The cell SCE// Ag,CrO4 (sat’d), CrO, 2- (xM) /Ag is employed for the determination of pCrO4-. ESCE = 0.244 V at 25 0C The half reaction at indicator electrode Ag, CrO4 (s) + 2e- 2 Ag (s) + CrO,²- E°= +0.446 V a) Calculate pCrO, when the cell potential is 0.402 V b) What type of indicator electrode is Ag in this case?

The cell SCE// Ag,CrO4 (sat’d), CrO, 2- (xM) /Ag is employed for the determination of pCrO4-. ESCE = 0.244 V at 25 0C The half reaction at indicator electrode Ag, CrO4 (s) + 2e- 2 Ag (s) + CrO,²- E°= +0.446 V a) Calculate pCrO, when the cell potential is 0.402 V b) What type of indicator electrode is Ag in this case?

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter25: Voltammetry

Section: Chapter Questions

Problem 25.16QAP

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-.
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?
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
A 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.
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 ).
When the difference in pH across the membrane of a glass electrode at 25C is 4.63 pH units, how much voltage is generated by the pH gradient? Assume that the constant in Equation 15-6 is 1.00.
In a electrochemical cell are the molarity of the electrolyte CdCl2=0.10 kg/mole. Calculate the cellpotential at 25 degrees celcius when the activity coefficient for the proces are 0.10 mol/kg, CdCl2-solvent are decided to be 0.228, and the standard cell-potential are 0.624 V. Please answer very soon will give rating surely Show your work
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)
Calculate the potential of the indicator electrode at 25o C relative to SCE at the equivalence point of the titration of 25.00 ml of 0.010 Fe2+ with 0.010 M Cr2O72- in a solution that is buffered at pH 3.50.
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?
In the temperature range 0-90 ºC , the potential difference of the following cell:Pt (s) | H2 (g, f = 1) | HCl (aq, m = 0.1) | AgCl (s) | Ag (s)changes as follows with the temperature:Ecell (V) = 0.35510 – 0.3422x10-4t - 3.2347x10-8t2 + 6.314x10-9t3 (t being the temperature in ºC) Write the reaction and calculate ΔG, ΔH and ΔS at 90 ºC.Result: -34388 J/mol, 10.94 J/Kmol, -30.42 KJ/mol