1. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 13 Practice Test Assignment #5 Test: 4/12/16

2. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 1.The rule like dissolves like is used to predict a.solubility. b. equilibrium. c. reactivity. d. phase. Standardized Test Preparation Understanding Concepts Chapter 12

3. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 1.The rule like dissolves like is used to predict a.solubility. b. equilibrium. c. reactivity. d. phase. Standardized Test Preparation Understanding Concepts Chapter 12

4. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 2. What is the molarity of a solution that contains 0.202 mol KCl in 7.98 L of solution? a.0.0132 M b.0.0253 M c.0.459 M d.1.363 M Standardized Test Preparation Understanding Concepts Chapter 12

5. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 2. What is the molarity of a solution that contains 0.202 mol KCl in 7.98 L of solution? a.0.0132 M b.0.0253 M c.0.459 M d.1.363 M Standardized Test Preparation Understanding Concepts Chapter 12

6. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 3.There are 3.4 mg of lead present in 2000 g of a water sample. What is the concentration of lead in ppm? a.1.7 ppm b. 1.7 x 10 -3 ppm c. 3.4 ppm d. 3.4 x 10 -3 ppm Standardized Test Preparation Understanding Concepts Chapter 12

7. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 3.There are 3.4 mg of lead present in 2000 g of a water sample. What is the concentration of lead in ppm? a.1.7 ppm b. 1.7 x 10 -3 ppm c. 3.4 ppm d. 3.4 x 10 -3 ppm Standardized Test Preparation Understanding Concepts Chapter 12

8. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 4. Which of the following does NOT express concentration? a.molality b. molarity c. parts per million d. solubility Standardized Test Preparation Understanding Concepts Chapter 12

9. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 4. Which of the following does NOT express concentration? a.molality b. molarity c. parts per million d. solubility Standardized Test Preparation Understanding Concepts Chapter 12

10. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 5.You know the number of grams of solute and the volume of solution. What is the first step in finding the molarity of the solution? a.Divide grams by molar mass to determine number of moles. b. Divide grams by the volume of solution. c. Divide the volume of solution by grams. d. Divide the number of moles by the volume of solution. Standardized Test Preparation Understanding Concepts Chapter 12

11. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 5.You know the number of grams of solute and the volume of solution. What is the first step in finding the molarity of the solution? a.Divide grams by molar mass to determine number of moles. b. Divide grams by the volume of solution. c. Divide the volume of solution by grams. d. Divide the number of moles by the volume of solution. Standardized Test Preparation Understanding Concepts Chapter 12

12. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 6. A 0.15 M solution of HCl reacts with an excess of calcium carbonate, CaCO 3. A volume of 25.0 mL of HCl is used. To determine the number of moles of CaCl 2 produced, you need to know a.the amount of the other product produced. b. the molar mass of HCl. c. the molar mass of CaCl 2. d. the balanced chemical equation. Standardized Test Preparation Understanding Concepts Chapter 12

13. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 6. A 0.15 M solution of HCl reacts with an excess of calcium carbonate, CaCO 3. A volume of 25.0 mL of HCl is used. To determine the number of moles of CaCl 2 produced, you need to know a.the amount of the other product produced. b. the molar mass of HCl. c. the molar mass of CaCl 2. d. the balanced chemical equation. Standardized Test Preparation Understanding Concepts Chapter 12

14. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 7. The solubility of a solute depends on a.the nature of the solute and the temperature of the solvent. b.the nature of the solute only. c.the temperature of the solvent only. d.neither the nature of the solute nor the temperature of the solvent. Standardized Test Preparation Understanding Concepts Chapter 12

15. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 7. The solubility of a solute depends on a.the nature of the solute and the temperature of the solvent. b.the nature of the solute only. c.the temperature of the solvent only. d.neither the nature of the solute nor the temperature of the solvent. Standardized Test Preparation Understanding Concepts Chapter 12

16. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 8. A solution of would not conduct an electric current. a.NaCl b. HCl c. C 6 H 12 O 6 d. CsI Standardized Test Preparation Understanding Concepts Chapter 12

17. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 8. A solution of would not conduct an electric current. a.NaCl b. HCl c. C 6 H 12 O 6 d. CsI Standardized Test Preparation Understanding Concepts Chapter 12

18. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 9. Which of the following factors does not, in general, increase the solubility of a solid in a liquid? a.increasing temperature b. increasing surface area c. increasing pressure d. shaking or stirring Standardized Test Preparation Understanding Concepts Chapter 12

19. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 9. Which of the following factors does not, in general, increase the solubility of a solid in a liquid? a.increasing temperature b. increasing surface area c. increasing pressure d. shaking or stirring Standardized Test Preparation Understanding Concepts Chapter 12

20. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 10. A dissolved solute that completely dissociates into ions is a.a nonelectrolyte. b. a weak electrolyte. c. a strong electrolyte. d. insoluble. Standardized Test Preparation Understanding Concepts Chapter 12

21. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 10. A dissolved solute that completely dissociates into ions is a.a nonelectrolyte. b. a weak electrolyte. c. a strong electrolyte. d. insoluble. Standardized Test Preparation Understanding Concepts Chapter 12

22. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 11. A mixture that appears to be uniform while being stirred but separates into different phases when agitation ceases is a a.solvent. b. colloid. c. suspension. d. solute. Standardized Test Preparation Understanding Concepts Chapter 12

23. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 11. A mixture that appears to be uniform while being stirred but separates into different phases when agitation ceases is a a.solvent. b. colloid. c. suspension. d. solute. Standardized Test Preparation Understanding Concepts Chapter 12

24. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 12. 210 mL of a 0.100 M solution of copper(II) nitrate reacts with an excess of iron. What is the molarity of the 0.575 L of iron(III) nitrate produced? Standardized Test Preparation Understanding Concepts Chapter 12

25. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 12. 210 mL of a 0.100 M solution of copper(II) nitrate reacts with an excess of iron. What is the molarity of the 0.575 L of iron(III) nitrate produced? =0.024 M Standardized Test Preparation Understanding Concepts Chapter 12

26. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 13. How many grams of CaCl 2 are needed to prepare 1.00 L of a 1.00 M solution? Standardized Test Preparation Understanding Concepts Chapter 12

27. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 13. How many grams of CaCl 2 are needed to prepare 1.00 L of a 1.00 M solution? =111 g CaCl 2 Standardized Test Preparation Understanding Concepts Chapter 12

28. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 14. Describe how you would prepare a 0.50 M solution of potassium iodide. Standardized Test Preparation Understanding Concepts Chapter 12

29. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 14. Describe how you would prepare a 0.50 M solution of potassium iodide. Add 166 g of potassium iodide to a flask and then add enough solvent to bring the total volume of the solution up to 2.0 L. Standardized Test Preparation Understanding Concepts Chapter 12

30. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 15. How many grams of MgCl 2 will be formed from 25.6 mL of a 0.100 M HCl solution reacting with excess magnesium metal? The other product is hydrogen gas. Standardized Test Preparation Understanding Concepts Chapter 12

31. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 15. How many grams of MgCl 2 will be formed from 25.6 mL of a 0.100 M HCl solution reacting with excess magnesium metal? The other product is hydrogen gas. =0.122 g MgCl 2 Standardized Test Preparation Understanding Concepts Chapter 12