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Chemistry Solutions and Mixtures

Learn about solute-solvent combinations, separation techniques, colligative properties, vocabulary, formulas, concentration problems, and solubility concepts in chemistry.

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Chemistry Solutions and Mixtures

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  1. Solutions Round Gases Round

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

  3. Random Points 400 points

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

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

  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 Back

  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 Back

  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 Back

  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 Back

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

  11. Colligative Properties - 400 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

  12. Daily Double

  13. Colligative Properties - 500 • 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

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

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

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

  17. Daily Double

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

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

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

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

  22. Formulas - 300 • 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

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

  24. Formulas - 500 • What is the formula used to calculate the change in freezing point. Answer: Tf = kfmN Back

  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 Back

  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 Back

  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 M1V1=M2V2) Back

  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 Back

  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 Back

  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 Back

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

  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 Back Answer: NaC2H3O2 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 Back

  36. Solubilty - 500 • 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

  37. Gases Round

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

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

  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 Back

  42. Daily Double

  43. Ideal Gases - 1000 2H2O(l) + electricity  2H2(g) + O2(g) What mass of H2O is needed to create 15.64 L of O2, if the temperature is 25°C and the pressure is 1.2 atm? 27.6 g Back

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

  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 Back

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

  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 Back

  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 Back

  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 Back

  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 Back

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