1. Chem 105 Chpt 4 Lsn 11 1 CHAPTER 5 Reactions in Aqueous Solution Turn in homework for Chapter 4 Turn in homework for Chapter 4

2. Chem 105 Chpt 4 Lsn 11 2 Road Map Where we were Where we were Chemical equations and chemical analysis review problems Chemical equations and chemical analysis review problems Where we are going Where we are going Critical skills: naming common ions, writing electrically neutral formulas/reactions, stoichiometric conversions Critical skills: naming common ions, writing electrically neutral formulas/reactions, stoichiometric conversions Types of reactions Types of reactions Use: Figure 5.3, page 179 Use: Figure 5.3, page 179 Know: Table 5.2, pg 182 Know: Table 5.2, pg 182

3. Chem 105 Chpt 4 Lsn 11 3 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.

4. Chem 105 Chpt 4 Lsn 11 4 Practice Problem 10-1 molecular equation Pb(NO 3 ) 2 (aq) + K 2 CrO 4 (aq) → PbCrO 4 (s) + 2 KNO 3 (aq) Write the Total Ionic and Net Ionic equations for Total Net

5. Chem 105 Chpt 4 Lsn 11 5 Practice Problem 10-2 Write the Total Ionic and Net Ionic equations for CaCl 2 (aq) + Na 2 CO 3 (aq) → CaCO 3 (s) + 2 NaCl(aq)

6. Chem 105 Chpt 4 Lsn 11 6 Practice Problem 10-3 Solutions of iron (III) chloride and potassium hydroxide give iron (III) hydroxide and potassium chloride when combined. Solutions of iron (III) chloride and potassium hydroxide give iron (III) hydroxide and potassium chloride when combined. Write the Write the Molecular equation Molecular equation Total ionic equation Total ionic equation Net ionic equation Net ionic equation

7. Chem 105 Chpt 4 Lsn 11 7 5.3 – Acids and Bases (know table 5.2) Acid: increases the H + concentration Acid: increases the H + concentration Base: increases the OH - concentration Base: increases the OH - concentration Strong acid: completely dissociates/ionizes Strong acid: completely dissociates/ionizes Weak acid: partial ionization Weak acid: partial ionization

8. Chem 105 Chpt 4 Lsn 11 8 5.4 - Reactions of Acids and Bases An Acid reacting with a base produce a An Acid reacting with a base produce a salt and water Neutralization reaction: a strong acid with a strong base Neutralization reaction: a strong acid with a strong base

9. Chem 105 Chpt 4 Lsn 11 9 Practice Problem 10 - 4 Calcium chloride and potassium phosphate combine to form calcium phosphate and potassium chloride. Write the molecular equation 3 CaCl 2 (aq) + 2 K 3 PO 4 (aq) → Ca 3 PO 4 (s) + 6 KCl(aq) Write the Total Ionic and Net Ionic equations

10. Chem 105 Chpt 4 Lsn 11 10 3 CaCl 2 (aq) + 2 K 3 PO 4 (aq) → Ca 3 PO 4 (s) + 6 KCl(aq) Write the Total Ionic and Net Ionic equations Combining 5 grams CaCl 2 with 3.5 grams of K 3 PO 4 produced only a 67% yield of KCl. What is the limiting reactant? What mass of product did you make?

11. Chem 105 Chpt 4 Lsn 11 11 5.8 Measuring Concentrations How many moles of each ion are in each solution? (a) 2 mol of potassium perchlorate dissolved in water (b) 354 g of magnesium acetate dissolved in water (c) 1.88 x 10 24 formula units of ammonium chromate dissolved in water (d) 1.32 L of 0.55 M sodium bisulfate

12. Chem 105 Chpt 4 Lsn 11 12 5.8 Measuring Concentrations How many moles of H + (aq) are present in 451 mL of 3.20 M hydrobromic acid?

13. Chem 105 Chpt 4 Lsn 11 13 5.4 Acid-Base Reactions: Acid-Base Titrations What volume of 0.1292 M Ba(OH) 2 would neutralize 50.00 mL of the HCl solution standardized in the preceding sample problem (4.5) ?

14. Chem 105 Chpt 4 Lsn 11 14 Precipitation Reactions: Predicting Whether a Precipitate Will Form Predict whether a reaction occurs, and write balanced total and net ionic equations. (a) iron(III) chloride(aq) + cesium phosphate(aq) → (b) sodium hydroxide(aq) + cadmium nitrate(aq) → (c) magnesium bromide(aq) + potassium acetate(aq) → (d) silver sulfate(aq) + barium chloride(aq) →

15. Chem 105 Chpt 4 Lsn 11 15 Next Lesson Chapter 5 Chapter 5 Gas forming reactions Gas forming reactions Classifying reactions Classifying reactions Oxidation reactions Oxidation reactions Measuring concentrations of compounds in solution Measuring concentrations of compounds in solution pH pH Stoichiometry of reactions in aqueous solution Stoichiometry of reactions in aqueous solution

16. Chem 105 Chpt 4 Lsn 11 16 Practice Problem 10 - 5 Write the Total Ionic and Net Ionic equations for Zn(s) + H 2 SO 4 (aq) → ZnSO 4 (aq) + H 2 (g)

17. Chem 105 Chpt 4 Lsn 11 17 Practice Problem 10-6 Write the Total Ionic and Net Ionic equations for HCl(aq) + NaOH(aq) → NaCl(aq) + H 2 O(l)