1. Review 4 Exam 4 on Chapters 9, 15 and 16

2. Chapter 9 Chemical Reactions Sections (9.1, 9.2 9.3) omit Rest of the sections Moles  moles of reactants and products –Start from Balanced chemical Equation –Moles is like cups in a recipe –In moles to moles problem – Moles from Balanced chemical equation –NO NEED TO CALCULATE molar mass, Avogadro number etc. Grams  Grams of reactants and products –Start from Balanced chemical Equation –Calculate the molar masses for things in question –Multiply by the coefficients with molar masses for stoichiometric equivalence Moles  Grams of reactants and products –Moles = weight in grams/molar mass

3. 15.2 Solutions: Homogeneous Mixtures A. Any homogenous mixture is a solution B. Solute: major component C. Solute: minor component, can be more than one 15.3 Solutions of Solids Dissolved in Water: How to Make Rock Candy A. Solubility and Saturation 1. Saturated: solvent holding as much solute as it can 2. Unsaturated: solvent can hold more solute 3. Supersaturated: solvent holding more than the maximum amount of solute B. Electrolyte solutions: dissolved ionic solids 1. Strong electrolyte solution 2. Nonelectrolyte solution C. Solubility is temperature dependent D. Rock candy 15.4 Solutions of Gases in Water: How Soda Pop Gets Its Fizz A. Solubility is a function of temperature and pressure B. Dilute vs. concentrated Chapter 15 Chapter 9 Balance equations First!!! Calculations in chemical reaction how much reactant will produce how much product, moles to moles, grams to grams etc- STOICHIOMETRY

4. 15.5 Specifying Solution Concentration: Mass Percent A.Mass percent = B.B. Conversion factor between amount of solution and amount of a particular solute 15.6 Specifying Solution Concentration: Molarity A. Molarity (M) = B. Volume of solution, not just solvent C. Units always mol/L D. Ion concentrations 15.8 Solution Stoichiometry A. Balanced chemical equations give molar ratios only B. Convert volume to moles using molarity, then use balanced chemical equation

5. 16.1 Sour Patch Kids and International Spy Movies 16.2 Acids: Properties and Examples A. Sour taste B. Dissolve many metals C. Turn litmus paper red D. Common acids 1. HCl is hydrochloric acid 2. H 2 SO 4 is sulfuric acid 3. HNO 3 is nitric acid 16.3 Bases: Properties and Examples A. Bitter taste B. Feel slippery C. Turn litmus paper blue D. Common bases 1. Ammonia NH 3 2. Sodium hydroxide NaOH 3. Sodium bicarbonate NaHCO 3 Chapter 16

6. 16.4 Molecular Definitions of Acids and Bases A. Arrhenius definition 1. Acids produce H+ ions in aqueous solution 2. Bases produce OH- ions in aqueous solution B. H+ is actually H3O+ C. Brønsted-Lowry Definition 1. Acids are proton (H+) donors 2. Base are proton (H+) acceptors D. Conjugate acid-base pairs 16.5 Reactions of Acids and Bases A. Neutralization reactions B. Acid reactions C. Base reactions

7. 16.6 Acid-Base Titrations: A Way to Quantify the Amount of Acid or Base in a Solution A. Add solution of known concentration to solution of unknown concentration B. Equivalence (end) point C. Indicator M a V a = M b V b For 1:1 acid base stoichiometry Check acid base formula to adjust the stoichiometry 16.7 Strong and Weak Acids and Bases A Strong acids are strong electrolytes B. Weak acids are weak electrolytes C. Diprotic and triprotic acids D. Strong bases E. Weak bases

8. 16.8 Water: Acid and Base in One A. Amphoteric B. All aqueous solution contains both H3O+ and OH- C. Kw = [H3O+][OH-] D. Acid : [H3O+] > 1.0 x 10-7 M E. Base : [H3O+] < 1.0 x 10-7 M 16.9 The pH Scale: A Way to Express Acidity and Basicity A. pH = -log[H3O+] B. In a acidic solution, pH <7 C. In a neutral solution, pH =7 D. In a basic solution, pH >7 16.10 Buffers: Solutions That Resist pH Change A. Resist pH change B. Contain both a weak acid and its conjugate base C. Weak acid neutralizes added base D. Conjugate base neutralizes added acid