Chapter 9 Guided Notes - Pleasanton Unified ?· Web viewChapter 16 Guided Notes Name: _____ 16.1 –…

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Chapter 9 Guided NotesChapter 16 Guided NotesName: ______________________16.1 Properties of Solutions1. What phases can solutions exist in? _____________, _____________ and _____________2. The _____________________ of the solvent and the solute determine whether a substance will dissolve. Explain this statement.3. What three factors that involve the contact of the solute with the solvent can increase how fast a solute dissolves? Explain each.a)b)c)4. Evaluate Figure 16.2. Explain the equilibrium it shows.5. How is solubility often expressed?6. Define the following terms:a. saturated solution b. unsaturated solution c. supersaturated solution d. solubility e. miscible f. immiscible 7. Give an example of two liquids that are immiscible.8. Give an example of a solid and a liquid that are insoluble.9. Carefully study Figure 16.4. Use it to answer the following.a. Does temperature ALWAYS increase solubility? __________b. Which substance has the highest solubility at 50 C? _________c. Which substance has the most consistent solubility across the range of temps? ____10. Describe how temperature affects the solubility of gas solutes in liquid solvents. (p475)11. True or FalseIncreasing temperature usually increases solubility of solid solutes in liquid solvents.12. True or FalseIncreasing temperature usually increases solubility of gas solutes in liquid solvents.13. True or FalseIncreasing pressure usually increases solubility of gas solutes in liquid solvents.14. True or FalseMore solute can easily be added to a supersaturated solution.15. True or FalseStirring, temperature change and particle size all affect solution formation.16. True or FalseA solution is comprised a solute that has dissolved into a solvent.16.2 Concentrations of Solutions1. Define concentration.2. Contrast the terms dilute and concentrated.3. Write the equation for calculating Molarity (M).4. Read sample problem 16.2, then do the practice problems below! Show work!8)9)5. Read sample problem 16.3, then do the practice problems below! Show work!10)11)6. Evaluate Figure 16.9. Draw a diagram showing a more concentrated solution and a dilute solution.more concentratedless concentrated7. What happens to the moles of solute when making a dilution?8. Copy the equation for calculating dilutions (highlighted in yellow on page 483).9. Read sample problem 16.4, then do the practice problems below! Show work!12)13)10. What is the equation for finding concentration using percent by volume?11. Read sample problem 16.5, then do the practice problems below! Show work!14)15)12. What is the equation for finding concentration using percent by mass?13. Do problem #23 in the section assessment.14. What are the three ways your book described in this section for expressing concentration?15. Your teacher will describe two other ways to calculate concentration called grams/liter and parts per million. =)16.3 Colligative Properties16. What are colligative properties?17. List three important colligative properties.18. Evaluate Figure 16.14. Which of the three solutions has the largest impact on colligative properties? ___________________ Explain.19. Consider freezing point depression. Describe how the freezing point of a solution compares to that of the pure solvent.20. Relate freezing point depression to the use of salt on roadways in areas with freezing cold winters.21. Consider boiling point elevation. Describe how the boiling point of a solution compares to that of the pure solvent.22. True or FalseA solution will freeze at a lower temperature than the pure solvent.23. True or FalseA solution is in the liquid phase for a wider range of temperatures than the pure solvent.24. True or FalseA 2 M KBr solution has more solute particles than a 1M KBr solution of the same volume.25. True or FalseThere is only one correct way to express concentration.26. True or False200 grams of pure water has a volume of 200 mL.27. True or False75 mL is equal to 0.075 L.28. True or False The equation for molarity is moles of solute L of solvent

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