1. Basic Principles of Chemistry Unit 2: Chemical Reactions and Their Significance Lecture #11

2. Precipitation Reactions A solid substance is formed in a solution where there was not solid previously

3. Solutions SOLUTE dissolves in SOLVENT to form SOLUTION Solute is SOLUBLE in solvent

4. How Substances Dissolve

5. Solubility Rules (p. 200)

7. Predicting Precipitations AgNO 3 (aq) + NaCl(aq)  AgCl(?) + NaNO 3 (?)

8. Predicting Precipitations AgNO 3 (aq) + NaCl(aq)  AgCl(?) + NaNO 3 (aq)

9. Predicting Precipitations AgNO 3 (aq) + NaCl(aq)  AgCl(s) + NaNO 3 (aq)

10. Molecular Equation AgNO 3 (aq) + NaCl(aq)  AgCl(s) + NaNO 3 (aq)

11. Total Ionic Equation Ag + (aq) + NO 3 - (aq) + Na + (aq) + Cl - (aq)  AgCl(s) + Na + (aq) + NO 3 - (aq)

12. Total Ionic Equation Ag + (aq) + NO 3 - (aq) + Na + (aq) + Cl - (aq)  AgCl(s) + Na + (aq) + NO 3 - (aq)

13. Total Ionic Equation Ag + (aq) + NO 3 - (aq) + Na + (aq) + Cl - (aq)  AgCl(s) + Na + (aq) + NO 3 - (aq)

14. Net Ionic Equation Ag + (aq) + Cl - (aq)  AgCl(s)

15. Inconvenient Precipitates

16. Acid-Base Neutralization HCl(aq) + NaOH(aq)  H 2 O(l) + NaCl Acid + base  water + salt

17. Acid-Base Neutralization HC 2 H 3 O 2 (aq) + NaHCO 3 (aq)  H 2 O(l) + NaC 2 H 3 O 2 (aq) + CO 2 (g)

18. Net Ionic Equation H + (aq) + OH - (aq)  H 2 O(l)

19. TUMS HCl(aq) + CaCO 3 (aq)  H 2 O(l) + CaCl 2 (aq) + CO 2 (g)

20. Tooth Decay HC 3 H 5 O 4 (aq) + Ca 5 (PO 4 ) 3 OH(s)  H 2 O(l) + Ca 5 (PO 4 ) 3 C 3 H 5 O 4 (aq)

21. Dissolving Scale CaCO 3 (s) + 2HCl(aq)  CaCl 2 + H 2 O(l) + CO 2 (g)

22. Oxidation-Reduction Al(s) + 6HCl(aq)  2AlCl 3 (aq) + 3H 2 (g)

23. Combustion 2H 2 (g) + O 2 (g)  2H 2 O(g)

24. General Categories Type of ReactionGeneric Equation combination reactionA + B  AB decomposition reactionAB  A + B single displacement reaction A + BC  AC + B double displacement reaction AB + CD  AD + CB