CHAPTER 15 APPLICATIONS OF AQUEOUS EQUILIBRIA

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1 Advanced Chemistry Name Hour Advanced Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 15 APPLICATIONS OF AQUEOUS EQUILIBRIA Day Plans for the day Assignment(s) for the day 15.1 Solution of Acids or Bases Assignment Containing a Common Ion 15.2 Buffered Solutions Assignment 15.1a Read section(s) Buffering Capacity Assignment 15.1b Read section(s) Titrations & ph Curves Read section(s) Acid-Base Indicators 15.6 Solubility Equilibria & the 4 Solubility Product o K sp o Problems Solubility Equilibria & the Solubility Product o K sp o Problems Assignment 15.2a Read section(s) Precipitation & Qualitative Assignment 15.2b Analysis 7 Grade & discuss assignment Review for Chapter 15 Test 8 Chapter 15 Test Read section(s)

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3 Advanced Chemistry Name Hour Study Guides Chapter 15 Quizzes Quiz Solutions of Acids or Bases Containing a Common Ion 1. Imagine making a single solution containing BOTH NaF and HF dissolved in water. What is the common ion shared by the chemicals in this solution? 15.2 Buffered Solutions 2. Define the term buffered solution. 3. In addition to water, all buffered solutions contain two chemicals. What are these two chemicals? 4. Calculate the ph of a buffered solution Buffering Capacity 5. Define the term "buffering capacity". 6. When is a buffer most effective? Quiz 15.6 Solubility Equilibria & the Solubility Product 7. What does the symbol "K sp " stand for? 8. Distinguish the terms "solubility" and "solubility product". 9. Calculate the solubility of a compound in water. 10. Calculate the K sp value of a compound given its solubility.

4 Study Guide Chapter 15 Test Advanced Chemistry At the completion of chapter 15 you should 1. Know the definitions of the following terms. a. Common Ion Effect b. Buffered Solution c. Equivalence Point d. Acid-base Indicator e. Solubility Product (Constant) 2. Calculate the ph of a buffered solution a. before adding acid or base b. after adding acid or base 3. Understand what is meant by the term buffer capacity. 4. Calculate the ph, at the equivalence point, of an acid-base titration. a. strong acid with strong base b. weak acid with strong base c. strong acid with weak base 5. Understand how an acid-base indicator works at the molecular level. 6. Understand how an acid-base indicator is chosen. 7. Calculate the value of K sp from solubility data. 8. Calculate the solubility of a compound from its K sp value. 9. Understand how a common ion affects solubility.

5 Advanced Chemistry Name Hour Assignment 15.0 Vocabulary Define each of the following terms. 1. Common Ion Effect 2. Buffered Solution 3. Equivalence Point 4. Acid-base Indicator 5. Solubility Product (Constant)

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7 Advanced Chemistry Name Hour Assignment 15.1a Buffers (#1) 1) In addition to water, what two things are needed to make a buffer? A) B) 2) Calculate the ph of each of the following solutions. A) M HONH 2 (K b = 1.1 x 10-8 ) B) M HONH 3 Cl C) Pure water D) A mixture containing M HONH 2 and M HONH 3 Cl

8 3) Which of the solutions in question #2 is a buffered solution? 4) Calculate the ph of a solution that is 0.60 M HF and 1.00 M KF. 5) Calculate the ph after 0.10 mol of NaOH is added to 1.00 L of the solution in problem #4. 6) Calculate the ph after 0.20 mol of HCl is added to 1.00 L of the solution in problem #4.

9 Advanced Chemistry Name Hour Assignment 15.1b Buffers (#2) 1) An aqueous solution contains dissolved C 6 H 5 NH 3 Cl and C 6 H 5 NH 2. The concentration of C 6 H 5 NH 2 is 0.50 M and the ph is Calculate the concentration of C 6 H 5 NH ) Consider a solution that contains both C 5 H 5 N and C 5 H 5 NHNO 3. Calculate the ratio [C 5 H 5 N] / [ C 5 H 5 NH + ] if the solution has the following ph values. A) ph = 4.50 B) ph = 5.00 C) ph = 5.23 D) ph = 5.50

10 3) Which of the following mixtures would result in a buffered solution when 1.0 L of each of the two solutions are mixed? Answer YES if the resulting solution is a buffer and NO if it is not a buffer. A) 0.2 M HNO 3 and 0.40 M NaNO 3. B) 0.2 M HNO 3 and 0.40 M HF. C) 0.2 M HNO 3 and 0.40 M NaF D) 0.2 M HNO 3 and 0.40 M NaOH

11 Advanced Chemistry Name Hour Assignment 15.2a Solubility Equilibria (#1) 1) Write balanced equations for the dissolution reaction and the corresponding solubility product expressions for each of the following solids. A) AgC 2 H 3 O 2 B) Al(OH) 3 C) Ca 3 (PO 4 ) 2 D) Ag 2 CO 3 E) Ce(IO 3 ) 3 F) BaF 2

12 2) Use the following data to calculate the K sp value for each solid. A) The solubility of Pb 3 (PO 4 ) 2 is 6.2 x mol/l. B) The solubility of Li 2 CO 3 is 7.4 x 10-2 mol/l. 3) The concentration of Ag + in a solution saturated with Ag 2 C 2 O 4 is 2.2 x 10-4 M. Calculate K sp for Ag 2 C 2 O 4.

13 Advanced Chemistry Name Hour Assignment 15.2b Solubility Equilibria (#2) 1) Calculate the solubility of each of the following compounds in moles per liter. Ignore any acid-base properties. A) CaCO 3, K sp = 8.7 x 10-9 B) PbI 2. K sp =1.4 x 10-8 C) CdCO 3, K sp =5.2 x D) Sr 3 (PO 4 ) 2, K sp = 1 x 10-31

14 2) Will a precipitate form when ml of 4.0 x 10-4 M Mg(NO 3 ) 2 is added to ml of 2.0 x 10-4 M NaOH? 3) A solution is prepared by mixing 50.0 ml of 0.10 M Pb(NO 3 ) 2 with 50.0 ml of 1.0 M KCl. Calculate the concentrations of Pb 2+ and Cl - at equilibrium. K sp = 1.6 x 10-5