1. Unit 8 – Solutions Review Game 12345678 910111213141516 1718192021222324 2526272829303132 3334353637383940 4142434445464748

2. Question 1 Describes two or more liquids that can dissolve into each other in various proportions. Answer: Miscible

3. Question 2 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

4. Question 3 How can the solubility of a gas be increased? Answer: Increase pressure, decrease temp, decrease agitation

5. Question 4 A compound that concentrates at the boundary surface between two immiscible phases (solid-liquid, liquid-liquid, or liquid- gas). Answer: Surfactant

6. Question 5 What does not experience the Tyndall effect? Answer: Solutions or homogeneous mixtures

7. Question 6 The law that relates partial pressure of a gas to its solubility is ____________________. Answer: Henry’s Law

8. Question 7 How do we change mg into grams? Answer: divide by 1000

9. Question 8 Carbon dioxide in water is an example of which solute-solvent combination? Answer: Gas-liquid

10. Question 9 This can be used to separate a solid from a liquid using heat. Answer: Evaporation

11. Question 10 Describes two or more liquids that do not mix with each other. Answer: Immiscible

12. Question 11 Silver and gold is an example of which solute-solvent combination? Answer: solid-solid

13. Question 12 What is symbolized by a capital M? Answer: Molarity

14. Question 13 This process can be used to separate two liquids that have different boiling points. Answer: Distillation

15. Question 14 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

16. Question 15 The ability of one substance to dissolve in another at a given temperature and pressure. Answer: Solubility

17. Question 16 Name two ways that concentration is expressed. Answer: Molarity, Molality, and parts per million

18. Question 17 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 )

19. Question 18 This can be used to separate liquids that have different densities. Answer: Centrifuge

20. Question 19 The amount of a particular substance in a given quantity of a mixture, solution, or ore. Answer: Concentration

21. Question 20 To determine the melting point elevation, the concentration of the solution should be in: Answer: Molality

22. Question 21 Which of the following has the least impact on solubility? a. Density b. Temperature c. Agitation d. Surface Area Answer: A

23. Question 22 The compound that will most likely dissolve in water a. is nonpolar b. is not a dipole. c. contains hydrogen sulfide. d. has a positive and negative region. Answer: D

24. Question 23 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

25. Question 24 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

26. Question 25 A homogeneous mixture of two or more substances uniformly dispensed throughout a single phase. Answer: Solution

27. Question 26 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

28. Question 27 How is molality calculated? Answer: moles divided by kilograms

29. Question 28 What does a small italicized m mean? Answer: molality

30. Question 29 In a solution, the substance that is dissolved. Answer: Solute

31. Question 30 The random movement of microscopic particles suspended in a fluid is known as: Answer: Brownian Motion

32. Question 31 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

33. Question 32 A water-soluble cleaner that can emulsify dirt and oil. Answer: Detergent

34. Question 33 Molecules that have both polar and nonpolar regions a. are unstable. b. could act as emulsifying agents. c. are likely to be flammable. d. will not dissolve in any solvent. Answer: b

35. Question 34 A special word that relates to separating a solid from a liquid by pouring. Answer: Decanting

36. Question 35 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

37. Question 36 In a solution, the substance that dissolves the other substance. Answer: Solvent

38. Question 37 607 g of NaCl is dissolved into 400 g of water. What is this concentration in the molality? Answer: 25.9 m

39. Question 38 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

40. Question 39 What is the formula used to calculate the change in freezing point. Answer:  T f = k f mN

41. Question 40 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

42. Question 41 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

43. Question 42 3.60 kg of water contains 1.52 moles of calcium hydroxide (Ca(OH) 2 ). What is the approximate molality of the solution? Answer: 0.422 m m = mol/kg = 1.52/3.60

44. Question 43 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

45. Question 44 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

46. Question 45 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

47. Question 46 Which of the pictures on the right is a homogenous mixture? Answer: A

48. Question 47 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

49. Question 48 At 10 °C, how much CsCl can be dissolved in 300 g of water? Answer: about 513 g 171 x 3