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Unit 8 – Solutions Review Game

Unit 8 – Solutions Review Game. Question 1. Describes two or more liquids that can dissolve into each other in various proportions. Answer: Miscible. Back. Question 2.

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Unit 8 – Solutions Review Game

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  1. Unit 8 – Solutions Review Game

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

  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 Back

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

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

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

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

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

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

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

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

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

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

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

  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 Back

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

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

  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 M1V1=M2V2) Back

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

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

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

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

  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 Back

  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 Back

  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 Back

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

  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 Back

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

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

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

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

  32. Question 31 Which of the following would have the greatest impact on the freezing point of water? a. glucose (C6H12O6) b. strontium sulfide (SrS) c. lithium bromide (LiBr2) d. sodium chloride (NaCl) Answer: C Back

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

  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 Back

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

  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 Back

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

  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 Back

  39. Question 38 • What is the formula to calculate the parts per million of a solution? Answer: m = gsolute /gsolvent x 1000000 Or m = masssolute /masssolvent x 1000000 Back

  40. Question 39 • What is the formula used to calculate the change in freezing point. Answer: Tf = kfmN Back

  41. Question 40 • What chemical has the most change in solubility as the temperature is changed from 0C to 100  C Back Answer: NaC2H3O2 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 Back

  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 Back

  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 Back

  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 Back

  46. Question 45 • At 90C, 30 g of Li2SO4 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 Li2SO4 Back

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

  48. Question 47 • Calculate the boiling point of a solution of 520 g of the ionic compound magnesium chloride, MgCl2, dissolved in 900 g of water. (kb of water is 0.51ºC/m and the normal boiling point of water is 100ºC) Answer: 520g x 1mol/95.3g = 5.45 mol Tb = KbmN = (0.51)(5.45/.900)(3) = 9.265ºC 100 + (9.265) = 109.3ºC Back

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

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