1. Catalyst – December Prime # between 13 and 19, 2009  Label the letters on the graph with the following:  Solid  Liquid  Gas  What is happening at letter “d”?  Define the following.  Condensation  Melting  What color does litmus paper turn when exposed to an acid? - 20° 0° 20° 40° 60° 80° 100 ° 120 ° Changes in the State of Water Energy (Heat) Added a b c d e

2. Today’s Agenda  HW Review  Review Acid-Base and stoich  Individual Work Time  Exit Question

3. Today’s Objectives  SWBAT master Acid base chemistry  SWBAT master stoichiometry.

4. pH Scale Key Point: pH is a scale used to identify acids, bases, and neutral solutions. It ranges from 1-14.  Acids have a pH less than 7  Bases have a pH more than 7

5. Acids and Bases  If I have solution with a LOT of Hydrogen ions (H + ), will it be an acid or a base???  Acid of course!!!  The more [H + ] ions we have the more acidic something is.  What about if we have a LOT of Hydroxide (OH - ) ions?  Base of course!!!!  The more [OH - ] ions we have, the more basic something is.

6. pH Math Review  To calculate pH:  Find the equation where the thing that you are looking for is BY ITSELF and the thing that you have is in the equation! EQUATIONS! pH= -log [H + ] [H+] = 10 -pH pOH= -log [OH - ] [OH - ]= 10 -pOH pH+pOH=14

7. Your turn  What’s the pH of a solution that has 4.1 * 10 -3 M [H + ]? EQUATIONS! pH= -log [H + ] [H+] = 10 -pH pOH= -log [OH - ] [OH - ]= 10 -pOH pH+pOH=14

8. Let’s practice  What is the [H + ] of a solution that has a pH of 9? EQUATIONS! pH= -log [H + ] [H+] = 10 -pH pOH= -log [OH - ] [OH - ]= 10 -pOH pH+pOH=14

9. Tricksters…  What’s the pH of a solution that has an [OH - ] of 1.5 * 10 -3 M? EQUATIONS! pH= -log [H + ] [H+] = 10 -pH pOH= -log [OH - ] [OH - ]= 10 -pOH pH+pOH=14

10. Neutralization!  KEY POINT #1: A neutralization reaction is a double-replacement reaction in which an acid and a base react in to produce water and a salt  A salt is an ionic compound made up of a cation from a base and an anion from an acid  Acid + Base  Water + Salt  HY + X(OH)  H 2 O + XY DON’T FORGET TO KRISS-KROSS!!!! ACIDBASESALTWATER

11. Example…  Example: Write the equation for the neutralization of hydrochloric acid (stomach acid) with an antacid (Aluminum Hydroxide)  HCl + Al(OH) 3 → AlCl 3 + H 2 O What reaction type is this? Water will ALWAYS be a product….

12. Stoichiometry Key Point #2: There are 3 steps to solving stoichiometric problems involving chemical reactions: 1) Balance the equation 2) Figure out what to what 3) Convert using train tracks And remember…

13. IIF YOU ARE CHANGING COMPOUNDS, YOU MUST USE A MOL-MOL CONVERSION FACTOR!

14. Your Turn! Mole to Mole! Balanced Equation: Coefficents = Moles __Co + __ F 2  __CoF 3 How many moles are CoF 3 are produced when 1.25 moles of Co reacts?

15. Can you step it up?? Mole to Mass Balanced Equation: Coefficents = Moles __ KCl + __ O 2  __ KClO 3 How many moles of KClO 3 will form if we start with 64 grams of O 2 ?

16. Practice, Practice, Practice … Did I mention practice? Balanced Equation: Coefficents = Moles __ Cu + __ AgNO 3  __ Cu(NO 3 ) 2 + __ Ag How many grams of Ag would form if we react 8 grams AgNO 3 ?

17. Showdown… ___N 2 + ___H 2  ___ NH 3  How many grams of NH 3 are produced when N 2 reacts with 10.0 mol H 2 ?

18. Balancing Equations Practice! TIME TO DOMINATE THE PRACTICE WORKSHEET!

19. SHOWDOWN PART 2!! Balanced Equation: Coefficents = Moles __ N 2 + __ H 2  __ NH 3 How many grams of NH 3 would be produced if 56 grams of N 2 are reacted?