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

10th Edition

ISBN:9781305957404

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

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

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 29Q: Give three example solutions that fit each of the following descriptions. a. a strong electrolyte...

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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
. 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.
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.
An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker at various times during the titration. These are presented out of order. Note: Counter-ions and water molecules have been omitted from the illustrations for clarity. (a) (b) (c) (d) (e) a. Is the acid a weak or strong acid? How can you tell? b. Arrange the beakers in order of what the contents would look like as the titration progresses. c. For which beaker would pH = pKa? Explain your answer. d. Which beaker represents the equivalence point of the titration? Explain your answer. e. For which beaker would the Ka value for the acid not be necessary to determine the pH? Explain your answer.
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.)
A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?
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.)
Repeat the description for Question 4, but use a weak acid rather than a strong one.
One half liter (500. mL) of 2.50 M HCl is mixed with 250. mL of 3.75 M HCl. Assuming the total solution volume after mixing is 750. mL, what is the concentration of hydrochloric acid in the resulting solution? What is its pH?
. Calculate the pH of each of the following solutions from the information given. a. [H+]=4.78102M b. pOH = 4.56 c. [OH]=9.74103M d. [H+]=1.24108M
. What does it mean to say that an acid is strong in aqueous solution? What does this reveal about the ability of the acids anion to attract protons?