The following data were measured in a 1.00-cm cell. Concentration (M) %T 1.50x10-4 14.9 1.00x10-4 26.1 7.50x10-5 38.0 5.00x10-5 54.3 3.00x10-5 65.7 Determine the molar absorptivity( in cm ¹M¹) using graphical methods. Question 5 Using the information, from question 4, calculate the % transmittance for a 2.1x10-4M solution.

The following data were measured in a 1.00-cm cell. Concentration (M) %T 1.50x10-4 14.9 1.00x10-4 26.1 7.50x10-5 38.0 5.00x10-5 54.3 3.00x10-5 65.7 Determine the molar absorptivity( in cm ¹M¹) using graphical methods. Question 5 Using the information, from question 4, calculate the % transmittance for a 2.1x10-4M solution.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.15QAP

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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?
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Zn|Zn2+(0.50M)Cd2+(0.020M)|Cd (b) Cu|Cu2+(0.0010M)H+(0.010M)|H2(1.00atm)|Pt
A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.
What is the cell potential of the following cell at 25C? Ni(s)Ni2+(1.0M)Sn2(1.5104M)Sn(s)
For the cell: Cr|Cr3+Co2+|Co E° is 0.46 V. The same cell was prepared in the laboratory at standard conditions. The voltage obtained was 0.40 V. A possible explanation for the difference is (a) the surface area of the chromium electrode was smaller than the cobalt electrode. (b) the mass of the chromium electrode was larger than the mass of the cobalt electrode. (c) the concentration of Cr(NO3)2 solution used was less than 1.0 M. (d) the concentration of Cr(NO3)2 solution used was less than 1.0 M. (e) the volume of Cr(NO3)2 solution used was larger than the volume of Cr(NO3)2 solution used.
Which of the changes below will increase the voltage of the following cell? Co|Co2+(0.010M)H+(0.010M)|H2(0.500atm)|Pt (a) Increase the volume of COCl2 solution from 100 mL to 300 mL. (b) Increase [H+] from 0.010 M to 0.500 M. (c) Increase the pressure of H2 from 0.500 atm to 1 atm. (d) Increase the mass of the Co electrode from 15 g to 25 g. (e) Increase [CO2+] from 0.010 M to 0.500 M.
The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making electrochemica1 measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCI. is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case. indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in Table 17.1. a. Cu2++2eCu b. Fe3++e-Fe2+ c. AgCl+e-Ag+Cl- d. Al3++3eAl e. Ni2++2eNi
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
A silver coulometer (Study Question 106) was used in the past to measure the current flowing in an electrochemical cell. Suppose you found that the current flowing through an electrolysis cell deposited 0.089 g of Ag metal at the cathode after exactly 10 min. If this same current then passed through a cell containing gold(III) ion in the form of [AuCl4], how much gold was deposited at the cathode in that electrolysis cell?

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