Chapter #17 Solutions - Physical Science with Modern Applications - Melvin Merken - 5th Edition

 

1. Are all liquids soluble in one another? Explain. Get solution

2. Gasoline is a nonpolar solvent; water is a polar solvent. Is KCl more likely to be soluble in gasoline or in water? Get solution

3. Compare the solubility of common table salt, NaCl, with that of naphthalene (moth flakes), C10H8, in (a) water, (b) gasoline. Get solution

4. How do a mixture, a solution, and a pure compound differ in composition? Get solution

5. Explain what “like dissolves like” means. Get solution

6. Give an example of solvation involving ion-dipole interaction. Get solution

7. A solution is made by dissolving sugar in water. Which is the solvent and which the solute? Get solution

8. Suppose a solution contains either stilt or sugar dissolved in water. Suggest a simple way by which you could easily tell which it is. Get solution

9. One mole of sugar is added to 1 liter of water. Is the concentration of the solution 1 M? Explain. Get solution

10. Calculate (a) the number of moles and (b) the number of grams of NaCl in 50.0 mL of 2.00 M NaCl. Get solution

11. Describe how you would prepare 250 mL of 0.100 M NaOH from solid NaOH and water. Get solution

12. A sample of rainwater has a nitric acid concentration of 3.00 × 10−8 M. How many grams of nitric acid are present in 1 liter? Get solution

13. Explain how you would make a 1.50-m calcium chloride solution. Get solution

14. How many grams of water would you have to add to 1000 g of sugar, C12H22O11, in order to prepare a 1-m solution? Get solution

15. How many molecules of ethyl alcohol, C2H5OH, must be dissolved in 500 g of water to make a 1-m solution? Get solution

16. An analysis of rainwater revealed a concentration of nitric acid, HNO3, of 2.2 × 10−6 g/liter. What is the molarity with respect to the nitric acid? Get solution

17. What is the meaning of the word “colligative” in the context of colligative properties? Get solution

18. Explain why seawater has a lower freezing point than fresh water. Get solution

19. How can you determine experimentally whether a substance is an electrolyte or a nonelectrolyte? Get solution

20. Which will freeze faster, a fresh-water pond or a salt-water pond? Get solution

21. How does the spreading of salt on ice-covered walks and roads cause the ice to melt? Get solution

22. Discuss the principle whereby the addition of antifreeze to an automobile radiator exerts its action. Get solution

23. The solution in a car radiator froze at 0°F. Determine the molality of the solution. Get solution

24. A solution contains 684 g of sucrose, C12H22O11, per 1000 g of water. Determine the freezing point of the solution. Get solution

25. A solution is made by dissolving 45.0 g of dextrose (C6H12O6) in 250.0 g of water.(a) Calculate the molality.(b) At what temperature will the solution freeze? Get solution

26. Which solution would produce the brighter light in an electrical conductivity apparatus, 0.100 M NaCl or 0.100 M Na3PO4? Explain. Get solution

27. List some general properties of acids. Get solution

28. List some general properties of bases. Get solution

29. In the Arrhenius definition, (a) what characterizes an acid; (b) what characterizes a base? Get solution

30. What does it mean to say that an acid is strong in aqueous solution? Get solution

31. When aqueous solutions of sodium chloride and silver nitrate are mixed, a precipitate forms instantaneously. How does the Arrhenius theory explain this result? Get solution

32. Complete and balance the following equations representing neutralization reactions:(a) HCl + Ca(OH)2 →(b) NH3 + H2SO4 →(c) NaOH + HNO3 →(d) H3PO4 + LiOH → Get solution

33. Why is the acidity of a solution expressed in terms of its pH rather than in terms of the molarity of hydrogen ion present? Get solution

34. How is pH defined? Get solution

35. Vinegar is an aqueous solution of acetic acid. Would you expect the pH of vinegar to be greater than or less than 7.00? Get solution

36. State whether each of the following solutions is acidic or basic. The H+ concentrations are given.(a) [H+] = 1.00 × 10−4 M(b) [H+] = 1.00 × 10−11 M(c) [H+] = 3.50 × 10−13 M(d) [H+] = 0.0001 M Get solution

37. Classify the following aqueous solutions as acidic, basic, or neutral if their pH is(a) 11. (b) 2. (c) 7. (d) 8.24. (e) 3.48. Get solution

38. Why can boric acid (H3BO3) be used in eyewashes, whereas hydrochloric acid (HCl) is not safe to use? Get solution

39. How do soaps and detergents cleanse? Get solution

40. In regions where the water supply is rich in calcium or magnesium compounds, why are detergents better cleaning agents than soaps? Get solution

41. Of what importance is biodegradability to the for-mulators of detergents? Get solution

42. What are the disadvantages of hard water? Get solution

43. What is the environmental impact of phosphorus compounds in detergents? Get solution

44. Why is an algal bloom—a thick mat of blue-green algae—on the surface of a lake an undesirable sign? Get solution

45. Plow can eutrophication lead to the death of a lake? Get solution

46. Multiple ChoiceA. Which of the following would be most soluble in the polar solvent water?(a) I2 (b) NaCl (c) CCl4 (d) N2B. The freezing point of H2o is(a) lowered by the addition of a solute.(b) raised by the addition of a solute.(c) not affected by the addition of a solute.(d) does not depend on the amount of solute added.C. When 1 mole of NaCl is dissolved in a kilogram of water, the concentration is(a) 0.50 molal.(b) 0.50 molar.(c) 1.00 molal.(d) 1.00 molar.D. A solution that has a pH of 7 is(a) slightly acidic.(b) strongly acidic.(c) neutral.(d) slightly basic.E. Kw(a) equals 10−14.(b) is the ion product of water.(c) equals [H3o+][OH-].(d) all of theseF. Which of the following is not a solution?(a) air free of smoke and dust(b) water free of other substances(c) sugar in water(d) HCl in waterG. When sodium chloride dissolves in water, the following species would be found in the resulting solution:(a) solvated NaCl molecules(b) solvated Na+(c) solvated Cl−(d) (b) and (c)H. Which one of the following observations is caused by a colligative property of solutions?(a) Water freezes at a lower temperature under pressure.(b) Water boils at a higher temperature under pressure.(c) Salt dissolves more rapidly in hot water than in cold.(d) Ice melts at a lower temperature when salt is added.I. A small amount of a certain solute melting at 800°C is added to water. The solution will be expected to freeze(a) above room temperature.(b) at 0°C.(c) slightly above 0°C.(d) slightly below 0°C.J. The pH of a solution refers to(a) the molarity of an acidic solution.(b) the molality of an acidic solution.(c) the concentration of hydronium ions in solution.(d) all of these. Get solution