47. The figure shows a steady-state microelectrode voltammogram of a neurotransmitter obtained in a solution of 0.1 M KCl at 10 mV/s. Which best describes this voltammogram? Current, i (NA) 20 1.0 0.5 G.D 43 01 00 01 02 03 04 05 Potential, E (V) vs. Ag/AgCl (A) A scan-rate dependent oxidation wave with a cathodic limiting current of 2.0 nA and a standard oxidation potential of 0.20 V vs Ag/AgCl. (B) A scan-rate independent reduction wave with a cathodic limiting current of 2.0 nA and a standard reduction potential of 0.40 V vs Ag/AgCl. (C) A scan-rate independent oxidation wave with an anodic limiting current of 2.0 nA and a standard reduction potential of 0.20 V vs Ag/AgCl. (D) An irreversible scan-rate dependent oxidation wave with an anodic limiting current of 0.0 nA and unable

47. The figure shows a steady-state microelectrode voltammogram of a neurotransmitter obtained in a solution of 0.1 M KCl at 10 mV/s. Which best describes this voltammogram? Current, i (NA) 20 1.0 0.5 G.D 43 01 00 01 02 03 04 05 Potential, E (V) vs. Ag/AgCl (A) A scan-rate dependent oxidation wave with a cathodic limiting current of 2.0 nA and a standard oxidation potential of 0.20 V vs Ag/AgCl. (B) A scan-rate independent reduction wave with a cathodic limiting current of 2.0 nA and a standard reduction potential of 0.40 V vs Ag/AgCl. (C) A scan-rate independent oxidation wave with an anodic limiting current of 2.0 nA and a standard reduction potential of 0.20 V vs Ag/AgCl. (D) An irreversible scan-rate dependent oxidation wave with an anodic limiting current of 0.0 nA and unable

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter11: Dynamic Electrochemistry

Section: Chapter Questions

Problem 10P

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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.
What is the cell potential of the following cell at 25C? Ni(s)Ni2+(1.0M)Sn2(1.5104M)Sn(s)
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?
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 cell Ag|AgCl(sat’d)||H+(a = x)|glass electrode has a potential of —0.2094 V when the solution in the right-hand compartment is a buffer of pH 4.006. The following potentials are obtained when the buffer is replaced with unknowns: (a) —0.2806 V and (b) —0.2132 V. Calculate the pH and the hydrogen ion activity of each unknown. (c) Assuming anuncertainty of 0.001 Vin the junction potential, what is the range of hydrogen ion activities withinwhich the true value might be expected to lie?
89. The differential pulse polarogram of 3.00 mL of solution containing the antibiotic tetracycline in 0.1 M acetate, pH 4, gives a maximum current of 152 nA at half-wave potential of -1.05 V. (vs S.C.E). When 0.500 mL containing 2.65.ppm of tetracycline was added, the current increased to 206 nA. How much tetracycline, in ppm, is in the original solution? A. 1.95 C. 0.76 B. D. 7.45 1.24
The following cell was found to have a potential of 0.2897 V:SCEIIMg2+(a = 3.32 * 10^-3M)membrane electrode for Mg^2+(a) When the solution of known magnesium activity was replaced with an unknown solution, the potentialwas found to be 0.2041 V. What was the pMg of this unknown solution?(b) Assuming an uncertainty of 60.002 V in the junction potential, what is the range of Mg21 activitieswithin which the true value might be expected?(c) What is the relative error in [Mg^2+] associated with the uncertainty in Ej?
In a polarographic experiment of a 60 mL of 0.08 M Cu2+solution, a limitingcurrent was left on for 15 minutes. If the average current during the time of theexperiment is 6.0 μA, what fraction of the copper is removed from the solution? TheFaraday constant is 96485 C/mol of electron.
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)
13.28 For the cell Pt,|Fe²*(a = 2.00), Fe**(a = 1.20):|I"(a = 0.100)|1½(s)|Ptg %3D %3D R (a) write the cell reaction; (b) calculate E298 assuming the net liquid-junction potential is negligible. (c) Which terminal is at the higher potential? (d) When the cell is connected to a load, into which terminal do electrons flow from the load?
Determine the potential of a platinum electrode (vs. SHE) when placed in a mixture of 0.00207 M TICI, and 0.0362 M TICI at 25 °C. T13+ (aq) + 2e- = TIt (aq) E° = 1.25 V EPt = V Determine the potential of a platinum electrode when placed in a mixture of 0.0137 M potassium permanganate (KMNO,) and 0.0667 M manganese chloride (MnCl,) at pH 5.46 and 25 °C. Mno, (aq) + 5e- + 8 H* (aq) = Mn²+ (aq) + 4 H, O(1) E° = 1.51 V Ept = V
5) a) Typical Mg²+ concentrations in blood plasma are 2.2mM. If the transmembrane po- tential across the cell membrane is -90mV (negative inside), calculate the equilibrium con- centration of Mg²+ inside the red blood cell at 37°C. b) Consider the difference in electrochemical potential inside vs outside the cell, Aµreleefchem Helece/chem (inside) – Helec/chem(outside). As discussed in class, this difference is written as a chemical and electrical contribution, Afdee/chem = Aflchem + Atelec: For the red blood cell at equilibrium, state whether Atelee/chem; Atchem, and Aftelec are greater than, less than, or equal to zero, and explain your answer.