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Which of the following
a. IV only
b. I and IV
c. I and II
d. I, II and IV
e. I, II, III and IV
Step by step
Solved in 2 steps
- Which of the following electrochemical methods requires the formation and measurement of an insoluble form of the analyte?I. coulometryII. voltammetry III. potentiometryIV. electrogravimetry17. 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 electrodeAll of the following can be used as indicator electrodes, except A. Ag/AgCl electrode B. Hg/HgCl electrode C. Cu/CuCl electrode D. Calomel electrode
- For indicator electrodes, which statements are true?I Indicator electrodes are made from relatively inert metals.II Indicator electrodes work best when the electrode surface is large and clean.III Platinum is a common indicator electrode.IV Platinum electrodes are more inert than gold electrodes. A. I, III, and IV B. I, II, and III C. I, II, III, and IV D. II and III E. I, II, and IVWhich electrode(s) will be useful to monitor the redox titration involving the species, Ce3+- Ce4+? I. Ag+ II. Pt III. Au IV. Cu2+ V. AgCl A. I and II B. II only C. II and III D. I and III E. I-VWhich of the following statements is/are correct for coulometry? I. Coulometric methods count the electrons used in a chemical reaction to measure the analyte. II. Coulometry uses constant current or constant potential conditions. III. An advantage of coulometric methods is low reproducibility and a disadvantage is low sensitivity. IV. Coulometric titrations are constant potential methods. V. Constant potential methods using a three-electrode cell are more selective than constant-current methods. A). I, II and V B). I, II, IV and V C). I, III and IV D.) II, IV and V
- 5. A solution of 0.100 M HCI and a solution of 0.100 M NAOH 14 are prepared. A 40.0 mL sample of one of the solutions is added to a beaker and then titrated with the other solution. A 12 pH electrode is used to obtain the data that are plotted in the 10 titration curve shown. 8. pH a. Identify the solution that was initially added to the beaker and which solution was in the buret. Explain your reasoning. 6. 2 b. At the equivalence point, how many moles of titrant 0- have been added? 20.0 40.0 60.0 80.0 Volume of Titrant Added (mL) c. The same titration is to be performed again, this time using an indicator. Use the information in the table below to select the best indicator for the titration. Explain your choice. pH Range of Color Change Indicator Methyl violet 0-1.6 Methyl red 4-6 Alizarin yellow 10 - 12Which of the following statements is/are correct for coulometry? I. Coulometric methods count the electrons used in a chemical reaction to measure the analyte. II. Coulometry uses constant current or constant potential conditions. III. An advantage of coulometric methods is low reproducibility and a disadvantage is low sensitivity. IV. Coulometric titrations are constant potential methods. V. Constant potential methods using a three-electrode cell are more selective than constant-current methods.4. Which of the following statement is true A. The change the in potential in equivalence-point region of an oxidation/reduction titration becomes larger as the reaction becomes more complete. the in potential in B. The change equivalence-point oxidation/reduction region titration of an becomes smaller as the reaction becomes more complete. C. The change in potential in equivalence-point oxidation/reduction constant as the reaction becomes more the of region titration an becomes complete. D. None of the above. 5. Which of the following statements are true: A. General oxidation/reduction indicators are substances that change color on being oxidized or reduced. B. The color changes of true redox indicators are largely independent of the chemical nature of the analyte and titrant. C. The color changes of true redox indicators are dependent on the changes in the electrode potential of the system that occur as the titration progresses D. All of the above
- Why do both Reference and Indicator electrodes need in Potentiometric titration? answer at your own words ans answer to the point not any irrelevant wordsHow many mL of 0.1200 M KSCN will be needed in the back titration after addition of 30 mL 0.110 M AgNO3 solution to 0.3655g KI dissolved in 100 mL water? a. 1.1951 mL b. 5.1919 mL c. 9.1519 mL d. 1.5911 mL1. Molarity of the NaOH solution 0.238 mol/L Trial 1 Trial 2 Trial 2. Volume of H;PO4 added to flask 22.0 mL 22.0 mL 22.0 mL 3. Initial NaOH volume _0.25_ mL _0.75_ mL 0.55 mL 4. Final NaOH volume 17.60_ mL 18.20_ mL _17.90_ mL 5. NAOH volume used for titration to reach green end point mL mL mL 6. NaOH volume used for titration 7. Moles of NaOH used for titration mol mel mel 8. Moles of H;PO4 that reacted mol mel mol 9. Volume of H;PO4 added to flask L 10. Molarity of H3PO4 mol/L mol/L mol/L