Answer is eitherTrue or FalseCoulometry consumes larger amount ofanalyte than voltammetryElectrodes of the second kind can respondto the activities of anions that form sparingly7.soluble precipitatesThe equivalence point is at the first quarter ofthe steep part of the titration curve when thereaction stoichiometry is 1:1.3In order to be useful in endpoint detection, a redox indicator's range of color change should be at least doublethe potential expected at the end of the titrationMembrane indicator electrodes aresometimes called p-ion electrodes becausethey measure the pH onlyThe IR drop refers to the deviation of theelectrode potential from the value predictedby the Nernst equation on the passage of6current

All question are true/false questions based on electrochemistry. The knowledge of electrodes,…

Coulometry consumes larger amount of analyte than voltammetry Electrodes of the second kind can respond to the activities of anions that form sparingly soluble precipitates The equivalence point is at the first quarter of the steep part of the titration curve when the reaction stoichiometry is 1:1. 3

Coulometry consumes larger amount of analyte than voltammetry Electrodes of the second kind can respond to the activities of anions that form sparingly soluble precipitates The equivalence point is at the first quarter of the steep part of the titration curve when the reaction stoichiometry is 1:1. 3

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

In a redox titration, during the standardization of permanganate, how would the calculated molarity of KMnO4 be affected? 1. The KMnO4 is added too rapidly and too much KMnO4 is added, overshotting the end point. 2. Some of the solid Na2CO4 is spilled on the bench top after weighing but before beginning the titration.
Determine the iodine value of an unknown sample of oil weighing 0.21g if 26ml and 12 ml of 0.1100N of sodium thiosulfate are required for the blank and residual titration respectively.
A solution containing a mixture of metal cations was treated with dilute HCl and no precipitate formed. Next, H, S was bubbled through the acidic solution. A precipitate formed and was filtered off. Then, the pH was raised to about 8 and H, S was again bubbled through the solution. A precipitate again formed and was filtered off. Finally, the solution was treated with a sodium carbonate solution, which resulted in no precipitation. Classify the metal ions based on whether they were definitely present, definitely absent, or whether it is possible they were present in the original mixture. Definitely present Definitely absent Possibly present Ag* Hg²+ Lit Ba²+ Pb2+ Mg²+ Hg3* 2+ Answer Bank Zn2+ Sn2+ Ni2+ Cu2+ Bi3+ A13+ Incorrect
18.12 For the following, calculate the hydroxide, carbonate, and bicarbonate alkalinity by the procedures (1) using alkalinity measurements alone and (2) using alkalinity plus pH measurements. The sample size is 100 mL, 0.020 N H,SO, is used as the titrant, and the water temperature is 25°C (BG = bromcresol green). Total mL titrant to reach end point Sample Sample pH Phenol. BG A 11.9 10.0 11.2 7.0 10.0 14.4 8.2 15.5 38.6 8.4 B 12.7
In order to adjust the Potassium Permanganate solution, 0.0544g Na2C2O4 was taken and necessary experimental procedures were performed on it and the titrant consumption was found to be 7.9 mL. What is the KMnO4 concentration? A. 0.040B. 0.044C. 0.021D. 0.027
Add 0.3 M AgNO3 to each of the cold sample solutions until AgCl is observed to coagulate. Determine the approximate amount of needed AgNO3 by calculating the volume that would be required if the unknown were pure NaCl.
Determination of Water Hardness experiment was designed and suitable for bottled mineral water. What would you observe (and the changes in the result) if you performed complexometric titration based on the performed procedure on...a) distilled water b) tap water
49.97 ml of 0.08726 M potassium oxalate buffered at pH 8.27 is titrated with 0.07172 M potassium permanganate. What is the potential after 39.47 mL of potasslum permanganate has been added? Report just the potential in volts; don't Include the units (Canvas is challenged).
The concentration of CO in the air can be determined by passing a known volume of air through a tube containing I2O5, resulting in the formation of CO2 and I2. I2 is removed from the tube by distillation and collected in a solution containing excess KI, producing I3-. I3- is titrated with a standard solution of Na2S2O3. A 4.79 L air sample was sampled as described here, requiring 7.17 ml of 0.00329 M Na2S2O3 to reach the endpoint in a typical analysis. If the density of the air is 1.23×10^-3 g/ml, what is the amount of CO in the air in ppm? (CO: 28 g/ml)
Titration is the addition of a chemically equivalent volume of a solution of known concentration called analyte titrant fluent None of them
Mention the types of volumetric titration and briefly point out their differences.
A solution containing a mixture of metal cations was treated as outlined. 1. Dilute HCl was added and a precipitate formed. The precipitate was filtered off. 2. H, S was bubbled through the acidic solution. No precipitate formed. 3. The pH was raised to about 9 and H, S was again bubbled through the solution. A precipitate formed and was filtered off. 4. Finally, sodium carbonate was added to the filtered solution and no precipitate formed. What can be said about the presence of each of these groups of cations in the original solution? Cation group Description Present in the original solution? Ag*, Pb²+, Hgž+ form insoluble chlorides Bi3+, Cd2+, Cu²+, Hg²+, form acid-insoluble sulfides Pb2+, Sb³+, Sn²+, Snª+ Al3+, Co+, Cr³+, Fe²+, form base-insoluble sulfides Fe+, Ni?+, Mn²+, Zn²+ or hydroxides Ba?+, Ca2+, Mg²+, Sr²+ form insoluble carbonates Lit, Na+, K*, completely soluble Answer Bank None of these ions were present. unknown At least one of these ions was present. All of these ions…