14-2. Convert the following potentials. The Ag | AgCl and calomelreference electrodes are saturated with KCI.(a) 0.523 V versus S.H.E. = ? versus Ag | A£CI(b) –0.111 V versus Ag | AgCl = ? versus S.H.E.(c) –0.222 V versus S.C.E. = ? versus S.H.E.(d) 0.023 V versus Ag | AgCl = ? versus S.C.E.? versus Ag | A£CI(e) –0.023 V versus S.C.E. =

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Answered: 14-2. Convert the following potentials.…

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter10: Potentiometry And Redox Titrations

Section: Chapter Questions

Problem 3P

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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
Galvanic cells harness spontaneous oxidationreduction reactions to produce work by producing a current. They do so by controlling the flow of electrons from the species oxidized to the species reduced. How is a galvanic cell designed? What is in the cathode compartment? The anode compartment? What purpose do electrodes serve? Which way do electrons always flow in the wire connecting the two electrodes in a galvanic cell? Why is it necessary to use a salt bridge or a porous disk in a galvanic cell? Which way do cations flow in the salt bridge? Which way do the anions flow? What is a cell potential and what is a volt?
. Calculate the potential of the following cells. Assume a temperature of 25°C and that activities equal the concentration. a. SCE|| Fe³+ (0.0250 M), Fe²* (0.0150 M) | Pt b. Saturated Ag-AgCl reference || Ti³ (0.0250 M), Ti²*(0.0450 M) | Pt Ti³ + e Ti²+ Eº = -0.369V
Convert the potentials listed below. The Ag | AgCl and calomel reference electrodes are saturated with KCl. (i) 0.523 V versus S.H.E. 5 ? versus Ag | AgCl (ii) 0.222 V versus S.C.E. 5 ? versus S.H.E.
What is the schematic representation of a cell with a saturated calomel electrode as the reference electrode and a silver indicator electrode to measure the p-function of [CrO4²-]? SCE | Ag2CrO4(sat'd), CrO42-(x M)| Ag O SCE || Ag2 CrO4(s), CrO4²-(x M)| Ag SCE ||Ag2 CrO4(sat'd), CrO4²-(x M) | Ag SCE || Ag2CrO4(s), CrO4²-(x M) | Ag
13.Dependence of emf on concentration | Nernst equation Given: Cr3+(aq)+3e-Cr(s); E= -0.74V Ag+(aq)+e-Ag(s); E= 0.80V What is the cell potential at 25Cfor the following cell? Cr(s)| Cr3+(0.010M)| | Ag+(0.00020M)| Ag(s)
solve very very fast in 15 min | I need a clear answer by hand, not by keyboard
Determine the potential of a platinum electrode (vs. SHE) when placed in a mixture of 0.00385 M TIC1, and 0.0431 M TICI at 25 °C. T1³+ (aq) + 2 e Tl* (aq) Ept Ept 1.2803 Incorrect || Determine the potential of a platinum electrode when placed in a mixture of 0.0173 M potassium permanganate (KMnO4) and 0.0876 M manganese chloride (MnCl₂) at pH 3.72 and 25 °C. E° = 1.25 V 2+ MnO4 (aq) + 5e + 8 H¹ (aq) = Mn²+ (aq) + 4H₂O(1) Incorrect V E° = 1.51 V V
The cell Ag|AgCl(sat'd)||H+(a=x)glass electrode has a potential of -0.2094V when tne solution in the right hand compartment is a buffer of pH 4.006. The following potential are obtained when the buffer is replaced with unknowns:(a)-0.2806V and (b)-0.2132V. Calculate the pH and the hydrogen ion activity of each unknown.(c)Assuming an uncertainty of 0.001V in the junction potential,what is range of hydrogen ion activities within which the true value might be expected to lie?
A soluion of 10.0 mL of 0.0500 mol/L AgNO3 is titrated with 0.0250 mol/L NaBr in the cell: VKE||onbekende oplossing||Ag(s) Calculate the potential of the cell after adding 0.1 mL, 10.0 mL, 20.0 mL and 30.0 ml of titrant. E\deg (Ag+, Ag = 0.799 V; E(VKE = 0.244 V; Ksp(ABr) = 5.0*10-13
Calculate the theoretical cell potential of the following cells. If the cell is short-circuited, indicate the direction of the spontaneous cell 12-5. reaction. (a) Zn Zn2+ (0.0955 M) || Co²+(6.78 × 10-3 M)|Co (b) Pt|Fe*(0.1310 M), Fe²*(0.0681 M) || Hg²+(0.0671 M)|Hg

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