2Determine the transport numbers of the ions in an exactly 0.200 molal solution of copper (II) sulfate. The cell was filled with solution and electrolyzed between copper electrodes for some time. The cathode solution of the cell was found to weigh 36.434 g and contains 0.4415 g of Cu. Further the cathode in the coulometer showed an increase in weight of 0.0405 g due to deposited Ag. Please answer completely

2Determine the transport numbers of the ions in an exactly 0.200 molal solution of copper (II) sulfate. The cell was filled with solution and electrolyzed between copper electrodes for some time. The cathode solution of the cell was found to weigh 36.434 g and contains 0.4415 g of Cu. Further the cathode in the coulometer showed an increase in weight of 0.0405 g due to deposited Ag. Please answer completely

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter22: Bulk Electrolysis: Electrogravimetry And Coulometry

Section: Chapter Questions

Problem 22.21QAP

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Determine the transport numbers of the ions in an exactly 0.200 molal solution of copper (II) sulfate. The cell was filled with solution and electrolyzed between copper electrodes for some time. The cathode solution of the cell was found to weigh 36.434 g and contains 0.4415 g of Cu. Further the cathode in the coulometer showed an increase in weight of 0.0405 g due to deposited Ag.
What Range of cathode potentials versus the saturated calomel electrode can be used to quantitatively separate Ag+ and Ni2+ by electrolytic deposition? Assume that the sample solution is initially 0.1000M in each ion and the quantitative removal of an ion is realized when only 1 part in 10000 remains undeposited. ESCE = 0.244V E0Red (Ag+) = 0.8V E0Oxid (Ni) = -0.25V
Use the shorthand notation to describe a cell consisting of a saturated calomel reference electrode and a silver indicator electrode for the measurement of (a) pSCN. (b) pI. (c) pSO3 (d) pPO. Then, generate an equation that relates pAnion to Ecell for each of the cells. (For Ag2SO3 Ksp = 1.5 * 10-14; for Ag3PO4, K,p = 1.3 *10-20 ).
A 0.2g sample of toothpaste containing fluoride was treated with 50 cm3 of a suitable buffer solution and diluted to 100 cm3. Using a fluoride ion-selective electrode, a 25.00 cm3 aliquot of this solution gave cell potentials of –155.3 mV before and –176.2 mV after spiking with 0.1 cm3 of a 0.5 mg/cm3 fluoride standard. Calculate the pF– corresponding to each cell potential and the percentage by weight of fluoride in the toothpaste.
Why is it necessary for the glass in the membrane of a pH sensitive electrode to beappreciably hygroscopic ?
It is desired to assemble a concentration cell with a potential of 120 mV withtwo Zn(s) electrodes immersed, each one, in a ZnSO4 solution. What should be theratio between Zn2+ activities in the two electrodes to reach the desired potential?
why is equivalent weight of KMnO4 is different in acidic, alkaline and neutral medium ?
If a dilute H2 SO4 solution is electrolyzed with copper electrodes, the most likely electrode reactions are 2H ^ + + 2e- = H2 (g) at the cathode and 2Cu (s) + H2O = Cu2O (s) + 2H ^ + + 2e- at the anode. If we observe the formation of 27.4 cm3 of moist hydrogen (751 barometric torrs, 23.3 ° C) at the cathode, what change in weight will there be simultaneously at the anode? Data: Pv H2O 23.3 ° C = 22 torr.Atomic mass: Cu (65); O (16); H (1)
Give Reason? (i) Why is a high supporting electrolyte concentration used in most electroanalyticalprocedures?(ii) Why is the reference electrode placed near the working electrode in a threeelectrode cell?
Given that ΔrG⦵ = −212.7 kJ mol−1 for the reaction Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) in the Daniell cell at 25 °C, and b (CuSO4) = 1.00 × 10−3 mol kg−1 and b (ZnSO4) = 3.00 × 10−3 mol kg−1, calculate (a) the ionic strengths of the solutions, (b) the mean ionic activity coefficients in the compartments, (c) the reaction quotient, (d) the standard cell potential, and (e) the cell potential. (Take γ+ = γ− = γ± in the respective compartments. Use the Debye–Hückel limiting law.)
The sensitivity of a coulometer is governed by the delivery of its minimum current for its minimum time. Suppose that 5 mA can be delivered for 0.1 s.(a) How many moles of electrons are delivered at 5 mA for 0.1 s? (b) How many milliliters of a 0.01 M solution of a two-electron reducing agent are required to deliver the same number of electrons?
A 40.00-mL aliquot of 0.05000 M HNO2 is diluted to 75.00 mL and titrated with 0.0800 M Ce4+. The pH of the solution is maintained at 1.00 throughout the titration; the formal potential of the cerium system is 1.44V a. Calculate the potential of the indicator electrode with respect to a saturated calomel reference electrode after the addition of 5.00, 10.00, 15.00, 25.00, 40.00, 49.00, 49.50, 49.60, 49.70, 49.80, 49.90, 49.95, 49.99, 50.00, 50.01, 50.05, 50.10, 50.20, 50.30, 50.40, 50.50, 51.00, 60.00, 75.00 and 90.00 mL of Cerium (IV). b. Draw a titration curve for these data. c. Generate a first- and second-derivative curve for these data. Does the volume at which the second-derivative curve crosses zero correspond to the theoretical equivalence point? Why or why not?