1. Solutions Round MixturesCollig. Props Vocab.FormulasConc. Problems Solubility 100 200 300 400 500 Gases Round

2. Mixtures - 100 Silver and gold is an example of which solute- solvent combination? Answer: solid-solid

3. Random Points 400 points

4. Mixtures - 200 This can be used to separate liquids that have different densities. Answer: Centrifuge

5. Mixtures - 300 What does not experience the Tyndall effect? Answer: Solutions or homogeneous mixtures

6. Mixtures - 400 Identify whether the following scenario describes a saturated, unsaturated or supersaturated solution. A single grain of solute is added to the solution, it sinks to the bottom of the container, and nothing else happens. Answer: Saturated

7. Mixtures - 500 A student is trying to determine if a liquid is a colloid, solution or suspension. The student cannot see through the mixture and the particles are not settling out. The liquid should be classified as a _______________________. Answer: Colloid

8. Colligative Properties - 100 A property that is determined by the number of particles present in a system but that is independent of the properties of the particles themselves. Answer: Colligative Property

9. Colligative Properties - 200 Which of the following is an example of using the concept of boiling point elevation? a. Adding table salt in water to cook pasta b. Adding rock salt on icy roads c. Adding valve oil to a brass instrument during a Christmas parade to keep the valves from locking up. d. Adding ethylene glycol (antifreeze) to a car engine during the winter. Answer: a

10. Colligative Property - 300 To determine the melting point elevation, the concentration of the solution should be in: Answer: Molality

11. Colligative Properties - 400 Which of the following would have the greatest impact on the freezing point of water? a. glucose (C 6 H 12 O 6 ) b. strontium sulfide (SrS) c. lithium bromide (LiBr 2 ) d. sodium chloride (NaCl) Answer: C

12. Daily Double

13. Colligative Properties - 500 Calculate the boiling point of a solution of 520 g of the ionic compound magnesium chloride, MgCl 2, dissolved in 900 g of water. (k b of water is 0.51ºC/m and the normal boiling point of water is 100ºC) Answer: 520g x 1mol/95.3g = 5.45 mol  T b = K b mN = (0.51)(5.45/.900)(3) = 9.265ºC 100 + (9.265) = 109.3ºC

14. Vocabulary - 100 In a solution, the substance that is dissolved. Answer: Solute

15. Vocabulary - 200 A water-soluble cleaner that can emulsify dirt and oil. Answer: Detergent

16. Vocabulary - 300 A compound that concentrates at the boundary surface between two immiscible phases (solid-liquid, liquid-liquid, or liquid- gas). Answer: Surfactant

17. Daily Double

18. Vocabulary - 400 The law that relates partial pressure of a gas to its solubility is ____________________. Answer: Henry’s Law

19. Vocabulary - 500 The random movement of microscopic particles suspended in a fluid is known as: Answer: Brownian Motion

20. Formulas - 100 What is symbolized by a capital M? Answer: Molarity

21. Formulas - 200 What does a small italicized m mean? Answer: molality

22. Formulas - 300 What is the formula to calculate the parts per million of a solution? Answer: m = g solute /g solvent x 1000000 Or m = mass solute /mass solvent x 1000000

23. Formulas - 400 How is molality calculated? Answer: moles divided by kilograms

24. Formulas - 500 What is the formula used to calculate the change in freezing point. Answer:  T f = k f mN

25. Concentration Problems - 100 A sample of 1500.0 g of drinking water is found to contain 42 mg Pb. What is this concentration in parts per million? Answer: 28 ppm

26. Random Points 300 points

27. Concentration Problems - 200 A solution contains 76.0 g of NaCl and has a volume of 550 mL. Find the molarity of the solution. Answer: 2.36 M

28. Concentration Problems - 300 You need to make 200 mL of 0.25 M HCl. How much 6.0 M HCl would you need? Answer: 8.33 mL (use M 1 V 1 =M 2 V 2 )

29. Concentration Problems - 400 How many grams of NaOH are required to prepare 1200 mL of a 0.50 M solution? Answer: 24 g 0.50 = x/1.200 (M=mol/L) x = 0.6 mol x 40g/1mol = 24 g

30. Concentration Problems - 500 Legally, the concentration of methyl mercury needs to be less than 1.0 ppm in fish meat to be sold or eaten. What is the maximum amount in milligrams of methyl mercury allowed in a fish that weighs 2.25 kg? Answer: 2.25 mg 1.0 = x/2250 x 1000000 x = 0.00225 g x 1000 = 2.25 mg

31. Solubility - 100 Describe a condition that has an effect on solubility. Answer: Temperature – increases solubility of solids and liquids, decreases solubility of gases, Agitation – increases solubility of liquids and solids Surface area – the smaller the surface area, the greater impact on solubility Polarity – has to be the same polarity to be soluble

32. Solubility - 200 How can the solubility of a gas be increased? Answer: Increase pressure, decrease temp, decrease agitation

33. Random Points 200 points

34. Solubility - 300 What chemical has the most change in solubility as the temperature is changed from 0  C to 100  C Answer: NaC 2 H 3 O 2 or sodium acetate

35. Solubility - 400 At 10 °C, how much CsCl can be dissolved in 300 g of water? Answer: about 513 g 171 x 3

36. Solubilty - 500 At 90  C, 30 g of Li 2 SO 4 is dissolved in 100 g of water. Is this solution saturated, unsaturated, or supersaturated? Answer: Unsaturated, because at 90  C, water can hold 31 g of Li 2 SO 4

37. Gases Round Ideal Gases Gas LawsGas Law Problems Diffusion Concepts Misc.Vocab 200 400 600 800 1000

38. Ideal Gases - 200 What is the ideal gas law formula? PV=nRT

39. Ideal Gases - 400 According to the diagram to the right, at what pressure do all the gases most resemble an ideal gas? 0 atm

40. Ideal Gases - 600 Calculate the approximate volume of a 2.50 mol sample of gas at -8.0°C and a pressure of 3.50 atm. 15.5 L

41. Ideal Gases - 800 A 10.5 L sample of a gas has a mass of 95.9 g at 7.6 atm and 35°C. What is the molar mass of the gas? (Hint: divide the given mass by n). 30.4 g/mol

42. Daily Double

43. Ideal Gases - 1000 2H 2 O(l) + electricity  2H 2 (g) + O 2 (g) What mass of H 2 O is needed to create 15.64 L of O 2, if the temperature is 25°C and the pressure is 1.2 atm? 27.6 g

44. Gas Laws - 200 What happens to the volume of a gas during compression? The Volume Decreases

45. Gas Laws - 400 Who developed the concept that the total pressure of a mixture of gases is the sum of their partial pressures? Dalton

46. Gas Laws - 600 Charles’s law is the direct relationship between ____________________ and volume. Temperature

47. Gas Laws - 800 Who is accredited with the idea that in a reaction, two volumes of hydrogen gas will combine with one volume of oxygen gas to produce two volumes of water vapor? Gay-Lussac

48. Gas Laws - 1000 The principle that under similar pressures and temperatures, equal volumes of gases contain the same number of molecules is attributed to ________________. Avogadro

49. Gas Law Problems - 200 A mixture of gases with a pressure of 800.0 mm Hg contains 60% nitrogen and 40% oxygen by volume. What is the partial pressure of oxygen in this mixture? 320 mm Hg

50. Gas Law Problems - 400 A sample of oxygen occupies 350 mL when the pressure is 5 atm. At constant temperature, what volume does the gas occupy when pressure falls to 3 atm? 583 mL

51. Gas Law Problems - 600 T 1 = 76  C P 1 = 4 atmV 1 = 560 mL T 2 = 92  C P 2 = 2 atmV 2 = ? 1171 mL

52. Daily Double

53. Gas Law Problems - 800 Nitrogen reacts with hydrogen to make ammonia [N 2 (g) + 3H 2 (g) --> 2NH 3 (g)]. If one needs to produce 4 L of ammonia, how many liters of nitrogen are needed? 2 L

54. Gas Law Problems - 1000 A sample of a gas has a pressure of 2.25 atm, a volume of 650 mL and a temperature of 36°C. What would the volume of the gas be if the pressure is increased to 3.20 atm and the temperature is decreased to 31°C? 449.6 mL

55. Random Points 500 points

56. Diffusion Concepts - 200 This is the passage of a gas under pressure through a tiny opening. Effusion

57. Diffusion Concepts - 400 The rate of diffusion of a gas depends on the ____________ of the gas. Molar Mass

58. Diffusion Concepts - 600 What scientist studied effusion in detail and determined that the rate of effusion is indirectly proportional to the square root of the molar mass of the gas, if pressure and temperature are kept constant. (Thomas) Graham

59. Diffusion Concepts - 800 To two decimal places, what will v A /v B be equal to if N 2 is considered to be gas A and NO is considered to be gas B. (A diffusion problem) 1.03

60. Diffusion Concepts - 1000 What is the molar mass of a gas if it diffuses at a rate of 258 m/s while Iodine gas diffuses at 125 m/s at the same temperature? 29.7 g

61. Miscellaneous - 200 The average kinetic energy of random motion is proportional to the temperature in what unit? Kelvin

62. Miscellaneous - 400 Standard temperature and pressure for a gas is ____________________ 0°C (or 273 K) and 1 atm.

63. Random Points 300 points

64. Miscellaneous - 600 What is the SI unit of pressure? Pascal

65. Miscellaneous - 800 A pressure of 165 kPa is equal to _____ atm. (1 atm = 101325 Pa) 1.63

66. Miscellaneous - 1000 Line D represents water. If the atmospheric pressure in a flask is lowered to 70 kPa, water would boil at what temperature? 92  C

67. Vocabulary - 200 What does the constant bombardment of gas molecules against the inside of a container cause? Pressure

68. Vocabulary - 400 The movement of particles from regions of higher concentrations to regions of lower concentration. Diffusion

69. Random Points 800 points

70. Vocabulary - 600 A device used to measure pressure is called a ____________________. Barometer

71. Vocabulary - 800 The pressure of each gas in a mixture is called the ____________________ pressure. Partial

72. Vocabulary - 1000 What is the theory that explains that the behavior of physical systems depends on the combined actions of the molecules constituting the system? Kinetic Molecular Theory