1. 11.3 REACTIONS IN AQUEOUS SOLUTIONS

2. Earth’s surface is 70% water….

3. We are made mostly of water

4. Here is a REAL-LIFE, very important example of an aqueous reaction occurring inside you even as we speak

5. ______________________________________________________________________

6. REMINDER: An aqueous physical state - (aq) means ___________________________________ An aqueous solution is a solution in which _____________________________

7. Remember the demo - Spirit Day precipitate ___ KI ( ) + ___ Pb(NO 3 ) 2 ( )→ Spirit Day precipitate A precipitate is a ________________so this means that the yellow precipitate is__________________ in water!

8. Not all ionic compounds are soluble in water. If a reaction is done in water… Under normal conditions, an ionic compound will ALWAYS SOMETIMES NEVER be a liquid or gas. WATER- SOLUBLE? PHYSICAL STATE IS…. YES (aq) NO (s) “Soda straws” in a cave

9. SOLUBLE COMPOUNDS Compounds containing IMPORTANT EXCEPTIONS nitratenone chloridesalts of silver, mercury, lead bromidesalts of silver, mercury, lead iodidesalts of silver, mercury, lead sulfatesalts of calcium, strontium, barium, mercury, lead SOLUBILITY CHART – mostly soluble

10. SOLUBILITY CHART – mostly insoluble INSOLUBLE COMPOUNDS Compounds containing IMPORTANT EXCEPTIONS sulfidesalts of ammonium, alkali metals, calcium, strontium, barium carbonatesalts of ammonium, alkali metals, phosphatesalts of ammonium, alkali metals, hydroxidecompounds of alkali metals, calcium, strontium, barium

11. You don’t have to memorize these charts, but YOU SHOULD REMEMBER THESE PATTERNS…. ALL COMMON SALTS WITH _____________________________________ and/or ________________________________________ ARE SOLUBLE. ALL COMMON COMPOUNDS of_________________ ARE SOLUBLE EXCEPT FOR _____________________

12. Determine whether these compounds are soluble or insoluble EXAMPLES write (s) or (aq) a. platinum nitrate ___ b. barium sulfide ___ c. magnesium chloride ___ d. Ammonium carbonate ___ _______________________________________________________________ NOW – YOU TRY IT! 1. iron (II) iodide ___2. aluminum phosphate ___ 3. aluminum sulfate ___4. ammonium carbonate ___ 5. barium sulfate ___6. barium sulfide ___ 7. silver nitrate ___8. mercury (I) chloride ___ 9. calcium hydroxide ___10. copper (I) phosphate ___

13. COMPLETE IONIC EQUATIONS _______________________________________ ______________________________________ RULE #1: Solids (s), liquids (l), and gases (g), ___________________________________________ ___________________________________________

14. 2 KI (aq) + __ Pb(NO 3 ) 2 (aq) → 2 KNO 3 (aq) + __ PbI 2 (s) RULE #2: Assume that all soluble aqueous compounds ______________________________________________________ (Actually – not all do – but save that for another year.) ___ NaCl (aq) → __KI (aq) →

15. 2 KI (aq) + __ Pb(NO 3 ) 2 (aq) → 2 KNO 3 (aq) + __ PbI 2 (s) 2K 1+ (aq) + 2I 1- (aq) → PbI 2 (s) RULE #3: When writing aqueous compounds as dissociated, the only subscripts that remain the same are those in _____________ _________________. The others become ____________________

17. NOW IT’S YOUR TURN! For the 2 reactants below, write the 1) complete, balanced chemical equation. 2) complete ionic equation. copper (II) sulfate + sodium phosphate

18. Net ionic equations show you _______________________________________

19. 2 KI (aq) + __ Pb(NO 3 ) 2 (aq) → 2K 1+ (aq) + 2K 1+ (aq) + Pb 2+ (aq) + 2NO 3 1- (aq) → 2 KNO 3 (aq) + __ PbI 2 (s) 2K 1+ (aq) + 2NO 3 1- (aq) + PbI 2 (s)

20. Ions that are unchanged during a chemical reaction are called…..

21. The DRIVING FORCE for this reaction (i.e., what made a chemical reaction occur) was the formation of a _____________________

22. Now - try the equation you did before. 3Cu 2+ (aq) + 3SO 4 2- (aq) + 6Na 1+ (aq) + 2PO 4 3- (aq) → 6Na 1+ (aq) + 3SO 4 2- (aq) + Cu 3 (PO 4 ) 2 (s) The DRIVING FORCE for this reaction was also the formation of a _____________________

23. The driving force isn’t always the formation of a precipitate… Below is an acid- base reaction you will do later – using the equipment shown here. HCl + NaOH → NaCl + HOH

24. Unless told otherwise – assume an acid is _________________ and water is a _________________ HCl ( ) + NaOH ( ) → NaCl ( ) + HOH ( )

25. The driving force for an acid-base reaction* is the formation of ___________. *For the type of acid-base reactions we’ll do this year.

26. __Al ( ) + __HCl ( ) →

27. Three potential DRIVING FORCES for chemical reactions are: the formation of ____________________________ _____________________________ ______________________________

28. The driving force for this reaction was the formation of a _____________

29. NOW IT’S YOUR TURN; try these. ALL EQUATIONS MUST INCLUDE PHYSICAL STATES Write the: 1. complete, balanced chemical equation, 2. complete ionic equation. 3. net ionic equation 4. driving force 1. ___HNO 3 ( ) + ___Ca(OH) 2 ( )→

30. Write the: 1. complete, balanced chemical equation, 2. complete ionic equation. 3. net ionic equation 4. driving force 2. ___(NH 4 ) 2 CO 3 ( ) + ___SnBr 2 ( )→

31. Write the: 1. complete, balanced chemical equation, 2. complete ionic equation. 3. net ionic equation 4. driving force 3. ___ H 3 PO 4 ( ) + ___ Mg ( )→