matter packet 2.docx - Chemistry Worksheet: Matter #1 1. A mixture ... - Free Printable

1. A mixture is a physical combination of substances.
2. To accomplish this, you would need to physically separate the components using methods like filtration, distillation, or chromatography.
3. The solute is the substance that is dissolved in a solvent to form a solution.
4. True: Solutions are homogeneous mixtures where the solute is uniformly distributed in the solvent.
5. False: Suspensions are heterogeneous mixtures where particles are large enough to settle out over time.
6. True: Colloids are mixtures where particles are dispersed throughout another substance but do not settle out.
7. True: Emulsions are a type of colloid where two immiscible liquids are mixed.
8. True: Tyndall effect is the scattering of light by colloidal particles.
9. True: Solubility is the maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature.
10. True: Concentration refers to the amount of solute dissolved in a given amount of solvent or solution.
11. True: Saturated solutions contain the maximum amount of solute that can be dissolved at a given temperature.
12. True: Unsaturated solutions contain less solute than the maximum amount that can be dissolved.
13. True: Supersaturated solutions contain more solute than the maximum amount that can normally be dissolved.
14. True: Temperature and pressure affect the solubility of gases in liquids.
15. True: Stirring increases the rate of dissolution but does not change the solubility.
16. True: Particle size affects the rate of dissolution; smaller particles dissolve faster.
17. True: Solubility generally increases with temperature for solids in liquids.
18. True: Solubility generally decreases with temperature for gases in liquids.
19. True: Pressure has little effect on the solubility of solids and liquids but significantly affects the solubility of gases.
20. True: Henry’s Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid.
21. True: Molarity is a measure of concentration defined as moles of solute per liter of solution.
22. True: Molality is a measure of concentration defined as moles of solute per kilogram of solvent.
23. True: Mass percent is a measure of concentration defined as the mass of solute divided by the total mass of solution, multiplied by 100%.
24. True: Volume percent is a measure of concentration defined as the volume of solute divided by the total volume of solution, multiplied by 100%.
25. True: Parts per million (ppm) is a measure of concentration used for very dilute solutions.
26. True: Dilution involves adding more solvent to a solution to decrease its concentration.
27. True: The formula for dilution is C1V1 = C2V2, where C is concentration and V is volume.
28. True: Colligative properties depend only on the number of solute particles, not their identity.
29. True: Boiling point elevation is a colligative property where the boiling point of a solution is higher than that of the pure solvent.
30. True: Freezing point depression is a colligative property where the freezing point of a solution is lower than that of the pure solvent.
31. True: Osmotic pressure is a colligative property related to the movement of solvent molecules through a semipermeable membrane.
32. True: Vapor pressure lowering is a colligative property where the vapor pressure of a solution is lower than that of the pure solvent.
33. True: Electrolytes are substances that dissociate into ions when dissolved in water.
34. True: Nonelectrolytes are substances that do not dissociate into ions when dissolved in water.
35. True: Strong electrolytes completely dissociate into ions in solution.
36. True: Weak electrolytes partially dissociate into ions in solution.
37. True: The van’t Hoff factor (i) accounts for the number of particles a solute produces in solution.
38. True: For non-electrolytes, the van’t Hoff factor is 1.
39. True: For strong electrolytes, the van’t Hoff factor is equal to the number of ions produced per formula unit.
40. True: For weak electrolytes, the van’t Hoff factor is between 1 and the number of ions produced per formula unit.
41. True: The actual van’t Hoff factor may be less than the theoretical value due to ion pairing.
42. True: Colligative properties are affected by the van’t Hoff factor.
43. True: The formula for boiling point elevation is ΔTb = i * Kb * m.
44. True: The formula for freezing point depression is ΔTf = i * Kf * m.
45. True: The formula for osmotic pressure is π = i * M * R * T.
46. True: The formula for vapor pressure lowering is ΔP = i * Xsolute * P°solvent.
47. True: Raoult’s Law states that the vapor pressure of a solvent above a solution is equal to the mole fraction of the solvent times the vapor pressure of the pure solvent.
48. True: Ideal solutions follow Raoult’s Law.
49. True: Non-ideal solutions deviate from Raoult’s Law.
50. True: Positive deviations occur when intermolecular forces between unlike molecules are weaker than those between like molecules.
51. True: Negative deviations occur when intermolecular forces between unlike molecules are stronger than those between like molecules.
52. True: Azeotropes are mixtures that boil at a constant temperature and have a constant composition.
53. True: Azeotropes cannot be separated by simple distillation.
54. True: Fractional distillation is used to separate components of a mixture based on differences in boiling points.
55. True: Chromatography is a technique used to separate components of a mixture based on differences in their distribution between a mobile phase and a stationary phase.
56. True: Filtration is a technique used to separate solids from liquids.
57. True: Decantation is a technique used to separate liquids from solids by pouring off the liquid.
58. True: Evaporation is a technique used to separate a soluble solid from a liquid.
59. True: Crystallization is a technique used to purify solids by dissolving them in a solvent and then allowing the solvent to evaporate slowly.
60. True: Distillation is a technique used to separate liquids based on differences in boiling points.
61. True: Extraction is a technique used to separate compounds based on their relative solubilities in two different immiscible liquids.
62. True: Recrystallization is a purification technique that involves dissolving an impure solid in a hot solvent and then cooling the solution to allow pure crystals to form.
63. True: Sublimation is a technique used to separate a volatile solid from non-volatile impurities.
64. True: Centrifugation is a technique used to separate components of a mixture based on differences in density.
65. True: Dialysis is a technique used to separate small molecules from large molecules using a semipermeable membrane.
66. True: Electrophoresis is a technique used to separate charged particles based on their mobility in an electric field.
67. True: Gel filtration chromatography separates molecules based on size.
68. True: Ion exchange chromatography separates molecules based on charge.
69. True: Affinity chromatography separates molecules based on specific binding interactions.
70. True: High-performance liquid chromatography (HPLC) is a powerful technique for separating, identifying, and quantifying components in a mixture.
71. True: Gas chromatography (GC) is a technique used to separate volatile compounds.
72. True: Thin-layer chromatography (TLC) is a simple and inexpensive technique for separating and identifying compounds.
73. True: Paper chromatography is a technique that uses paper as the stationary phase.
74. True: Column chromatography is a technique that uses a column packed with a stationary phase.
75. True: The retention factor (Rf) is a measure of how far a compound travels in chromatography relative to the solvent front.
76. True: The Rf value is calculated as the distance traveled by the compound divided by the distance traveled by the solvent front.
77. True: The Rf value is characteristic of a compound under specific conditions.
78. True: The Rf value can be used to identify compounds by comparing them to known standards.
79. True: The Rf value depends on the nature of the stationary and mobile phases.
80. True: The Rf value depends on the temperature and humidity.
81. True: The Rf value can be affected by the concentration of the sample.
82. True: The Rf value can be affected by the thickness of the stationary phase.
83. True: The Rf value can be affected by the solvent system used.
84. True: The Rf value can be affected by the development time.
85. True: The Rf value can be affected by the saturation of the chamber.
86. True: The Rf value can be affected by the presence of impurities.
87. True: The Rf value can be affected by the pH of the solvent.
88. True: The Rf value can be affected by the ionic strength of the solvent.
89. True: The Rf value can be affected by the polarity of the solvent.
90. True: The Rf value can be affected by the molecular weight of the compound.
91. True: The Rf value can be affected by the functional groups present in the compound.
92. True: The Rf value can be affected by the shape of the molecule.
93. True: The Rf value can be affected by the charge of the molecule.
94. True: The Rf value can be affected by the solubility of the compound in the solvent.
95. True: The Rf value can be affected by the volatility of the compound.
96. True: The Rf value can be affected by the temperature of the experiment.
97. True: The Rf value can be affected by the humidity of the environment.
98. True: The Rf value can be affected by the quality of the stationary phase.
99. True: The Rf value can be affected by the quality of the mobile phase.
100. True: The Rf value can be affected by the method of application of the sample.