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Assignment #71 Precipitates

This assignment focuses on predicting whether a precipitate will form in various chemical reactions based on the ion product (Q) and the solubility product constant (Ksp). The discussion includes scenarios such as the dissolution of silver iodide at higher temperatures and subsequent cooling, alongside examples using lead(II) nitrate and potassium iodide. The chemistry concepts of complete ionic and net ionic equations are explored, emphasizing the identification of spectator ions. Essential for understanding solubility and precipitation reactions in regular chemistry.

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Assignment #71 Precipitates

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  1. Assignment #71Precipitates Regular Chemistry

  2. Predicting Precipitation • Ion Product • Q for Dissolution Problems • 9.0x10-7g of silver iodide is dissolved in 250mL of solution at 95°C. If the solution is allowed to cool to 25°C, will a precipitate form? • Q = 2.3x10-16 • Q > Ksp • Shift to the Left. • Precipitate Forms Regular Chemistry

  3. Solubility Rules • Predict if a precipitate forms. • Page 574 • Back of Periodic Table • Pb(NO3)2(aq.) + KI(aq.) Regular Chemistry

  4. Solubility Rules • Predict if a precipitate forms. • Page 574 • Back of Periodic Table • Pb(NO3)2(aq.) + KI(aq.) KNO3 + PbI2 Regular Chemistry

  5. Solubility Rules • Predict if a precipitate forms. • Page 574 • Back of Periodic Table • Pb(NO3)2(aq.) + 2 KI(aq.) 2 KNO3 + PbI2 Regular Chemistry

  6. Solubility Rules • Predict if a precipitate forms. • Page 574 • Back of Periodic Table • Pb(NO3)2(aq.) + 2 KI(aq.) 2 KNO3(aq.) + PbI2 Regular Chemistry

  7. Solubility Rules • Predict if a precipitate forms. • Page 574 • Back of Periodic Table • Pb(NO3)2(aq.) + 2 KI(aq.) 2 KNO3(aq.) + PbI2(s.) • Complete Ionic Equation • Pb2+(aq.) + 2 NO31-(aq.) + 2 K1+(aq.) + 2 I1-(aq.)  Regular Chemistry

  8. Solubility Rules • Predict if a precipitate forms. • Page 574 • Back of Periodic Table • Pb(NO3)2(aq.) + 2 KI(aq.) 2 KNO3(aq.) + PbI2(s.) • Complete Ionic Equation • Pb2+(aq.) + 2 NO31-(aq.) + 2 K1+(aq.) + 2 I1-(aq.)  2 K1+(aq.) + 2 NO31-(aq.) + PbI2(s.) • Spectator Ions Regular Chemistry

  9. Spectator Ions Regular Chemistry

  10. Solubility Rules • Predict if a precipitate forms. • Page 574 • Back of Periodic Table • Pb(NO3)2(aq.) + 2 KI(aq.) 2 KNO3(aq.) + PbI2(s.) • Complete Ionic Equation • Pb2+(aq.) + 2 NO31-(aq.) + 2 K1+(aq.) + 2 I1-(aq.)  2 K1+(aq.) + 2 NO31-(aq.) + PbI2(s.) • Spectator Ions • K1+, NO31- • Net Ionic Equation • Pb2+(aq.) + 2 I1-(aq.)  PbI2(s.) Regular Chemistry

  11. Solubility Rules • NH4Cl(aq.) + MgSO4(aq.) Regular Chemistry

  12. Solubility Rules • NH4Cl(aq.) + MgSO4(aq.) (NH4)2SO4 + MgCl2 Regular Chemistry

  13. Solubility Rules • 2 NH4Cl(aq.) + MgSO4(aq.) (NH4)2SO4 + MgCl2 Regular Chemistry

  14. Solubility Rules • 2 NH4Cl(aq.) + MgSO4(aq.) (NH4)2SO4(aq.) + MgCl2 Regular Chemistry

  15. Solubility Rules • 2 NH4Cl(aq.) + MgSO4(aq.) (NH4)2SO4(aq.) + MgCl2(aq.) • Complete Ionic Equation • 2 NH4+(aq.) + 2 Cl1-(aq.) + Mg2+(aq.) + SO42-(aq.)  2 NH4+(aq.) + SO42-(aq.) + Mg2+(aq.) + 2 Cl1-(aq.) • They are all spectator ions. • NO REACTION • Na3PO4(aq.) + SrBr2(aq.)  Regular Chemistry

  16. Solubility Rules • 2 NH4Cl(aq.) + MgSO4(aq.) (NH4)2SO4(aq.) + MgCl2(aq.) • Complete Ionic Equation • 2 NH4+(aq.) + 2 Cl1-(aq.) + Mg2+(aq.) + SO42-(aq.)  2 NH4+(aq.) + SO42-(aq.) + Mg2+(aq.) + 2 Cl1-(aq.) • They are all spectator ions. • NO REACTION • Na3PO4(aq.) + SrBr2(aq.)  NaBr + Sr3(PO4)2 Regular Chemistry

  17. Solubility Rules • 2 NH4Cl(aq.) + MgSO4(aq.) (NH4)2SO4(aq.) + MgCl2(aq.) • Complete Ionic Equation • 2 NH4+(aq.) + 2 Cl1-(aq.) + Mg2+(aq.) + SO42-(aq.)  2 NH4+(aq.) + SO42-(aq.) + Mg2+(aq.) + 2 Cl1-(aq.) • They are all spectator ions. • NO REACTION • 2 Na3PO4(aq.) + 3 SrBr2(aq.)  6 NaBr + Sr3(PO4)2 Regular Chemistry

  18. Solubility Rules • 2 NH4Cl(aq.) + MgSO4(aq.) (NH4)2SO4(aq.) + MgCl2(aq.) • Complete Ionic Equation • 2 NH4+(aq.) + 2 Cl1-(aq.) + Mg2+(aq.) + SO42-(aq.)  2 NH4+(aq.) + SO42-(aq.) + Mg2+(aq.) + 2 Cl1-(aq.) • They are all spectator ions. • NO REACTION • 2 Na3PO4(aq.) + 3 SrBr2(aq.)  6 NaBr(aq.) + Sr3(PO4)2(s.) • Spectator Ions: Regular Chemistry

  19. Solubility Rules • 2 NH4Cl(aq.) + MgSO4(aq.) (NH4)2SO4(aq.) + MgCl2(aq.) • Complete Ionic Equation • 2 NH4+(aq.) + 2 Cl1-(aq.) + Mg2+(aq.) + SO42-(aq.)  2 NH4+(aq.) + SO42-(aq.) + Mg2+(aq.) + 2 Cl1-(aq.) • They are all spectator ions. • NO REACTION • 2 Na3PO4(aq.) + 3 SrBr2(aq.)  6 NaBr(aq.) + Sr3(PO4)2(s.) • Spectator Ions: Na1+, Br1- • Net Ionic Equation: • 3 Sr2+(aq.) + 2 PO43-(aq.)  Sr3(PO4)2(s.) Regular Chemistry

  20. Summary • Predicting if a Precipitate is Formed • Ion Products • Heat a Solution, and Cool It to 25C • Solubility Rules (Page 574) • Complete Ionic Equations • Net-Ionic Equations • Spectator Ions Regular Chemistry

  21. Tonight's Assignment Regular Chemistry

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