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

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The Sn in a 0.4352 g mineral specimen was reduced to the +2 state and titrated with 29.77 mL of 0.01735 M K2Cr2O7. Identify: (a) type of redox titrimetry used (b) appropriate indicator and its type (c) color at the end point (d) weight percent Sn (118.71 g/mol) in the sample
What is the current efficiency of a nickel-plating bath if the cathode of a copper coulometer in series with the experimental cell was found to have gained 1.025 g and the weight of nickel deposited was 0.905 g?
The Sn in a 0.4352 g mineral specimen was reduced to the +2 state and titrated with 29.77 mL of 0.01735 M K2Cr2O7. Identify: (a) method of redox titrimetry used (Dichrometry, Cerimetry, iodimetry, iodometry or, permanganometry) (b) appropriate indicator and its type (c) color at the end point (d) weight percent Sn (118.71 g/mol) in the sample
The following statements are true for Amperostatic Cuolometric Methods of analysis except - in constant current system, the potential of the cell will vary in time as analyte is consumed cuolometric titrations can be performed at constant current to generate a known quantity of titrant electrochemically a second electrode is no longer needed to detect endpoint of the analysis can be used for acid/base, complexometric and redox titrations The following are true about redox reactions except: * it involves transfer of electrons or charged particles the reaction is performed by bringing the oxidant and the reductant into direct contact in a container the reaction is carried out in an electrochemical cell in which the reactants do not come into contact. an anode is where reduction takes place The following are excitation signals used for voltammetry except-* linear scan differential pulse square wave triangular wavelength quant
A solution prepared by mixing 60.0 mL of 0.360 M AGNO, and 60.0 mL of 0.360 M TINO, was titrated with 0.720 M NaBr in a cell containing a silver indicator electrode and a reference electrode with a constant potential of 0.175 V. The reference electrode is attached to the positive terminal of the potentiometer, and the silver electrode is attached to the negative terminal. The solubility constant of TIBr is Kp = 3.6 × 10-6 and the solubility constant of AgBr is = 5.0 x 10-13. Ksp Which precipitate forms first? O TIBI O AgBr Which of the expressions shows how the cell potential, E, depends on [Ag*]? E = 0.175 V – [0.799 V – 0.05916log ([Ag+])] 1 E = |0.799 V – 0.05916log - 0.175 V [Ag*) E = [0.799 V – 0.05916log ([Ag*]D] – 0.175 V E = 0.175 V - |0.799 V – 0.05916log [Ag* * (ল) Calculate the first and second equivalence points of the titration. first equivalence point: mL second equivalence point: mL What is the cell potential after each of the given volumes of 0.720 M NaBr have been…
Given that standard reduction potentials at 298.15 K are E° Mg*2 /Mg = -2.37 V and E° Sn2*/Sn = -0.140; then if a Mg(s) foil is soak in 1.0 M SnCl2(ag), the Mg foil be will be oxidized and eventually dissolve.
Predict the product and balance redox reaction The presence of sulfuric acid , an excess KMN04 will oxidize a chromic salt to dichromate and manganous ion.
. Consider a galvanic cell with the anode containing a Zn metal electrode and a 0.10 M Zn(NO3)2solution and the other half-cell containing a Sn metal electrode and a 0.10 M Sn(NO3)2 solution. If themeasured Ecell value is +650 mV and the Zn2+/Zn reduction potential is assumed to be −790 mV, what isthe Sn2+/Sn reduction potential? Show all work.
Answer my question please
V. (6)H in 0.20 bar Salt bridge |(ag) H(ao) Pt Ag wire coated with Agi(s) Nal (0.10 M) HCI (0.10 M) (a) Write the line notation for this cell. (b) Calculate the potential for each half-cell and the cell voltage E. (c) Write the spontaneous net cell reaction.
You are given the following three half-reactions
2) A 90.00 ml solution, density = 1.0582 g/mL. with a AG = specif ic heat of 4.079 J/(GC), increased in temperature ΔΗ- from 20.36 C to 28.13 t with Al added. The copper collected, weighed 2.087 g. The electrochemical AS = potential mean was +1.821 volts. Calculate AG AH and AS for the reaction below. +3 2A (aq) +2 2 Als) * 3 Cuaq) 3 C46)