2. POD
1)What is the pH of a M HCl solution? 2)What is the pOH of a M HCl solution? 3)What is the pH of a 6.50x 10-3M KOH solution? 4)A solution is created by measuring 3.60 x 10-3 moles of NaOH and 5.95 x 10-4moles of HCl into a container and then water is added until the final volume is 1.00 L. What is the pH of this solution? 5)What is the pH of a 6.2x 10-5M NaOH solution? 6) A solution with a H+ concentration of E-7M is said to be neutral. Why?

3. 1)What is the pH of a 0. 0235 M HCl solution. pH=1
1)What is the pH of a M HCl solution? pH=1.63 2)What is the pOH of a M HCl solution? pOH=12.4 3)What is the pH of a 6.50x 10-3M KOH solution? pH=13.0 4)A solution is created by measuring 3.60 x 10-3 moles of NaOH and 5.95 x 10-4moles of HCl into a container and then water is added until the final volume is 1.00 L. What is the pH of this solution? pH=2.52 5)What is the pH of a 6.2x 10-5M NaOH solution? pH=9.79 6)A solution with a H+ concentration of 1.00E-7 is said to be neutral. Why? Because pH=-log[H+] -log[H+] =-log[1.00E-7]=7

4. TEST ON MARCH 26 OR 30!?!?! SWBAT: Write balanced net ionic equations
Predict the products for reactions
Agenda
Net ionic equations
Writing equations
Solubility lab
TEST ON MARCH 26 OR 30!?!?!

5. Cuteness Overload

6. Reaction types
Synthesis – when two or more reactants combine to form a single product
A metal combines with a nonmetal to form a binary salt Li + N2  2Li3N
Metallic oxides and water form bases
Na2O + HOH  2NaOH
Nonmetallic oxides and water form acids
CO2 + H2O  H2CO3
Metallic oxides and nonmetallic oxides form salts
Na2O + CO2  Na2CO3

7. Reaction types
Decomposition – when a single reactant is broken down into two or more products (products can be elements OR another compound)
Metallic carbonates decompose into metallic oxides and carbon dioxide
MgCO3  MgO + CO2
Metallic chlorates decompose into metallic chloride and oxygen Mg(ClO3)2  MgCl2 + O2
Ammonium carbonate decomposes into ammonia, water, and carbon dioxide
(NH4)2CO3  2NH3 + H2O + CO2

8. Reaction types
Decomposition – when a single reactant is broken down into two or more products (products can be elements OR another compound)
Sulfurous acid decomposes into sulfur dioxide and water H2SO3  H2O + SO2
Carbonic acid decomposes into carbon dioxide and water H2CO3  H2O + CO2
A binary compound breaks down to produce 2 elements NaCl  2Na + Cl2

9. Reaction types
Decomposition – when a single reactant is broken down into two or more products (products can be elements OR another compound)
Hydrogen peroxide decomposes into water and oxygen H2O2  2H2O + O2
Ammonium hydroxide decomposes into ammonia and water NH4OH  NH3 + HOH

10. Reaction types
Single Replacement – an element replaces one part of a compound, an element can only replace another element that is less active than itself
Activity Series for metals
(most active) Li Ca Na Mg Al Zn Fe Pb H2 Cu Ag Pt Au (least active)
Activity Series for nonmetals
(most active) F2 Cl2 Br2 I2 (least active)

11. Reaction types
Single Replacement – an element replaces one part of a compound, an element can only replace another element that is less active than itself
Active metals replace less active metals from their compounds 3Mg + 2FeCl3  2Fe + 3MgCl2
Active metals replace hydrogen in water
2Na + 2HOH  H2 + 2NaOH
Active metals replace hydrogen in acids
2Li + 2HCl  H2 + 2LiCl

12. Reaction types
Single Replacement – an element replaces one part of a compound, an element can only replace another element that is less active than itself
Active nonmetals replace less active nonmetals from their compounds
Cl2 + 2KI  I2 + 2KCl
If a less reactive element is combined with a more reactive element in a compound, there will be no reaction
Cl2 + KF  no reaction
Zn + NaCl  no reaction

13. Chemical Eqns Handbook pg 46
A piece of copper is dropped into a container of water
Liquid bromine is added to a container of sodium iodide crystals
An aluminum strip is immersed in a solution of silver nitrate
Zinc pellets are added to a sulfuric acid solution
Fluorine gas is bubbled into a solution of aluminum chloride

14. Reaction types
Double Replacement (metathesis) – two compounds react to form two new compounds (both reactants switch partners), all double replacement reactions MUST have a driving force
Driving forces:
Formation of a precipitate (insoluble compound)
Formation of a gas
Formation of a molecular species (a covalent compound such as water)

15. Predict & Balance the following metathesis rxns (hint: some do not go to completion) Chemical Equations Handbook pg 51
Silver nitrate + potassium chromate
Ammonium chloride + cobalt (II) sulfate
iron (III) sulfate + barium iodide
Zinc acetate + cesium hydroxide
Ammonium sulfide + lead(II) nitrate
Lithium hydroxide + sodium chromate

16. Ultimate Chemical Equations Handbook
Blue or Green pgs 41, 43, 46, 51 DUE Friday March 20