Which statement is NOT correct? pH meter should always be standardized before using to make sure that your readings are accurate and repeatable. The electrode tips should never touch the bottom or sides of a beaker. When finished using the pH meter, rinse the electrode and place it in the pH 7 buffer solution on standby. One buffer solution is enough to standardize a pH meter before using.

Which statement is NOT correct? pH meter should always be standardized before using to make sure that your readings are accurate and repeatable. The electrode tips should never touch the bottom or sides of a beaker. When finished using the pH meter, rinse the electrode and place it in the pH 7 buffer solution on standby. One buffer solution is enough to standardize a pH meter before using.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter22: Bulk Electrolysis: Electrogravimetry And Coulometry

Section: Chapter Questions

Problem 22.26QAP

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2.1 Calculate the pH of 1.0 M HC2H3O2 solution, using Ka = 1.7 × 10-5 . Begin this calculation by defining the variable x. List the pH answer as “theoretical pH” on the report sheet. Have the instructor check this answer and all subsequent calculations. To test your prediction, obtain about 35 mL 1.0 M HC2H3O2 and add to a clean, dry 50 mL beaker. Measure the pH of this solution. Be sure the electrode is properly submerged and gives a stable reading. Record the pH reading in the “Observed pH” column on the report sheet. The value should be within ± 0.2 pH units of the calculated value. From the experimental pH and beginning concentrations of the solution components, calculate the remainder of the entries across the table to pKa . Save this solution for Sections 2.3 and 2.6. 2.2 Calculate the pH of 0.10 M HC2H3O2 solution. List this answer as “theoretical pH” on the report sheet. Test your prediction by placing 5 mL of 0.10 M HC2H3O2 in a test tube and testing its…
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Which of the following statements is correct for the titration of Fe2+ ion with standard Ce4+ ion? I- The indicator electrode potential is calculated using the Fe3+ half-reaction after calculating the equilibrium concentrations of Fe3+ and Fe2+ in the solution before the Ce4+ solution is added. II- Before the equivalence point, the indicator electrode potential is calculated using the Fe3+ half-reaction since [Fe3+] and [Fe2+] are known. III- At the equivalence point, the indicator electrode potential is the average of the E0 values of Fe3+ and Fe2+. IV- After the equivalence point, the indicator electrode potential is calculated using the Ce4+ half-reaction since [Ce3+] and [Ce4+] are known.
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Which of the following statements are correct for the titration of Fe2+ ion with standard Ce4+ ion? I- Indicator electrode potential is calculated using the Fe3+ half-reaction after calculating the equilibrium concentrations of Fe3+ and Fe2+ in the solution before the Ce4+ solution is added. II- Before the equivalence point, the indicator electrode potential is calculated using the Fe3+ half-reaction since [Fe3+] and [Fe2+] are known. III- At the equivalence point, the indicator electrode potential is the average of the E0 values of Fe3+ and Fe2+ IV- After the equivalence point, the indicator electrode potential is calculated using the Ce4+ half-reaction since [Ce3+] and [Ce4+] are known. A.II and IVB. I, II, III and IVC. I, III and IVD. II, III and IV
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		pH meter should always be standardized before using to make sure that your readings are accurate and repeatable.
		The electrode tips should never touch the bottom or sides of a beaker.
		When finished using the pH meter, rinse the electrode and place it in the pH 7 buffer solution on standby.
		One buffer solution is enough to standardize a pH meter before using.