{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

Chapter 4A TAVSS

Chapter 4A TAVSS - CHEM 161-2007 CHAPTER 4A CHEMICAL...

Info icon This preview shows pages 1–5. Sign up to view the full content.

View Full Document Right Arrow Icon
CHEM 161-2007 CHAPTER 4A - CHEMICAL REACTIONS IN AQUEOUS SOLUTIONS PRACTICE PROBLEMS DR. ED TAVSS Strong and weak electrolytes Precipitation reactions Acid-Base reactions (Also, see Chapter 3B, Solution Conc.: Molarity)
Image of page 1

Info icon This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
Strong and weak electrolytes CHEM 161-2006 EXAM II HILL & PETRUCCI CHAPTER 4 TYPES OF CHEMICAL REACTIONS AND SOLUTION STOICHIOMETRY STRONG AND WEAK ELECTROLYTES 12. Which one of the following 0.10 M aqueous solutions is a non-electrolyte? (a) NaCl (b) MgSO 4 (c) CH 3 COOH (d) C 12 H 22 O 11 (e) HCl (a) NaCl is a soluble salt. All soluble salts are strong electrolytes. (b) MgSO 4 is a soluble salt. All soluble salts are strong electrolytes. (c) CH 3 COOH is a weak acid. All weak acids are weak electrolytes. (d) C 12 H 22 O 11 is an organic molecule. Virtually all organic molecules, except for organic acids, are non-electrolytes. (e) HCl is a strong acid. All strong acids are strong electrolytes. 18. Chem 161-2004 Exam I Zumdahl 6 th edition Chapter 4 Strong and Weak Electrolytes Consider two organic molecules, ethanol and benzene. One dissolves in water and the other does not. Why? A. One is ionic, the other is not. B. They have different molar masses. C. Choose this choice if more than one of the other reasons given is correct. D . One contains a polar O-H bond and the other does not E. One is an electrolyte, the other is not A. Neither one is ionic. B. Although they have different molar masses, molar mass is only a small factor in determining solubility. D. The ethanol is a polar molecule. Water is a polar molecule. Polar molecules dissolve in water. Benzene is not polar. Non-polar molecules do not dissolve in water. E. They are both organic molecules. Neither one is an organic acid or base. Hence, neither one ionizes, and therefore neither one is an electrolyte.
Image of page 2
CHEM 161-1999 FINAL EXAM + ANSWERS CHAPTER 4 - TYPES OF CHEMICAL REACTIONS AND SOLUTION STOICHIOMETRY STRONG AND WEAK ELECTROLYTES 14. Which one of the following is a weak electrolyte when dissolved in water? A. Hydrogen chloride. B . Ammonia. C. Sodium sulfate. D. Perchloric acid. E. Potassium hydroxide. CHEM 161-2001-HOURLY EXAM I + ANSWERS ZUMDAHL CHAPTER 4 - TYPES OF CHEMICAL REACTIONS AND SOLUTION STOICHIOMETRY STRONG AND WEAK ELECTROLYTES 18. Of the substances below, which ones are the weak electrolytes? V. AgCl W. glucose (C 6 H 12 O 6 ) X. HI Y. H 3 PO 4 Z. NH 3 A. none of them B. all of them C. W and Y D . Y and Z E. V and W A strong electrolyte is one that is available in solution almost exclusively as ions (by ionizing completely). A solution of a strong electrolyte is a good electrical conductor. A non-electrolyte
Image of page 3

Info icon This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
is one which provides no ions in the solution (i.e., it doesn’t ionize at all). Therefore a solution of a non-electrolyte doesn’t conduct electricity. A weak electrolyte is one that provides very few ions in solution, by ionizing weakly. A weak electrolyte is a weak electrical conductor. Silver chloride, as an option, created a lot of controversy in this exam. Since it is a salt, what little of it dissolves ionizes completely, and therefore may be considered as being a strong electrolyte.
Image of page 4
Image of page 5
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}

What students are saying

  • Left Quote Icon

    As a current student on this bumpy collegiate pathway, I stumbled upon Course Hero, where I can find study resources for nearly all my courses, get online help from tutors 24/7, and even share my old projects, papers, and lecture notes with other students.

    Student Picture

    Kiran Temple University Fox School of Business ‘17, Course Hero Intern

  • Left Quote Icon

    I cannot even describe how much Course Hero helped me this summer. It’s truly become something I can always rely on and help me. In the end, I was not only able to survive summer classes, but I was able to thrive thanks to Course Hero.

    Student Picture

    Dana University of Pennsylvania ‘17, Course Hero Intern

  • Left Quote Icon

    The ability to access any university’s resources through Course Hero proved invaluable in my case. I was behind on Tulane coursework and actually used UCLA’s materials to help me move forward and get everything together on time.

    Student Picture

    Jill Tulane University ‘16, Course Hero Intern