Chapter 5 and 6

1. What is often the source of the ammonium ion in waste water? fish by-products human and animal waste industrial plating compounds algae

2. In an alcoholic beverage with 10% alcohol content by volume, how can the alcohol be defined? as a solvent as a solute as a solution as a fluid

3.Blood plasma is considered what component of a solution? the solvent the protein the solute the lipid

4.How are molecules described when they contain both a positive and negative end? planar apolar non-polar polar

5.In general, when an aqueous solution is heated, what happens to the solubility of ionic compounds within it? Solubility decreases. Solubility increases. Kinetic energy is added by the solute. Kinetic energy is removed by the solute.

6.What affects the rate at which solutes dissolve? temperature of the solution surface area of the solute concentration of the solute all of the above

7.Why does powdered sugar dissolve in water more rapidly than a sugar cube? greater surface area of the powder more kinetic energy in the powdered sample greater concentration in the sugar cube greater density of the sugar cube

8.What is an electrolyte? a compound that dissolves in water a compound that dissociates into ions in water a compound that dissociates into molecules in water an ionic compound that doesn't dissolve in water

9.What is a weak electrolyte? a compound that completely forms ions in solution a compound that only partially forms molecules in solution a compound that completely forms molecules in solution a compound that only partially forms ions in solution

10. Which compounds could be electrolytes? SO3 NO2 CH4 MgCl2

11.Which of these are electrolytes? ICl CO2 NaCl CO

12. Which of the following are not electrolytes? NaI CaCl2 KBr NO2

13. What is a saturated solution? one that contains the maximum amount of solute that can be dissolved. one that contains the maximum amount of solvent that can be dissolved. one that contains the maximum amount of solution that can be dissolved. one that contains the maximum amount of a salt that can be dissolved.

14. What type of compound is NH4NO3? acidic basic insoluble soluble

15. Molarity is what? moles of solvent per liters of solution moles of solute per liters of solution moles of solute per liters of solute moles of solvent per liters of solvent

16. What is the molarity of a solution made from 54. 9 g of NaCl in 0 16. What is the molarity of a solution made from 54.9 g of NaCl in 0.75 L of water? 73.2 M 1.25 M 1.42 M 0.01 M

17. What is the molarity of a solution made from 0.25 mol of KBr and 0.80 L of water?

18. An acid is any compound that can release what?

19. What do all weak acids have in common? They are weak electrolytes. They are non-electrolytes. They are strongly acidic. They are strong electrolytes.

20. NaOH is classified as what kind of compound? weak base strong acid strong base weak acid

21. How is a base defined? as a compound that produces hydroxide ions as a compound that produces H+ ions as a compound with a pH below 7 as a compound with pH = 7

22. What is lithium hydroxide? LiOH, a strong base LiOH, a weak base Li(OH)2, a strong base Li(OH)2, a weak base

23. A solution with a pH = 3.5 is said to be what? acidic basic neutral can't tell from the information given

24. The pH of a solution with a [H+] = 1.0 x 10–8 is what? 12 can't be determined

25. What is a solution with a pH of 12? neutral acidic basic concentrated

26. Attractive forces that exist between particles are called what? intermolecular forces intramolecular forces heteromolecular forces intravenous-molecular forces

27. What is surface tension? a measure of how much energy is needed to decrease the surface volume of a liquid a measure of how much surface is needed to increase the energy within a liquid a measure of how much energy is needed to increase the surface area of a liquid a measure of how much surface is needed to decrease the energy within a liquid

28. What takes place within the electron cloud of an atom? Electrons acquire positive charge. Electrons acquire negative charge. Electrons are fixed in positions. Electrons are in constant motion.

29. How is an induced dipole created? by an electron positioning next to it by an electron inversion near it by dipoles placed on both sides of it by the presence of a dipole next to it

30. Polarizability is defined how? by how easily an atom changes shape and charge by how deformable an atomic nucleus is by how deformable an electron cloud is by how easily an electron changes shape and charge

31. How would the following—HCl, HF, and HBr—be ranked from least to most polarizable? HCl, HF, HBr HF, HCl, HBr HF, HBr, HCl HBr, HCl, HF

32. Rank HCl, HI, and HBr from least to most polarizable. HCl, HBr, HI HI, HBr, HCl HBr, HCl, HI HI, HCl, HBr

33. How would the following, Ne, Kr, Ar, He, be ordered from lowest to highest melting point? He, Ne, Ar, Kr Kr, He, Ar, Ne He, Ar, Ne, Kr Kr, Ar, Ne, He

34. To what is the positive region of a polar molecule attracted? a magnet the positive region of a neighboring molecule the negative region of a neighboring molecule to a non-polar molecule, thus inducing a dipole

35. Of the following choices, which can form hydrogen bonds? H2S HCl

36. When a solute is added to a solvent, why does the boiling point increase? Intermolecular attractions hold solute and solvent apart, requiring more energy to make the solution boil. Intermolecular attractions hold solute and solvent together, requiring less energy to make the solution boil. Intermolecular attractions hold solute and solvent together, requiring more energy to make the solution boil. Intermolecular attractions hold solute and solvent apart, requiring less energy to make the solution boil.

37. How does boiling an unknown sample of water allow you to determine if it is pure water or a salt solution? In a salt solution, the b.p. should be lower than 100°C. In a salt solution, the b.p. should be higher than 100°C. In pure water, the b.p. should be lower than 100°C. In pure water, the b.p. should be higher than 100°C.

38. As the molecular mass of the compound increases, the higher the melting point. True false

39. Which of the following aqueous solution will have the lowest freezing point? 1 M MgBr2 1 M KBr 2 M C6H12O6 2 M C12H22O11

40. When comparing the freezing point of pure water and a salt solution, the best explanation would be: When a salt is dissolved in a solvent, it blocks part of the liquid solvent from interacting with the molecules resulting in a decreased rate of binding into a solid. When a salt is dissolved in a solvent, it blocks part of the liquid solvent from interacting with the molecules resulting in a increased rate of binding into a solid. A salt solution would freeze much faster than pure water because there are more molecules to bind to. Pure water will not freeze because there are not enough molecules to bind.

41. In general, ionic compounds have High boiling points and low melting points. Low boiling points and high melting points. High boiling points and high melting points. Low boiling points and low melting points.

42. Which of the following is most likely to have a high boiling point? NaCl CO2 CH4 H2O

43. Place the following list of atoms in order of increasing polarizability:Ga, B, Al, In B, Al, Ga, In Al, Ga, B, In Ga, B, Al, In In, Al, B, Ga

44. What is the one factor upon which boiling point elevation depends? number of particles in solution size of particles in solution charges of particles in solution types of particles in solution

45. A solution with pH = 3 has what [H+] concentration? 1 x 10–3 1 x103 3 x 10–13 3 x 103

not enough information to tell 46. If equal molar amounts of two solutions, one with pH = 1, the other with pH = 14, were mixed carefully and no solution was lost, what would be the pH of the final solution? 15 13 7 not enough information to tell

47. What is the pH of a completely neutral solution? 14 1 7

48. The products that would be expected in the neutralization reaction involving nitric acid and barium hydroxide are: BaO and H2O BaO2 and 2H2O BaNO3 and H2O Ba(NO3)2 and 2H2O