CHAPTER 4 TYPES OF CHEMICAL REACTIONS & SOLUTION STOICHIOMETRY

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1 Advanced Chemistry Name Hour Advanced Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 4 TYPES OF CHEMICAL REACTIONS & SOLUTION STOICHIOMETRY Day Plans for the day Assignment(s) for the day 4.2 The Nature of Aqueous Solutions o Strong v Weak Electrolytes Assignment 4.0 Assignment The Composition of Solutions Read section(s) o Solution, solute, solvent o Molarity o Dilution problems 4.4 Types of Chemical Reactions Read section(s) Precipitation Reactions Describing Reactions in Solution o Formula Equations o Net ionic Equations Stoichiometry of precipitation Assignment 4.2 reactions Read section(s) Acid-Base Reactions o Arrhenius v Brønsted-Lowry Assignment 4.3 Read section(s) o Strong acids & bases o Reactions o Titrations 4.9 Oxidation-Reduction Reactions Read section(s) o Definitions o Determining oxidation numbers 4.10 Balancing Oxidation Reduction 6 Reactions o The ½ reaction method acidic solution Balancing Oxidation Reduction 7 Reactions o The ½ reaction method basic solution Balancing Oxidation Reduction 8 Reactions o Change in oxidation number method 9 Work on assignment Assignment Grade & discuss assignment 11 Chapter 4 Test Read section(s) 6.1

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3 Advanced Chemistry Name Hour Study Guides Chapter 4 Quizzes Advanced Chemistry Quiz Electrolytes, Nonelectrolytes, & Solutions 1. Define a. electrolyte b. nonelectrolyte c. solute d. solvent e. strong electrolyte f. weak electrolyte 2. Write a chemical equation showing what happens when an electrolyte dissolves in water. 3. Write a chemical equation showing what happens when a nonelectrolyte dissolves in water. Quiz The Composition of Solutions 4. Define the term molarity. 5. Explain the process of dilution. 6. Calculate the molarity of a solution. 7. Calculate the molarity of ions in solution. Quiz Precipitation Reactions 8. Define the term precipitation reaction. 9. Define the term precipitate. 10. Use the solubility rules to determine whether a substance is soluble or insoluble in water. 4.7 Stoichiometry of Precipitation Reactions 11. Solve a solution stoichiometry problem. Quiz Acids & Bases 12. Define the following terms. a. acid b. base c. titration 13. Solve a titration problem.

4 Quiz Redox 14. Define the following terms. a. oxidation-reduction reaction b. oxidation state c. oxidation d. reduction 15. Give the oxidation state of each atom in a molecular or ion Balancing Redox Reactions 16. Use the ½ reaction method to balance a redox reaction in acidic solution. 17. Balance a redox reaction in basic solution.

5 Advanced Chemistry Name Hour Study Guide Chapter 4 Test Advanced Chemistry At the completion of chapter 4 you should 1. Know the definitions of the following terms. a. Electrolyte b. Nonelectrolyte c. Strong d. Weak e. Acid (Arrhenius and Bronsted-Lowry models) f. Base (Arrhenius and Bronsted-Lowry models) g. Molarity h. Dilution i. Precipitate j. Spectator Ions k. Titration l. Equivalence Point m. Oxidation State n. Oxidation o. Reduction p. Oxidizing Agent q. Reducing Agent 2. Be able to write chemical equations show what happens when an electrolyte and a nonelectrolyte dissolves in water. 3. Know the parts of a solution. 4. Be able to calculate the molarity of a solution. 5. Be able to use the solubility rules to determine if a substance is soluble or insoluble in water. 6. Be able to write and balance precipitation reactions. a. Formula Equations b. Net Ionic Equations 7. Know the strong acids and strong bases 8. Be able to write and balance acid-base reactions. a. Formula Equations b. Net Ionic Equations 9. Know how to solve titration problems. 10. Be able to balance oxidation reduction reactions. a. acid solution b. basic solution 11. Solve all types of solution stoichiometry problems.

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7 Advanced Chemistry Name Hour Assignment Vocabulary Define each of the following terms. 1. Electrolyte 2. Nonelectrolyte 3. Strong 4. Weak 5. Acid (Arrhenius & Bronsted Lowry models) 6. Base (Arrhenius & Bronsted Lowry models) 7. Molarity 8. Dilution 9. Precipitate 10. Spectator Ions

8 11. Titration 12. Equivalence Point 13. Oxidation State 14. Oxidation 15. Reduction 16. Oxidizing Agent 17. Reducing Agent

9 Advanced Chemistry Name Hour Assignment 4.1 Molarity Show all work. No work = no credit. 1) Calculate the molarity of each of these solutions. A) A g sample of NaHCO 3 is dissolved in enough water to make ml of solution. B) A mg sample of K 2 Cr 2 O 7 is dissolved in enough water to make ml of solution C) A g sample of copper metal is dissolved in 35 ml of concentrated HNO 3 to form Cu 2+ ions. Water is then added to make the total volume ml. Calculate the molarity of the Cu 2+ ion in the final solution. D) A solution of ethanol (C 2 H 5 OH) in water is prepared by dissolving 75.0 ml of ethanol (density = 0.79 g/cm 3 ) in enough water to make ml of solution. What is the molarity of the ethanol in this solution?

10 2) Calculate the molarity of all ions present in each of the following solutions of strong electrolytes. A) mol of sodium phosphate in 10.0 ml of solution B) mol of barium nitrate in ml of solution C) 1.00 g of potassium chloride in L of solution D) 132 g of ammonium sulfate in 1.50 L of solution

11 Advanced Chemistry Name 3) How would you prepare 1.00 L of 0.50 M solution of each of the following? A) H 2 SO 4 from concentrated (18 M) sulfuric acid Hour B) HCl from concentrated (12 M) reagent C) HNO 3 from concentrated (16 M) reagent D) NiCl 2 from the solid salt NiCl 2 6H 2 O E) sodium carbonate from the solid

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13 Advanced Chemistry Name Hour Assignment 4.2 Solubility and Precipitation Reactions Show all work. No work = no credit. 1) On the basis of the general solubility rules given in Table 4.1, predict which of the following substances are likely to be soluble in water. (Write soluble or insoluble.) A) zinc (II) chloride B) lead (II) nitrate C) lead (II) sulfate D) sodium iodide E) cobalt (III) sulfide F) chromium (III) hydroxide G) magnesium carbonate H) ammonium carbonate I) aluminum nitrate J) magnesium chloride K) rubidium sulfate L) nickel (II) hydroxide M) lead (II) sulfide N) magnesium hydroxide O) iron (III) phosphate

14 2) For each of the following pairs of reactants, decide if a precipitate will form. If a precipitate forms write the molecular equation and the net ionic equation for the reaction. If no precipitate forms write No reaction. A) Hg 2 (NO 3 ) 2 (aq) + CuSO 4 (aq) B) Ni(NO 3 ) 2 (aq) + CaCl 2 (aq) C) K 2 CO 3 (aq) + MgI 2 (aq) D) Na 2 CrO 4 (aq) + AlBr 3 (aq) 3) What volume of M Na 3 PO 4 is required to precipitate all of the silver ions from 75.0 ml of a M solution of AgNO 3?

15 Advanced Chemistry Name Hour 4) What mass of barium sulfate can be produced when ml of a M solution of barium chloride is mixed with ml of a M solution of iron (III) sulfate? 5) A 1.42 g sample of a pure compound, with formula M 2 SO 4, was dissolved in water and treated with an excess of aqueous calcium chloride, resulting in the precipitation of all of the sulfate ions as calcium sulfate. The precipitate was collected, dried, and found to weigh 1.36 g. Determine the atomic mass of M, and identify the element.

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17 Advanced Chemistry Name Hour Assignment 4.3 Acid-Base Reactions Show all work. No work = no credit. 1) Write the balanced molecular equation and the net ionic equation for each of the following acid-base reactions. A) HNO 3 (aq) + Al(OH) 3 (aq) B) HC 2 H 3 O 2 (aq) + KOH (aq) C) Ca(OH) 2 (aq) + HCl (aq) 2) What volume of each of the following bases will react completely with ml of M HCl? A) M NaOH B) M Ba(OH) 2 C) M KOH

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19 Advanced Chemistry Name Hour Assignment 4.4 Redox Reactions 1) Assign oxidation states for all atoms in each of the following compounds and ions. A) As 2 O 3 B) NaBiO 3 C) Cl 2 D) HAsO 2 E) UO 2 2+ F) MnO 4 1- G) CrO 4 2-2) Balance each of the following redox reactions in acidic solution. Indicate the species being oxidized, the species being reduced, the oxidizing agent and the reducing agent. A) Cu (s) + NO 3 1- (aq) Cu 2+ (aq) + NO (g) B) Cr 2 O 7 2- (aq) + Cl 1- (aq) Cr 3+ (aq) + Cl 2 (g)

20 C) Mn 2+ (aq) + BiO 3 1- (aq) Bi 3+ (aq) + MnO 4 1- (aq) D) H 3 AsO 4 (aq) + Zn (s) AsH 3 (g) + Zn 2+ (aq) 3) Balance each of the reactions in question #2 in basic solution.