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Chapter 16 Aqueous Equilibria: Applications 1. neutralization reactions

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 K f solubility

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Chapter 16 Aqueous Equilibria: Applications 1. neutralization reactions

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

  2. 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, NH41+, NO31-, ClO31-, ClO41-, C2H3O21- • 2. compounds with the following ions are usually soluble: • Cl1-, Br1-, I1- (except: Ag1+, Hg22+, Pb2+ compounds) • SO42- (except: Ba2+, Hg22+, Pb2+ compounds) Chapter 16 Notes

  3. The chemistry:some examples. • Write the products for the reaction using the solubility rules. • Write the net ionic equation.. • 1. NaCl(aq)+AgNO3(aq) • 2. K2SO4(aq)+Pb(ClO4)2(aq)  • 3. Write a balanced chemical equation and net ionic equation showing how calcium fluoride could be made. Chapter 16 Notes

  4. Ksp & 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 Na1+ and six different water molecules surround each Cl1-? (about 29g) Solubility and equilibria: some examples. AgCl(s)Ag1+(aq)+Cl1-(aq) Bi2S3(s)  2Bi3+(aq)+3S2-(aq) AgCl and Bi2S3 are insoluble according to rules Chapter 16 Notes

  5. Solubility and equilibria: Ksp. AgCl(s)  Ag1+(aq)+Cl1-(aq) Bi2S3(s)  2Bi3+(aq)+3S2-(aq) Chapter 16 Notes

  6. Solubility and equilibria: Ksp. AgCl(s) Ag1+(aq)+Cl1-(aq) Bi2S3(s) 2Bi3+(aq)+3S2-(aq) Calculations: 1. What is the solubility of AgCl (Ksp=1.8x1010)? Working definition of solubility: moles of compound dissolved in one liter of solution; symbol S. 2. The solubility of Bi2S3 is 1.0x10-15 M; what is Ksp? Chapter 16 Notes

  7. Solubility and equilibria: Ksp. • AgCl(s) Ag1+(aq)+Cl1-(aq) • Calculations: • 3. If 100.0 ml of 0.10 M AgNO3 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 Ksp and Qsp (your book refers to Qsp as IP, for ion product) to determine if a precipitate will form Chapter 16 Notes

  8. common ion effect Bi2S3(s) 2Bi3+(aq)+3S2-(aq) Calculations: 4. Calculate the solubility of Bi2S3 in a 0.0010 M Na2S solution; compare your answer to the solubility of Bi2S3 in pure water. Chapter 16 Notes

  9. Figure 16.11 Chapter 16 Notes

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

  11. 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. MgF2 • b. AgCl • c. PbSO4 • d. CaCO3 • e. FeS Chapter 16 Notes

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