Solve for all questions The titration solution in the cell below had a total volume of 50.0 ml and contained0.100 M Mg2+ and 1.00 x 10-5 M Zn(EDTA)2- at a pH of 10.00s.C.E. || Zn(s) | titration solutionZn2* + 2e- Zn(s) E' = -0.762 vMgY2-: Kf = 6.2 x 108; Zny2- : Kf = 3.2 x 1016.What will be the cell voltage when 10.0 mL of 0.100 M EDTA has been added? (Hint: SeeExercise 15-B.)i)Total mmoles of Mg*2mmoles of EDTA added ismmoles of Mg*2 reacting with EDTAiv)mmoles of MgY2-v)Concentration of MgY2- in Mvi)mmoles of excess unreacted Mg+2vii)Concentration of Mg*2 in Mviii)Concentration of EDTA (Y4-) in Mix)Total mmoles of Zn+2{1:NUMERICAL:%100%0.500:0.15}x)mole of Zny2- in Mxi)Concentration of ZnY2- in Mxii)Concentration of Zn2+ in Mxiii)Potential of the cell in voltage, Ecell={1:NUMERICAL-1.364:0.1}13 marks

Dear students , according to bartleby policy I am only authorized to answer starting 1st three parts…

The titration solution in the cell below had a total volume of 50.0 mL and contained 0.100 M Mg2+ and 1.00 x 10-5 M Zn(EDTA)2- at a pH of 10.00 s.C.E. || Zn(s) | titration solution Zn2* + 2e- Zn(s) E' = -0.762 v Mgy2-: Kf = 6.2 x 108; Zny2-: Kf = 3.2 x 1016. What will be the cell voltage when 10.0 mL of 0.100 M EDTA has been added? (Hint: Se Exercise 15-B.) i) Total mmoles of Mg*2 ii) mmoles of EDTA added is iii) mmoles of Mg*+2 reacting with EDTA

The titration solution in the cell below had a total volume of 50.0 mL and contained 0.100 M Mg2+ and 1.00 x 10-5 M Zn(EDTA)2- at a pH of 10.00 s.C.E. || Zn(s) | titration solution Zn2* + 2e- Zn(s) E' = -0.762 v Mgy2-: Kf = 6.2 x 108; Zny2-: Kf = 3.2 x 1016. What will be the cell voltage when 10.0 mL of 0.100 M EDTA has been added? (Hint: Se Exercise 15-B.) i) Total mmoles of Mg2 ii) mmoles of EDTA added is iii) mmoles of Mg+2 reacting with EDTA

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter22: Bulk Electrolysis: Electrogravimetry And Coulometry

Section: Chapter Questions

Problem 22.21QAP

See similar textbooks

Similar questions

Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
What cathode potential (versus SCE) would be required to lower the total Hg(II) concentration of the following solutions to 1.00 10-6 M (assume reaction product in each case is elemental Hg): (a) an aqueous solution of Hg2+? (b) a solution with an equilibrium SCN- concentration of 0.100 M? Hg2+ + 2SCN- Hg(SCN)2(aq) = Kf = 1.8 107 c) a solution with an equilibrium Br- concentration of 0.100 M? HgBr42++ 2e- Hg(l) + 4Br- E0= 0.223 V
The measurement of pH using a glass electrode obeys the Nernst equation. The typical response of a pH meter at 25 00C is given by the equation where contains the potential of the reference electrode and all other potentials that arise in the cell that are not related to the hydrogen ion concentration. Assume that = 0.250 V and that a. What is the uncertainty in the values of pH and [H+] if the uncertainty in the measured potential is 1 m V ( 0.001 V)? b. To what precision must the potential be measured for the uncertainty in pH to be 0.02 pH unit?
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.
I want all questions answered Consider the cell: Pt|H₂(g,p°)| HCl(aq)|AgCl(s)|Ag for which the cell reaction is 2AgCl(s) +H₂(g) → 2 Ag(s) + 2HCl(aq). At 25 °C and a molality of HCl of 0.010 mol kg⁻¹ . Calculate ionic strength of solution?Calculate (in volts) Standard Electrode Potential of the cell E°:?Calculate (in kJ/mol) Standard Gibbs Free Energy of the cell ΔrG°?Assuming Debye-Huckel limiting law holds at this concentration, calculate (in volts) Ecell (Cl⁻, AgCl, Ag)? Assuming Debye-Huckel limiting law holds at this concentration, calculate (in kJ) ΔrG?
Black-and-white photographic film is coated with silver halides. Because silver is expensive, the manufacturer monitors the Ag⁺ content of the waste stream, [Ag⁺]ᵥᵥₐₛₜₑ, from the plantwith an Ag-selective electrode at 25°C. A stream of known Ag⁺ concentration, [Ag⁺](standard), is passed over the electrode inturn with the waste stream and the data recorded by a computer.(a) Write the equations relating the nonstandard cell potential tothe standard cell potential and [Ag⁺] for each solution.(b) Combine these into a single equation to find [Ag⁺]ᵥᵥₐₛₜₑ.(c) Rewrite the equation from part (b) to find [Ag⁺]ᵥᵥₐₛₜₑ in ng/L.(d) If Eᵥᵥₐₛₜₑ is 0.003 V higher than E(standard), and the standard so-lution contains 1000. ng/L, what is [Ag⁺]ᵥᵥₐₛₜₑ?(e) Rewrite the equation in part (b) to find [Ag⁺]ᵥᵥₐₛₜₑ for a sys-tem in which T changes and Tᵥᵥₐₛₜₑ and T(standard) may be different.
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
The concentration of NO3- in a water sample was determined using ion-selective electrode. A 25.00 mL of the sample is placed in a beaker and a potential of 0.102 V is obtained. A 1.00 mL aliquot of a 200.0 mg/L standard solution of NO3- is added to this sample which gave a potential reading is 0.089 V. What is the concentration (ppm) of NO3- (FW = 62.00 g/mol) in the water sample?
Given the following: A cell SCE // Ag2CrO4 (saturated), CrO42- (xM) /AG is used for the determination of pCrO4- (ESCE = -0.244 V at 25 C). The half reaction at indicator electrode is: Ag2CrO4(s) + 2e-   2 Ag(s) + CrO42- (E0 = +0.446 V) What is pCrO4, given the cell potential of 0.402? What type of indicator electrode is Ag in this situation?
The concentration of nitrate, NO3-, in a water sample was determined using ion-selective electrode. A 25.00 mL of the sample is placed in a beaker and a potential of 0.102 V is obtained. A 1.00 mL aliquot of a 200.0 mg/L standard solution of NO3- is added to this sample which gave a potential reading is 0.089 V. What is the concentration (ppm) of NO3- (FW = 62.00 g/mol) in the water sample?
A pH meter is calibrated using a pH 4.00 buffer with 174.48 mV, pH 7.00 with 0 mV and pH 10.0 buffer with (-)174.48 mV. Calculate the Molar concentration of a HCl solution with electrode potential of 396.31 mV.
A Hittorf cell fitted with silver-silver chloride electrodes is filled with HCl solution that contains 0.3856 x 10-3 g HCL per g of water a current of 2 mA is passed for exactly three hours. The solutions are withdrawn, weighed and analysed. Total weight of the anode solution weighs 52.0461 g and contains 0.0133 g of HCl. Calculate the transference number of the H+