Chapter 14 Acids and Bases

Chapter 14 – Acids and Bases Section 14:1 The Nature of Acids and Bases What are the properties of acids and bases?

Describe the role of equilibrium in acid-base chemistry.

Describe each of the following Acid-Base Models: 1. Arrhenius

2. Lewis

3. Bronsted-Lowry

Section 14.2 Acid Strength Describe a strong acid:

-What are the six strong acids?

Describe a weak acid:

What is the difference between strong and weak acids?

Define the following: Monoprotic Acid

Diprotic Acid

Oxyacid

Organic Acid Water as an Acid and a Base Define amphoteric

Describe the autoionization of water

Write the equilibrium expression for the autoionization of water

Product of [H+] and [OH-] values:  In a neutral solution,

 In an acidic solution,

 In a basic solution,

Calculate the [H+] and [OH-] in the following solutions at 25 °C

a. 0.01 M HClO4

b. 0.050 M HNO3

Section 14.3 The pH scale The pH scale depends upon

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

+ - Calculate the [H3O ], [OH ], pH and pOH for a 0.015 M HNO3 solution.

+ - 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?

Section 14.5 Calculating the pH of a weak acid

Example: What is the pH of a 0.2 M solution of HIO3. The ka value for HIO3 is 0.17.

-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

Percent Dissociation Equation:

Example: Calculate the percent dissociation of a 0.20 M solution of HNO2. The Ka -4 value for HNO2 is 4.0 x 10 .

Example: Calculate ka value for a 0.01 solution of acetic acid that is has a percent dissociation of 4.2%.

Section 14:6 Bases Give some examples of strong bases:

Give some examples of weak bases:

Calculate the pH of a 9.8 x 10-4 M NaOH solution at 25 C

Calculate the [OH-], pH and percent dissociation for a 2.0 M aqueous NH3 solution.

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?

Types of Salts from Acid-Base Solutions Salt pH of solution Strong base + Strong acid

Strong base + Weak acid

Weak base + Strong acid

Weak base + Weak acid

Example: Salt of a Strong Base + Weak Acid: -5 Calculate the pH for 0.10 NaCN. The kb for CN = 2.5 x 10 .

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.

Classify the following as an acidic, basic or neutral salt. 1) (NH4)2SO4 2) NH4NO3 3) Na2CO3