cell: Saturated Calomel Electrode | Titration solution | Ag(s) for the cell as writted, what is the voltage after the addition of 10.00 mL of the NaI sooution? The reduction potential for the saturated calomel electrode is E=0.241 V. The standard reduction potential for the reaction: Ag++e- ® Ag(s) E0= 0.79993V. The solubility constant of AgI is Ksp=8.3x10-17 Note: the cell potential could be negative since the condditions are non-standard ones. a)0.169 b)0.354 c)0.235 d)2.360 e)0.441
Hittorf cells with silver-silver chloride electrodes were filled with HCl solution with a molality of 0.0106 mol / kg. 2 mA strong current flowed into the cell for 3 hours. At the end of the experiment, the solution at the cathode contained 51.7169 g water and 0.0267 g HCl. Find the transport numbers H + and Cl-
A 50.00-mL aliquot of a solution containing 0.0400 M Fe(NH4)2(SO4)2 is titrated with 0.0500 M Ce(SO4)2. Calculate the potential of the indicator cathode with respect to an SCE reference electrode after addition of 42.00 mL of cerium(IV). Given: E(Ce4*/Ce3*) = 1.44 V, E'(Fe3*/Fe2*) = 0.771 V O 1.12 V O 0.91 V O 2.21 V O 1.71 V O 1.36 V
The 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-3

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