Ionic Equilibria Chapter Exam

Exam Instructions:

Choose your answers to the questions and click 'Next' to see the next set of questions. You can skip questions if you would like and come back to them later with the yellow "Go To First Skipped Question" button. When you have completed the practice exam, a green submit button will appear. Click it to see your results. Good luck!

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Question 1 1. What does a buffer do?

Question 2 2. How do you calculate the pH of a buffered solution?

Question 3 3. What is NOT true about buffered solutions that is true about other solutions in equilibrium?

Question 4 4. When hydronium ions are produced by the conjugate acid of a salt, the solution becomes more

Question 5 5. Salt hydrolysis is a reaction where

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Question 6 6. Sodium acetate, or CH3COONa, comes from a weak acid and a strong base. When this salt dissociates, the solution becomes more,

Question 7 7. How is the Bronsted-Lowry definition of an acid different from the Arrhenius definition?

Question 8 8. What is a Lewis acid-base reaction?

Question 9 9. According to Bronsted and Lowry, which of the following is a base?

Question 10 10. Which of the following is NOT a common property of acids?

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Question 11 11. A lab technician immerses an Arrhenius base in a beaker of water. What sort of ions would the lab technician find in the beaker?

Question 12 12. What information would you need to determine if a base is strong or weak?

Question 13 13. What is a common ion?

Question 14 14. When does a precipitate form?

Question 15 15. What is the net effect of the common ion?

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Question 16 16. The equilibrium constant tells us _____

Question 17 17. Ostwald's Law of Dilution states that, if we know the equilibrium constant for a substance, we can calculate the extent of its dissociation (or association, in the case of a weak base, for example) if we also know its _____.

Question 18 18. Ostwald's Law of Dilution cannot be used when?

Question 19 19. Why doesn't oil dissolve in water?

Question 20 20. What does it mean to be a polar molecule?

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Question 21 21. What holds a water molecule together?

Question 22 22. How is solubility determined?

Question 23 23. Which of the following statements best describes a supersaturated solution?

Question 24 24.

Suppose a solution at 50℃ contains 12g Potassium dichromate (K₂Cr₂O₇) per 100g of water.

Based on the provided solubility curve, how much additional mass of Potassium dichromate would be required to saturate the solution at the same temperature?

Question 25 25. What is the hydronium ion concentration or [H3O+] of juice pH 2.25?

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Question 26 26. What is the pH of a 0.3 M solution of a strong acid?

Question 27 27. Which of the following does pH measure?

Question 28 28. What is a buffer?

Question 29 29. What determines the pH of a solution when the salt that dissociates is formed from a weak acid and weak base?

Question 30 30. What is a conjugate base?

Ionic Equilibria Chapter Exam Instructions

Choose your answers to the questions and click 'Next' to see the next set of questions. You can skip questions if you would like and come back to them later with the yellow "Go To First Skipped Question" button. When you have completed the practice exam, a green submit button will appear. Click it to see your results. Good luck!

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