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CHAPTER 5 Reactions in Aqueous Solution

CHAPTER 5 Reactions in Aqueous Solution. Turn in homework for Chapter 4. Road Map. Where we were Percent yield Chemical equations and chemical analysis Where we are going Review problems

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CHAPTER 5 Reactions in Aqueous Solution

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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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