Explain the meaning of the advantages of coulometry * No need to prepare, standardize, or store standard solutions. * Can prepare unstable reagents in situ (original place) since they react almost as soon as they are generated - e.g., C12, Br2 * Straightforward to generate tiny quantities of reagent with good accuracy since it is easy to control current and time electronically. * A single coulometric titration apparatus can be used for redox, acid/base, precipitation, complexometric, etc., titrations.

Explain the meaning of the advantages of coulometry * No need to prepare, standardize, or store standard solutions. * Can prepare unstable reagents in situ (original place) since they react almost as soon as they are generated - e.g., C12, Br2 * Straightforward to generate tiny quantities of reagent with good accuracy since it is easy to control current and time electronically. * A single coulometric titration apparatus can be used for redox, acid/base, precipitation, complexometric, etc., titrations.

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

Chapter22: An Introduction To Electroanalytical Chemistry

Section: Chapter Questions

Problem 22.18QAP

See similar textbooks

Similar questions

3. A pH electrode system is calibrated with standard buffer solutions, with the following voltages observed for each: pH 4.01 = 111 mV; pH 7.00 = -55 mV; ph 10.01 = -215 mv. The electrode system generates a response of -30 mV when analyzing a soil solution. What is the pH of the solution? (
In this station, you will find a sample of table salt; the chemical formula of table salt is NaCl. Using the balance, weigh out 6.00 g of NaCl and dissolve in 50 mL of deionized (d.i.) water. Once com-pletely dissolved, add additional d.i. water to make the final volume of solution 100.0 mL. What is the mass percent NaCl in the solution? What is the molarity of the solution
1. A nitrate ion (NO;) selective electrode gives the following data of standard solutions. C (Concentration) (mM) 8. 16 E (Cell potential) (mV) 98.4 79.7 59.4 38.8 Find an unknown concentration of solution that gives a cell potential of 45.8 mV.
The concentration of H2S in wastewater samples was determined by coulometric titration using Kl as mediator and I3 as "titrant". standard concentration Peak area (a.u) (ppm) 50 8354 100 16925 150 25218 200 33584 250 42002 A 50 ml wastewater sample was placed in a coulometric cell, added with excess Kl and starch indicator. Electrolysis was carried out at a constant current of 84.6 mA for 386 s to reach the end point of the titration. What is the concentration of H2S in the sample (in ppm)?
Determine the transport numbers of the ions in an exactly 0.200 molal solution of copper (II) sulfate. The cell was filled with solution and electrolyzed between copper electrodes for some time. The cathode solution of the cell was found to weigh 36.434 g and contains 0.4415 g of Cu. Further the cathode in the coulometer showed an increase in weight of 0.0405 g due to deposited Ag.
Q4:-Put a mark of true or false in front of the following statements and correct the error, if any.- 1-In (Cathodic protection system) sacrificial anode, which is more voltage than the metal to be protected from corrosion 2-In oxidation-reduction reactions of solutions of strong acids, the oxygen ions are less reduced than the liberated hydrogen ions. 3-Techniques Tafel extrapolation test are used in corrosion rate measurements to overcoming the disadvantages of the Linear polarization method 4-A differential aeration cell,corrosion take place from electrode being thoroughly aerated to another de aerated. 5-Selective Leaching corrosion based on the more electrochemical component of an alloy is usually the element that is removed. 6-Electrolytic Cells are Non-spontaneous redox reactions and convert the chemical energy to electric energy. 7- Sour Corrosion term refer on corrosion due to gases which contain high concentrations of CO₂ alone, and called sour gas, while acid gas, can refer…
in ppm Pb(l) 5-31. Standard addition. The U.S. Environmental Protection water below which no adverse health effects are likely to occur. Agency sets guidelines for the level of contaminants in drinking using anodic stripping voltammetry, a very sensitive electro- chemical method. The blank-corrected current at -0.68 Vis The limit for thallium is 0.5 µg/L. Thallium (TI) was measured of 5.0 µL of a 100-µg/L TI standard were made to a 5.00-ml. proportional to the concentration of thallium. Repeated additions sample solution. Blank subtracted current (A) 0.08 0.06 0.04 0.02 0.00 -0.80 20-μL spike 15-μL spike 10-μL spike 5-μL spike No spike -0.60 -0.75 -0.70 -0.65 Voltage (V versus Ag | AgCl reference) -0.55 Standard additions of TI* to an unknown solution [Data from F. Ciepiela and K Węgiel, "Novel Method for Standard Addition Signal Analysis in Voltammetry Analyst 2017. 142, 1729.] (a) Measure the responses in the figure and prepare a graph to find out how much T1+ was in the unspiked…
Describe how you could use titration to calculate the concentration of an acidified tin (II) chloride sample solution with a standard potassium permanganate solution. Your answer should include: - a list of materials and equipment. - a sample step-by-step procedure - a balanced spontaneous redox reaction equation using half reactions - One observations of reaction evidence - one lab safety concern using this technique
2. The formation of insoluble MgNH,PO,-6H,0, which is ignited to Mg.P.O, for weighing, can be used for the determination of Mg, N, or P. Write appropriate gravimetric factor that would apply to each determination.
17. The actual design of the indicator electrode referred to the pH electrodes cell, in the following convenient writing form is missing. (-) ( ) | test solution H* (x=mol/L) || SCE (+) A. potential redox C. glass membrane electrode B. cathode D. reference electrode
3 Suppose at 25 oC and 1.0 bar pressure that the Galvanic cell: Mn|MnCl2||LiCl||ZnCl2|Zn is constructed. Use your table of Standard Reduction Potentials to determine the cell reaction in this case. Write the balanced net ionic equation for that reaction in the answer box. Place any needed superscript charges in your equation using the formatting palette above the text area using the: x2 button. Place subscript phases of materials in your equation using the formatting palette above the text area using the x2 button. You should also put an arrow (→) in your equation using the formatting palette above the text area using the Ω button.
What is precipitation from homogeneous solution; what are the benefits of this method.