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Assignment #71 Precipitates

Assignment #71 Precipitates. Predicting Precipitation. Ion Product Q for Dissolution Problems 9.0x10 -7 g 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 > K sp Shift to the Left.

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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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