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Aqueous Solution Reactions: Understanding Molecular Equations and Stoichiometry

Chapter 5 delves into the complexities of reactions in aqueous solutions, focusing on identifying chemical equations and understanding stoichiometric conversions. Critical skills such as naming common ions and writing electrically neutral formulas are emphasized. The chapter covers various reaction types, including precipitation, neutralization, and gas-forming reactions, along with practice problems that challenge your understanding. Students will learn to write molecular, total ionic, and net ionic equations, enhancing their analytical skills essential in chemistry.

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Aqueous Solution Reactions: Understanding Molecular Equations and Stoichiometry

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  1. CHAPTER 5 Reactions in Aqueous Solution Turn in homework for Chapter 4 Chem 105 Chpt 4 Lsn 10

  2. Road Map • Where we were • Percent yield • Chemical equations and chemical analysis • Where we are going • Review problems • Critical skills: naming common ions, writing electrically neutral formulas/reactions, stoichiometric conversions • Types of reactions Chem 105 Chpt 4 Lsn 10

  3. Determining the Formula of an Unknown Compound: Molecular Formulas Chem 105 Chpt 4 Lsn 10

  4. Chem 105 Chpt 4 Lsn 10 p.162b

  5. Chemical Analysis/Equation • A dry-cleaning solvent (M = 146.99 g/mol) that contains C, H, and Cl is suspected to be a cancer-causing agent. When a 0.250 g sample was studied by combustion analysis, 0.451 g of CO2 and 0.0617 g of H2O formed. Calculate the molecular formula. • Empirical C3H2Cl • Molecular C6H4Cl2 Chem 105 Chpt 4 Lsn 10

  6. Are you up to the challenge? • Iodine is made by the reaction 2 NaIO3 (aq) + 5 NaHSO3 (aq)  3 NaHSO4 (aq) + 2 Na2SO4 (aq) + H2O (l) + I2 • Name the two reactants • If you wish to prepare 1.00 kg of I2, what mass of NaIO3 is required? • What mass of NaHSO3? Chem 105 Chpt 4 Lsn 10

  7. 5.1 Aqueous solutions • Hyponitriemia • Electrolytes: aqueous solutions which conduct electricity • Strong – complete/nearly complete dissociation • Weak – only partial dissociation • Figure 5.3, page 179 (know) Chem 105 Chpt 4 Lsn 10

  8. 5.2 Precipitation reactions Writing Equations for Aqueous Ionic Reactions • Three types of equations are used to represent aqueous ionic reactions: molecular, total ionic, and net ionic equations. • molecular equation: shows all reactants and products as if they were intact, undissociated • total ionic equation: shows all the soluble ionic substances dissociated into ions. Charges must balance • Spectator ions not involved in chemical change. • net ionic equation: it eliminates the spectator ions and shows the actual chemical change taking place. Chem 105 Chpt 4 Lsn 10

  9. Practice Problem 10-1 • molecular equation Pb(NO3)2(aq) + K2CrO4(aq) → PbCrO4(s) + 2 KNO3(aq) • Write the Total Ionic and Net Ionic equations for • Total • Net Chem 105 Chpt 4 Lsn 10

  10. Practice Problem 10-2 • Write the Total Ionic and Net Ionic equations for HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) Chem 105 Chpt 4 Lsn 10

  11. Practice Problem 10-3 • Solutions of iron (III) chloride and potassium hydroxide give iron (III) hydroxide and potassium chloride when combined. • Write the • Molecular equation • Total ionic equation • Net ionic equation Chem 105 Chpt 4 Lsn 10

  12. 5.3 – Acids and Bases(know table 5.2) • Acid: increases the H+ concentration • Base: increases the OH- concentration • Strong acid: completely dissociates/ionizes • Weak acid: partial ionization Chem 105 Chpt 4 Lsn 10

  13. 5.4 - Reactions of Acids and Bases • An Acid reacting with a base produce a salt and water • Neutralization reaction: a strong acid with a strong base Chem 105 Chpt 4 Lsn 10

  14. Lesson summary • Calcium chloride and potassium phosphate combine to form calcium phosphate and potassium chloride. • Write the molecular equation 3 CaCl2(aq) + 2 K3PO4(aq) → Ca3PO4(s) + 6 KCl(aq) • Write the Total Ionic and Net Ionic equations Chem 105 Chpt 4 Lsn 10

  15. 3 CaCl2(aq) + 2 K3PO4(aq) → Ca3PO4(s) + 6 KCl(aq) • Write the Total Ionic and Net Ionic equations • Combining 5 grams CaCl2 with 3.5 grams of K3PO4 produced only a 67% yield of KCl. • What is the limiting reactant? • What mass of product did you make? Chem 105 Chpt 4 Lsn 10

  16. Next Lesson • Chapter 5 • Gas forming reactions • Classifying reactions • Oxidation reactions • Measuring concentrations of compounds in solution • pH • Stoichiometry of reactions in aqueous solution Chem 105 Chpt 4 Lsn 10

  17. Practice Problem 10-4 • Write the Total Ionic and Net Ionic equations for CaCl2(aq) + Na2CO3(aq) → CaCO3(s) + 2 NaCl(aq) Chem 105 Chpt 4 Lsn 10

  18. Practice Problem 10 - 5 • Write the Total Ionic and Net Ionic equations for Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g) Chem 105 Chpt 4 Lsn 10

  19. Chem 105 Chpt 4 Lsn 10

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