Chemistry. Approximate Timeline. Students are expected to keep up with class work when absent.

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1 Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 15 SOLUTIONS Day Plans for the day Assignment(s) for the day 1 Begin Chapter Forming Solutions o Solubility Assignment 15.0 Assignment 15.1 Read section(s)15.2 o Solution Composition: An Introduction o Factors Affecting the Rate of Dissolving Describing Solution Composition Assignment 15.2a o Solution Composition: Mass Percent Describing Solution Composition Assignment 15.2b o Solution Composition: Molarity Describing Solution Composition o Solution Composition: Dilution Assignment 15.2c Read section(s) Properties of Solutions o Stoichiometry of Solution Reactions Properties of Solutions o Stoichiometry of Solution Reactions Properties of Solutions Assignment 15.3 o Neutralization Reactions 8 Work on Assignment 15.4 Assignment Grade & discuss Assignment 15.4 Review for Chapter 15 Test 10 Chapter 15 Test Read section(s) 16.1

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3 Chemistry Name Hour Study Guides Chapter 15 Quizzes Quiz 15.1 Forming Solutions 1. Define the following terms. a. Concentrated b. Dilute c. Saturated d. Solute e. Solution f. Solvent g. Supersaturated h. Unstaurated 2. What happens to an ionic substance dissolves in water? 3. What is meant by the expression like dissolves like? 4. List three factors affecting the rate of dissolving. 5. Write a chemical equation to show what happens when an ionic compound dissolves in water. 6. Write a chemical equation to show what happens when a covalent compound dissolves in water. Quiz 15.2 Describing Solution Composition 7. Write the equation used to calculate solution concentration in terms of mass percent. 8. Write the equation used to calculate solution concentration in terms of molarity. 9. Define the term dilution. 10. Write the equation used when solving a dilution problem. 11. Be able to calculate the mass percent of a solute in solution. 12. Be able to calculate the molarity of a solute in solution. 13. Be able to solve a dilution problem. Quiz 15.3 Solution Stoichiometry 14. Be able to solve solution stoichiometry problems.

4 Study Guide Chapter 15 Test At the completion of chapter 15 you should 1. Know the definitions of the following terms. a. Solution b. Solvent c. Solute d. Saturated e. Unsaturated f. Supersaturated g. Concentrated h. Dilute i. Mass Percent j. Molarity k. Neutralization Reaction l. Colligative Property 2. Be able to describe, on the molecular level, what happens when a substance dissolves in water. 3. Know and explain the factors affecting the rate of dissolving. a. Surface area b. Stirring c. Temperature 4. Be able to calculate the concentration of a solution in terms of mass percent and molarity. 5. Use mass percent and molarity to calculate the amount of substance needed to make a solution. 6. Be able to solve dilution problems. 7. Be able to solve solution stoichiometry problems. 8. Know how a solute affects the boiling point and freezing point of a solution.

5 Chemistry Name Hour Assignment 15.0 Vocabulary (2 pages) Define each of the following terms. 1. Solution 2. Solvent 3. Solute 4. Saturated 5. Unsaturated 6. Supersaturated 7. Concentrated 8. Dilute 9. Mass Percent 10. Molarity

6 11. Neutralization Reaction 12. Colligative Property

7 Chemistry Name Hour Assignment 15.1 Forming Solutions 1) Determine the number of moles of each type of ion in solution when 1 mole of each of the following dissolves in water: (show your work) A) sodium sulfate B) ammonium acetate C) calcium chloride D) copper (II) sulfate 2) Chemists often say like dissolves like. What does this mean? 3) Why does water by itself not dissolve a grease stain? 4) Can a dilute solution also be saturated?

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9 Chemistry Name Hour Assignment 15.2a Mass Percent 1) Calculate the mass percent of calcium chloride in each of the following solutions. Show your work. A) 5.00 g of calcium chloride in 75.0 g of water B) 1.00 g of calcium chloride in 39.0 g of water C) 2.00 g of calcium chloride in 63.0 g of water 2) Calculate the mass, in grams, of sodium chloride present in each of the following solutions. Show your work. A) 11.5 g of 6.25% solution B) 6.25 g of 11.5% solution C) 452 g of 12.3% solution

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11 Chemistry Name Hour Assignment 15.2b - Molarity 1) Calculate the molarity of each of the following solutions. Show your work. A) 4.25 g CuCl 2 in enough water to make 125 ml of solution B) 25.9 g Na 2 CO 3 in enough water to make ml of solution C) 10.1 g NaNO 3 in enough water to make ml of solution 2) Calculate the mass, in grams, of solute present in each of the following solutions. Show your work. A) ml of 1.50 M NaOH B) 225 ml of M KNO 3 C) 2.00 L of M Na 2 SO 3

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13 Chemistry Name Hour Assignment 15.2c Describing Solution Composition Show your work. 1) Vinegar is made by adding 33 g of acetic acid to 625 g of water. What is the percent by mass of acetic acid in this solution of vinegar? 2) A solution is labeled M magnesium nitrate. Calculate the concentration of each ion present in solution. 3) Calculate the number of moles of KOH in ml of M KOH solution. 4) If 4.25 g of CaBr 2 is dissolved in enough water to make 125 ml of solution, what is the molarity of the solution? 5) Calculate the new concentration when 50.0 ml of water is added to 725 ml of 1.25 M NaCl.

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15 Chemistry Name Hour Assignment 15.3 Properties of Solutions (2 pages) 1) The key to solving stoichiometry problems is the mole. How do we find the number of moles when solutions are mixed to produce a reaction? 2) How many milliliters of 0.10 M Pb(NO 3 ) 2 solution are required to precipitate all of the lead, as PbI 2, from ml of 0.10 M NaI solution? Pb(NO 3 ) 2 (aq) + 2 NaI (aq) PbI 2 (s) + 2 NaNO 3 (aq) 3) Determine the mass of Ag 2 CrO 4 produced when ml of M silver(i) nitrate is added to ml of M potassium chromate. 2 AgNO 3 (aq) + K 2 CrO 4 (aq) Ag 2 CrO 4 (s) + 2 KNO 3 (aq)

16 4) What volume of 0.25 M NaOH is required to neutralize ml of 0.15 M HCl? NaOH (aq) + HCl (aq) H 2 O (l) + NaCl (aq) 5) Other than for taste, why is salt added to water when cooking pasta?

17 Chemistry Name Hour Assignment 15.4 Chapter Review (4 pages) 1) A solution that contains as much solute as will dissolve at a given temperature is said to be. 2) A solution that has not reached its limit of dissolved solute is said to be. 3) The label concentrated H 2 SO 4 on a bottle means that there is a relatively amount of H 2 SO 4 present in the solution. 4) A lab assistant prepared a potassium chloride solution for her class by dissolving 5.34 g KCl in 152 g of water. What is the mass percent of KCl in the solution she prepared? 5) What mass of each solute is present in 285 g of a solution that contains 5.00% by mass NaCl and 7.50% by mass Na 2 CO 3? 6) A solution that is labeled M NaOH would contain mol of NaOH per liter of solution. 7) If you were to prepare exactly 1.00 L of a 5 M NaCl solution, you would not need exactly 1.00 L of water. Explain.

18 8) If a 45.3 g sample of potassium nitrate is dissolved in enough water to make 225 ml of solution, what will be the molarity of the solution? 9) If 495 g of NaOH is dissolved to a final total volume of 20.0 L, what is the molarity of the solution? 10) Standard silver (I) nitrate solutions are used in the analysis of samples containing chloride ion. How many grams of silver (I) nitrate are needed to prepare 250. ml of a M AgNO 3 solution?

19 Chemistry Name Hour 11) Many laboratories keep bottles of 3.0 M solutions of the common acids on hand. Given the following molarities of the concentrated acids, determine how many milliliters of each concentrated acid would be required to prepare 225 ml of a 3.0 M solution of the acid. Acid HCl 12.1 HNO H 2 SO HC 2 H 3 O H 3 PO Molarity of Concentrated Reagent

20 12) How much water must be added to 500. ml of M HCl to produce a M solution? (Assume that the volumes are additive.) 13) One way to determine the amount of chloride ion in a water sample is to react the sample with standard AgNO 3 solution to produce solid AgCl. If a 25.0 ml water sample requires 27.2 ml of M AgNO 3 in such a reaction, what is the concentration of Cl - in the sample? Ag + (aq) + Cl - (aq) AgCl (s) 14) If 36.2 ml of M CaCl 2 solution is added to 37.5 ml of M Na 2 CO 3, what mass of calcium carbonate, CaCO 3, will be precipitated? CaCl 2 (aq) + Na 2 CO 3 (aq) CaCO 3 (s) + 2 NaCl (aq)