AP+Chem+Acid+Base

The study of simple acid-base reactions allows us to investigate the details of a chemical reaction. We will carry out these investigations using the technique called titration.

Also study slides 1 to 38 on the powerpoint (See the file below this table). || 16.17, 16.19, 16.21, 16.23, 16.25, 16.27, 16.29 ||
 * Date of assignment || Due date ||= Details of reading assignment || Problems to do ||
 * February 19 || February 21 || Read very carefully section 16.6 on weak acids, up to page 633. Study the sample problems and examine figure 16.9. Pages 634 and 635 are less important than pages 628 to 633. Do the problems at the right. || 16.45 and 16.49 ||
 * March 1 || March 4 || Read sections 16.3 and 16.4, page 620 to 625. Study figure 16.5 (p 623).
 * March 1 || March 4 || Read section 16.5 to understand the definition of a strong acid. Do the problems at the right. These calculations are the same easy pH calculations you have completed in the previous assignment. The only difference is that the source of the H+ is identified. Problem 16.39 is a challenge that requires you to examine equation 16.23 on page 627. || 16.31, 16.33, 16.35, 16.37, 16.39 ||
 * March 1 || March 4 || Review of weak acid calculations. Do the problems listed at the right. || 16.43, 16.55 ||
 * March 1 || March 4 || Read section 16.1 and 16.2 up to page 617. Your goal is to understand the difference between a strong and a weak acid (or base) as well as the difference between the Arrhenius and Bronsted-Lowry definitions. ADDITIONAL READING that will help you with the concepts: Section 4.1 gives a nice summary of solubility and Chapter 20 of the Addison-Wesley book reviews pH calculations and acid-base definitions using easier-to-understand vocabulary. || 16.5, 16.7 ||
 * ||  || Read sections 16.7 and 16.8. Also read sections 17.1 to 17.3. Section 4.6 reviews the basic ideas involved in a titration. Page 141 has a nice pictorial summary. || 16.61, 16.63, 16.65, 16.67 and 17.27, 17.29, 17.31 and 17.13. ||
 * ||  || Create a pH for the titration of 0.075 M nitric acid with 0.10 M sodium hydroxide. The original volume of the acid sample is 100.0 mL. According to Mr. Robinson's calculations, the amount of sodium hydroxide needed to neutralize the acid completely (reach the equivalence point) is 75.00 mL. Use stoichiometric calculations to complete the table shown below. Then, using a spreadsheet, plot the pH versus volume of base added. SECTION 17.3 reviews the ideas we covered in class on Friday, January 14. ||   ||
 * ||  ||   || 16.5, 16.7, 16.9, 16.11 ||
 * ||  || To understand weak and strong acids and bases, review Sections 16.5, 16.6, and 16.7. These sections are long, but you can get the major ideas quickly by focusing on the following sample exercises: 16.8 and 16.9 on page 626, 16.10 on page 629, and 16.14 on page 637. || 16.33, 16.35, 16.53, pages 655 and 656 ||
 * || Test Review || Studying titration curves is a good way to review all of the acid-base chemistry we have learned.

The two pdf files below summarize the work we did in the review sessions.

Titrating a strong acid with a strong base:

Titrating a weak acid with a strong base: || Sections 1 to 9 of chapter 16 are included. Sections 2 and 3 of chapter 17 are included. Section 16.10 is a good essay to read. Section 16.11 will be covered later. ||
 * || Unit Test ||  ||   ||

Here is a powerpoint for this unit.

The following pages contain data from experiments.

Titration of Acetic (Ethanoic) Acid, also known as vinegar.

How to review this information:
 * Step || Exercise ||
 * 1. || List the formulas of all seven strong acids. Write equations for their dissociation (single-sided arrow). Use hydronium in the equation. ||
 * 2. || Write the equations for the dissociation of these two weak acids: hydrofluoric (HF) and acetic (CH3COOH). ||
 * 3. || In the equations you have written, label all conjugate acid - conjugate base pairs. ||
 * 4. || Draw the Lewis structures for hydronium ion and acetate ion. ||
 * 5. || List the formulas of all eight strong bases. Write equations for their dissociation (single-sided arrow). ||
 * 6. || Write the equations for the dissociation of these two weak bases: magnesium hydroxide - Mg(OH)2 - and ammonia (NH3). ||
 * 7. || In the equation for ammonia in water, label the conjugate acid - conjugate base pairs. ||
 * 8. || Draw the Lewis structure for ammonium. ||
 * 9. || Write the equilibrium expression for any of the weak acid or weak base equilibria i.e. Ka = [products] / [reactants] ||

Important Vocabulary: complete dissociation partial dissociation or incomplete dissociate monoprotic, diprotic, triprotic, polyprotic Arrhenius Bronsted-Lowry