<p> Chapter 14 – Acids and Bases Section 14:1 The Nature of Acids and Bases What are the properties of acids and bases?</p><p>Describe the role of equilibrium in acid-base chemistry.</p><p>Describe each of the following Acid-Base Models: 1. Arrhenius</p><p>2. Lewis</p><p>3. Bronsted-Lowry</p><p>Section 14.2 Acid Strength Describe a strong acid:</p><p>-What are the six strong acids?</p><p>Describe a weak acid:</p><p>What is the difference between strong and weak acids?</p><p>Define the following: Monoprotic Acid</p><p>Diprotic Acid</p><p>Oxyacid</p><p>Organic Acid Water as an Acid and a Base Define amphoteric</p><p>Describe the autoionization of water</p><p>Write the equilibrium expression for the autoionization of water</p><p>Product of [H+] and [OH-] values:  In a neutral solution, </p><p> In an acidic solution,</p><p> In a basic solution,</p><p>Calculate the [H+] and [OH-] in the following solutions at 25 °C</p><p> a. 0.01 M HClO4</p><p> b. 0.050 M HNO3</p><p>Section 14.3 The pH scale The pH scale depends upon</p><p>Calculate the pH, pOH for the following: + -9 a. a solution whose [H3O ] = 6.2 x 10 b. a solution whose [OH-] = 2.3 x 10-12</p><p>+ - Calculate the [H3O ], [OH ], pH and pOH for a 0.015 M HNO3 solution.</p><p>+ - Calculate the [H3O ], [OH ], pH and pOH for a 0.015 M Ca(OH)2 solution. Section 14.4 Calculating the pH of a strong acid Example: What is the pH of a 5.0 M HCl aqueous solution?</p><p>Section 14.5 Calculating the pH of a weak acid</p><p>Example: What is the pH of a 0.2 M solution of HIO3. The ka value for HIO3 is 0.17. </p><p>-4 Mixtures: Calculate the pH of a solution that contains 1.0 M HF(Ka value of 7.2 x 10 ) and -10 - 1.0 M HOC6H5(Ka value of 1.6 x 10 ). Also, calculate the concentration of OC6H5 in this solution at equilibrium</p><p>Percent Dissociation Equation:</p><p>Example: Calculate the percent dissociation of a 0.20 M solution of HNO2. The Ka -4 value for HNO2 is 4.0 x 10 .</p><p>Example: Calculate ka value for a 0.01 solution of acetic acid that is has a percent dissociation of 4.2%.</p><p>Section 14:6 Bases Give some examples of strong bases:</p><p>Give some examples of weak bases:</p><p>Calculate the pH of a 9.8 x 10-4 M NaOH solution at 25 C</p><p>Calculate the [OH-], pH and percent dissociation for a 2.0 M aqueous NH3 solution.</p><p>Section 14:7 Polyprotic Acids Section 14:8 Acid-Base Properties of Salts What type of reaction is formed from the reaction of an acid and a base? What is the K value?</p><p>Types of Salts from Acid-Base Solutions Salt pH of solution Strong base + Strong acid</p><p>Strong base + Weak acid</p><p>Weak base + Strong acid</p><p>Weak base + Weak acid</p><p>Example: Salt of a Strong Base + Weak Acid: -5 Calculate the pH for 0.10 NaCN. The kb for CN = 2.5 x 10 .</p><p>Example: Salt of a Weak Base + Strong Acid + Calculate the pH of a 0.20 M solution of ammonium nitrate, NH4NO3. The Ka value of NH4 is 5.6 x 10-10.</p><p>Classify the following as an acidic, basic or neutral salt. 1) (NH4)2SO4 2) NH4NO3 3) Na2CO3</p>