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Drill – 4/14/11

Drill – 4/14/11. REVIEW! Write the following: Ionic charge of Calcium and Phosphate Ionic formula for Calcium Phosphate Balanced chemical equation for the reaction between Calcium Phosphate and Ammonium Oxide. Drill – 4/15/11. What is a precipitate?

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Drill – 4/14/11

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  1. Drill – 4/14/11 REVIEW! Write the following: • Ionic charge of Calcium and Phosphate • Ionic formula for Calcium Phosphate • Balanced chemical equation for the reaction between Calcium Phosphate and Ammonium Oxide

  2. Drill – 4/15/11 • What is a precipitate? • Does a precipitate separate into its ions?

  3. Drill – 4/26/11 • Balance and Write the complete and net ionic equation for the following unbalanced chemical equation: CaCl2(aq) + Na3PO4(aq)NaCl(aq) + Ca3(PO4)2(s)

  4. Ions in Aqueous SolutionChapter 13, Section 1

  5. Dissociation • The separation of ions that occurs when an ionic compound dissolves. • NaCl (s)  Na+ (aq) + Cl- (aq) • CaCl2 (s)  Ca+2 (aq) + 2Cl- (aq) H2O Notice: ions cannot be diatomic H2O

  6. H2O • NaCl (s)  Na+ (aq) + Cl- (aq) • 1 mol 1 mol 1 mol • CaCl2 (s)  Ca+2 (aq) + 2Cl- (aq) • 1 mol 1 mol 2 mol • Al2(SO4)3 (s)  2Al3+ (aq) + 3SO42- (aq) • 1 mol 2 mol 3 mol H2O H2O

  7. How many solute ions in each case?

  8. Complete Ionic Equations • Shows all the ions that are present in an aqueous solution.

  9. How to write complete ionic equations 1. Write the balanced chemical equation. 2. Include the state of matter, making sure to identify precipitates. 3. Dissociate chemical equations for all aqueous (aq) compounds to ions (do not dissociate precipitates). 4. Make sure to keep the equation balanced!

  10. Net Ionic Equations • Include only those compounds and ions that undergo a chemical change in a reaction in aqueous solution.

  11. How to write net ionic equations 1. Write the complete ionic equation. 2. Cancel spectator ions from both sides of the equation. Spectator ions do not take part in the chemical reaction and are found in solution both before and after the reaction.

  12. CdSO4 and H2S • CdSO4 + H2S  CdS + H2SO4 • CdSO4 (aq) + H2S (aq)  CdS (s) + H2SO4 (aq) • Cd2+(aq) + SO42-(aq) + 2H+(aq) + S2-(aq)  CdS(s) + SO42-(aq) + 2H+(aq) • Cd2+(aq) + S2-(aq)  CdS(s)

  13. Practice Problem Write the complete and net ionic equations for the reaction between aqueous ammonium carbonate and aqueous calcium chloride. (calcium carbonate is a precipitate)

  14. Complete: 2NH4+(aq) + CO32- (aq) + Ca+2 (aq) + 2Cl-(aq)  CaCO3 (s) + 2NH4+(aq) + 2Cl- (aq) Net: Ca+2 (aq) + CO32-(aq)  CaCO3 (s)

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