1. Chapter 16 Notes1 Chapter 16 Aqueous Equilibria: Applications 1. neutralization reactions 2. common ion effect; buffers 3. titrations 4. solubility equilibria review precipitation reactions and solubility rules K sp & solubility common ion effect solubility & pH 5. complex ion formation KfKf solubility (6. selective precipitation; qualitative analysis)

2. Chapter 16 Notes2 4. solubility equilibria review precipitation reactions and solubility rules “insoluble” compounds: <0.1 g/L rules: 1. compounds with the following ions are soluble: Group 1A cations, NH 4 1+, NO 3 1-, ClO 3 1-, ClO 4 1-, C 2 H 3 O 2 1- 2. compounds with the following ions are usually soluble: Cl 1-, Br 1-, I 1- (except: Ag 1+, Hg 2 2+, Pb 2+ compounds) SO 4 2- (except: Ba 2+, Hg 2 2+, Pb 2+ compounds)

3. Chapter 16 Notes3 The chemistry:some examples. Write the products for the reaction using the solubility rules. Write the net ionic equation.. 1. NaCl(aq)+AgNO 3 (aq)  2. K 2 SO 4 (aq)+Pb(ClO 4 ) 2 (aq)  3. Write a balanced chemical equation and net ionic equation showing how calcium fluoride could be made.

4. Chapter 16 Notes4 K sp & solubility: No compound is infinitely soluble; no compound in perfectly insoluble. What is the maximum mass of NaCl that can be dissolved in water, assuming six water molecules surround each Na 1+ and six different water molecules surround each Cl 1- ? (about 29g) Solubility and equilibria: some examples. AgCl(s)  Ag 1+ (aq)+Cl 1- (aq) Bi 2 S 3 (s)  2Bi 3+ (aq)+3S 2- (aq) AgCl and Bi 2 S 3 are insoluble according to rules

5. Chapter 16 Notes5 Solubility and equilibria: K sp. AgCl(s)  Ag 1+ (aq)+Cl 1- (aq) Bi 2 S 3 (s)  2Bi 3+ (aq)+3S 2- (aq)

6. Chapter 16 Notes6 Solubility and equilibria: K sp. AgCl(s)Ag 1+ (aq)+Cl 1- (aq) Bi 2 S 3 (s)2Bi 3+ (aq)+3S 2- (aq) Calculations: 1. What is the solubility of AgCl (K sp =1.8x10 10 )? Working definition of solubility: moles of compound dissolved in one liter of solution; symbol S. 2. The solubility of Bi 2 S 3 is 1.0x10 -15 M; what is K sp ?

7. Chapter 16 Notes7 Solubility and equilibria: K sp. AgCl(s)Ag 1+ (aq)+Cl 1- (aq) Calculations: 3. If 100.0 ml of 0.10 M AgNO 3 are mixed with 200.0 ml of 0.010 M NaCl, what happens? first, write out the chemical equation describing what you think might happen second, use K sp and Q sp (your book refers to Q sp as IP, for ion product) to determine if a precipitate will form

8. Chapter 16 Notes8 common ion effect Bi 2 S 3 (s)2Bi 3+ (aq)+3S 2- (aq) Calculations: 4. Calculate the solubility of Bi 2 S 3 in a 0.0010 M Na 2 S solution; compare your answer to the solubility of Bi 2 S 3 in pure water.

9. Chapter 16 Notes9 Figure 16.11

10. Chapter 16 Notes10 solubility and pH 5. The solubility of Mg(OH) 2 increases in acidic solutions. Explain, using chemical equations and considering driving forces.

11. Chapter 16 Notes11 solubility and pH 6. Decide whether the solubility of the following salts increases significantly, slightly, or not at all in acidic solution. Write balanced chemical equations for each salt to support your answer, and identify the important driving forces. a. MgF 2 b. AgCl c. PbSO4 d. CaCO 3 e. FeS