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11.3 REACTIONS IN AQUEOUS SOLUTIONS

11.3 REACTIONS IN AQUEOUS SOLUTIONS. Earth’s surface is 70% water…. We are made mostly of water. Here is a REAL-LIFE, very important example of an aqueous reaction occurring inside you even as we speak. ______________________________________________________________________.

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11.3 REACTIONS IN AQUEOUS SOLUTIONS

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  1. 11.3REACTIONS INAQUEOUS SOLUTIONS

  2. Earth’s surface is 70% water….

  3. We are made mostly of water

  4. Here is a REAL-LIFE, very important exampleof 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 inwhich _____________________________

  7. Remember the demo - Spirit Day precipitate___ KI ( ) + ___ Pb(NO3)2 ( )→ 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. “Soda straws” in a cave

  9. SOLUBILITY CHART – mostly soluble

  10. SOLUBILITY CHART – mostly insoluble

  11. You don’t have to memorize these charts, butYOU 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 insolubleEXAMPLES 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(NO3)2 (aq) → 2 KNO3 (aq) + __ PbI2 (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(NO3)2 (aq) → 2 KNO3 (aq) + __ PbI2 (s)2K1+ (aq) + 2I1-(aq) →PbI2 (s)RULE #3: When writing aqueous compounds as dissociated, the only subscripts that remain the same are those in ______________________________. The others become ____________________

  16. NOW IT’S YOUR TURN!For the 2 reactants below, write the1) complete, balanced chemical equation.2) complete ionic equation. copper (II) sulfate + sodium phosphate

  17. Net ionic equations show you_______________________________________

  18. 2 KI (aq) + __ Pb(NO3)2 (aq) → 2K1+ (aq) + 2K1+ (aq) + Pb2+ (aq) + 2NO31- (aq) → 2 KNO3 (aq) + __ PbI2 (s) 2K1+ (aq) + 2NO31- (aq) + PbI2 (s)

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

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

  21. Now - try the equation you did before.3Cu2+ (aq) + 3SO42- (aq) + 6Na1+ (aq) + 2PO43- (aq) → 6Na1+ (aq) + 3SO42- (aq) + Cu3(PO4)2 (s)The DRIVING FORCE for this reaction was also the formation of a _____________________

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

  23. Unless told otherwise – assume an acid is_________________ and water is a _________________HCl( ) + NaOH( ) → NaCl( ) + HOH ( )

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

  25. __Al ( ) + __HCl( ) →

  26. Three potential DRIVING FORCES for chemical reactions are:the formation of_______________________________________________________________________________________

  27. The driving force for this reaction was theformation of a _____________

  28. NOW IT’S YOUR TURN; try these. ALL EQUATIONS MUST INCLUDE PHYSICAL STATESWrite the:1. complete, balanced chemical equation,2. complete ionic equation.3. net ionic equation4. driving force1. ___HNO3( ) + ___Ca(OH)2( )→

  29. Write the:1. complete, balanced chemical equation,2. complete ionic equation.3. net ionic equation4. driving force2. ___(NH4)2CO3( ) + ___SnBr2( )→

  30. Write the:1. complete, balanced chemical equation,2. complete ionic equation.3. net ionic equation4. driving force3. ___ H3PO4( ) + ___ Mg ( )→

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