When a SBIA021 student measured the pH of 1.0M HCI, the student obtained a pH meter and failed to neither check the condition nor the manner of usage of the instrument. The pH meter reading timed out (Did not give a reading) Which of the following problem explanations is most correct? O The sample in the glass beaker was being swirled vigourously while the electrode was submerged in it for a reading O The electrode got submerged much deeper into the solution than it should have. O All of the above are correct problem explanations O The electrode had long direct contact with the environment and the glass membrane got dry

When a SBIA021 student measured the pH of 1.0M HCI, the student obtained a pH meter and failed to neither check the condition nor the manner of usage of the instrument. The pH meter reading timed out (Did not give a reading) Which of the following problem explanations is most correct? O The sample in the glass beaker was being swirled vigourously while the electrode was submerged in it for a reading O The electrode got submerged much deeper into the solution than it should have. O All of the above are correct problem explanations O The electrode had long direct contact with the environment and the glass membrane got dry

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 119QRT

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Similar questions

. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
Give three example solutions that fit each of the following descriptions. a. a strong electrolyte solution that is very acidic b. a strong electrolyte solution that is slightly acidic c. a strong electrolyte solution that is very basic d. a strong electrolyte solution that is slightly basic e. a strong electrolyte solution that is neutral
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
Consider a salt of a weak base and a weak acid such as ammonium cyanide. Both the NH4+ and CN ions interact with water in aqueous solution, but the net reaction can be considered as a proton transfer from NH4+ to CN. NH4+(aq) + CN(aq) NH3(aq) + HCN(aq) (a) Show that the equilibrium constant for this reaction, Kact, is 1. Knet=KaKbKw where Ka is the ionization constant for the weak acid NH4+ and Kb, is the constant for the weak base CN. (b) Calculate Knet values fur each of the following, NH4CN, NH4CH3CO2, and NH4K Which salt has the largest value of Kact, and why? (c) Predict whether a solution of each of the compounds in (b) is acidic or basic. Explain how you made this prediction (Yon do not need a calculation to make this prediction.)
8-60 How is the buffer capacity affected by the ratio of the conjugate base to the conjugate acid?
The titration of Na2CO3 with HCl bas the following qualitative profile: a. Identify the major species in solution at points AF. b. Calculate the pH at the halfway points to equivalence, B and D. (Hint: Refer to Exercise 113.)
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You have a solution of the weak acid HA and add some HCl to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
When might a pH meter be better than an indicator to determine the end point of an acid-base titration?
Sodium benzoate, NaC6H5COO (molar mass 144.1 g mol-1) is a common food preservative. The Ka of benzoic acid, C6H5COOH, is 1.6 X 10-5. A chemist titrates 25.00 mL of a stock solution of sodium benzoate, NaC6H5COO, with 1.20 M HCl solution using a pH meter and an indicator. f) A typical sodium benzoate solution used for preserving food has a concentration of 0.069 M (iii) Determine the mass of sodium benzoate present in this solution.