SC2 – O’Malley SAT II Review (Solutions)

For 1 – 2: a. Molarity b. Formality c. Density d. Molality e. Normality

1. Which is defined as moles of solute per kilogram of solvent?

2. Which is defined as moles of solute

per liter of solution?

For 3 – 6: a. Solute b. Solvent c. Solubility d. Aqueous solution e. Solvation

3. Which is present in a lesser amount in a solution?

4. Which describes a species in which

the solvent is water?

5. Which is present in greater quantity in solution?

6. Which is the interaction between

the solute and the solvent molecules?

For 7 – 9: a. Dilute b. Concentrated c. Unsaturated d. Saturated e. Supersaturated

7. Which is the condition, unrelated to quantities, that indicates that the rate going into solution is equal to the rate coming out of solution?

8. Which is the condition that exists

when a water solution that has been at equilibrium is heated to a higher temperature with a higher solubility, but no additional solute is added?

9. Which is the descriptive term that

indicates there is a large quantity of

solute, compared with the amount of solvent, in a solution?

For 10 – 11: a. i, ii and iii b. i and ii c. ii and iii d. i only e. iii only

10. The ionization of salts in water is useful in explaining

i. Their unusually large solubility in water

ii. Their electrical conductivity in solution

iii. The lowered freezing points and increased boiling points of their solutions

11. Which of the following describe

water? i. Solvent for polar solutes ii. Polar molecule iii. Good conductor of electricity

Q Statement I Because Statement II

12. When a solute is added to pure water, the vapor pressure of the water will decrease

Because All solutes dissociate into positive and negative ions

13. NaCl(aq) is an electrolyte Because It forms ions in solution

14. A salt dissolved in an organic solvent will be a good electrical conductor

Because Salts will not dissolve appreciably in an organic solvent

15. A super saturated solution of glucose in boiling water crystallizes as it cools

Because The solubility increases as the temperature decreases

16. Salt dissolved in water lowers the freezing point Because The change in freezing point is given by: Tf = iKfm

17. Sodium chloride forms aqueous solution of ions Because The sodium has a +1 charge and the chloride has a -1 charge and they are hydrated by the water molecules

18. What is the molarity if a 500 mL solution

contains 20 g of CaBr2? a. 0.1 M b. 0.2 M c. 0.5 M d. 1 M e. 5 M

19. How many moles of sulfate ions are in 200 mL of a 2 M sodium sulfate solution? a. 0.2 mol b. 0.4 mol c. 0.6 mol d. 0.8 mol e. 1.0 mol

20. A 0.5 m solution could be prepared by

dissolving 20 g NaOH in a. 0.5 L water b. 0.5 kg water c. 1 L water d. 1 kg water e. 2 L water

21. What volume of water would be needed to

dilute 50 mL of a 3 M HCl solution to 1 M? a. 25 mL b. 50 mL c. 75 mL d. 100 mL e. 150 mL

22. About how many grams of sodium chloride would be dissolved in water to form a 0.5 M solution in 500 mL solution? a. 7 b. 29 c. 14.5 d. 58 e. 112

23. A one liter solution of 2 M NaOH can be

prepared with a. 20 g NaOH b. 40 g NaOH c. 60 g NaOH d. 80 g NaOH e. 100 g NaOH

24. What is the molarity of a 10 mL solution in

which 3.7 g KCl are dissolved? a. 0.05 M b. 0.1 M c. 1 M d. 5 M e. 10 M

25. A solution of 10 M NaOH was used to

prepare 2 L of 0.5 M NaOH. How many mL of the original NaOH solution are needed? a. 10 mL b. 100 mL c. 1000 mL d. 200 mL e. 2000 mL

26. A 1 molal solution of NaCl results when

58.5 g of sodium chloride is dissolved in a. One liter of water b. 100 mL of water c. one kilogram of water d. 100 g of water e. one cubic meter of water

27. A small crystal of NaCl is added to a sodium chloride solution resulting in the precipitation of more than 1 gram of sodium chloride. This solution had been a. Unsaturated b. Saturated c. Supersaturated d. Dilute e. Concentrated

28. Sodium chloride would be most soluble in a. Ether b. Benzene c. Water d. Carbon tetrachloride e. Gasoline

29. Which of the following would produce a

highly conductive aqueous solution? a. Cyclohexane b. Hydrochloric acid c. Benzene d. Sucrose e. Acetic acid

30. A 10% solution of HNO3 would be produced by dissolving 63 g HNO3 in how many mL water? a. 100 b. 300 c. 567 d. 630 e. 1000

31. What is the boiling point of an aqueous

solution containing 117 g NaCl in 1000 g H2O? Kb = 0.52

oC kg/mol

a. 98.96 oC

b. 99.48 oC

c. 100.52 oC

d. 101. 04 oC

e. 102.08 oC

32. Which of the following sequences lists the

relative sizes of particles in a water mixture from smallest to largest? a. Solutions, suspensions, colloids b. Solutions, colloids, suspensions c. Colloids, solutions, suspensions d. Colloids, suspensions, solutions e. Suspensions, colloids, solutions

33. A compound which, when dissolved in

water, barely conducts electrical current can probably be a. A strong electrolyte b. An ionic salt c. A strong acid d. A strong base e. None of the above

34. How many grams of HCl must be added to

500 mL water to produce a solution that freezes at -1.86

oC? (molal freezing

constant = 1.86 oC kg/mol)

a. 4.6 b. 9.1 c. 18.3 d. 36.5 e. 73.0

35. A solution can be both

a. Dilute and concentrated b. Saturated and dilute c. Saturated and unsaturated d. Supersaturated and saturated e. None of these

36. The solubility of a solute indicates

a. The temperature of the solution b. The quantity of solvent c. The quantity of solute d. The nature of the solute & solvent e. All of these

37. A 10% solution of NaCl means that in 100

g of solution there is a. 5.85 g NaCl b. 58.5 g NaCl c. 10 g NaCl d. 94 g NaCl

38. The molarity of a solution made by placing

98 g H2SO4 in sufficient water to make 500 mL of solution is a. 0.5 b. 1 c. 2 d. 3

39. If 684 g sucrose (MM = 342 g) is dissolved

in 2000 g H2O (essentially 2 L), what will be the freezing point of this solution? a. -0.51

oC

b. -1.86 oC

c. -3.72 oC

d. -6.58 oC

40. Ten grams of sodium hydroxide dissolved

in 1 L of water makes a solution that is a. 0.25 M b. 0.5 M c. 1 M d. 1.5 M e. 4 M

41. How much water, in liters, must be added

to 0.5 L of 6 M HCl to make it 2 M? a. 0.33 b. 0.5 c. 1 d. 1.5 e. 2

42. How many grams of NaOH are needed to

make 100 g of a 5 % solution? a. 2 b. 5 c. 20 d. 40 e. 95

43. What is the boiling point of water at the top

of a mountain? a. 100

oC

b. > 100 oC since the pressure is less

than at ground level c. < 100

oC since the pressure is less

than at ground level d. > 100

oC since the pressure is greater

than at ground level e. < 100

oC since the pressure is greater

than at ground level

44. 1 mol NaCl in 1000 g H2O will change the boiling point of water to a. 100.51

oC

b. 101.04 oC

c. 101.53 oC

d. 101.86 oC

e. 103.62 oC

45. To what volume, in mL, must 50.0 mL of

3.50 M H2SO4 be diluted in order to make 2 M H2SO4? a. 25 b. 60.1 c. 87.5 d. 93.2 e. 101

46. What is the molar mass of a non-ionizing

solid if 10 g of this solid, dissolved in 100 g of water, formed a solution that froze at -1.21

oC?

a. 0.65 g b. 6.5 g c. 130 g d. 154 g e. 265 g

47. What is the melting point of 0.2 L water containing 6.20 g C2H6O2? a. -1.86

oC

b. -0.93 oC

c. 0 oC

d. 0.93 oC

e. 1.86 oC

48. Which of the following are TRUE?

i. Adding a solute raises the vapor pressure & boiling point

ii. The change in boiling & freezing point depends on molality.

iii. The number of solute particles in a solvent is an important factor in determining the boiling point elevation

a. i only b. ii only c. i and ii d. ii and iii e. i, ii and iii

Answers:

1. D 2. A 3. A 4. D 5. B 6. E 7. D 8. C 9. B 10. A 11. B 12. T F 13. T T CE 14. F T 15. T F 16. T T CE 17. T T CE 18. B 19. B 20. D 21. D 22. C 23. D 24. D 25. B 26. C 27. C 28. C 29. B 30. C 31. E 32. B 33. E 34. B 35. B 36. E 37. C 38. C 39. B 40. A 41. C 42. B 43. C 44. B 45. C 46. D 47. B 48. D