1. Reaction in Aqueous Solution
Chapter 4

2. Precipitation reactions
Form a solid---precipitate!
Remember:
Solubility Rules
Found on page 91 figure 4.2
Or on the web
Or you saved them from last year
Yep ya gotta know em

3. Are the following soluble or insoluble?
BaCl2
soluble
Mg(OH)2
insoluble
Cr2(CO3)3
K3PO4
All Chloride are soluble except Ag+Hg2+Pb2+
All hydroxides are insoluble except Ca2+ Sr2+ Ba 2+
All carbonates are insoluble except group I and NH4+
All group I elements are soluble!

4. Net ionic equations Ba(NO3)2 + Na2CO3

5. BaCl2 + NaOH
All aqueous—no precipitate—no rxn!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!

6. When sodium hydroxide and copper (II) sulfate react a with precipitate is formed. What volume of M NaOH solution is required to produce g of precipitate? Net ionic equation?

7. = L NaOH

8. Acid-base reactions Acids Bases Produce H+ in water Strong acids
Completely dissociate in water
HCl
HBr HI
H2SO4
HClO4
HClO3
HNO3
Bases
Produce OH- in water
Strong bases
Completely dissociate in water
Group I metals
Heavier group II metals

9. Strong acid-strong base -neutralization

10. Weak acid-strong base

11. Strong acid-weak base

12. Acid –base titrations
Used to determine an unknown concentration of either the acid or the base
The concentration of the other solution is known and so is the volume of both solutions
Equivalence point
The point at which the reaction is complete
Moles of acid = moles of base

13. What volume of 0. 10 M NaOH is required to completely neutralize 250
What volume of 0.10 M NaOH is required to completely neutralize mL of 0.30 M HCl?
= 0.75 L NaOH

14. If 25. 0mL of 0. 500 M NaOH is required to react with 15
If 25.0mL of M NaOH is required to react with 15.0 mL HCl what is the molarity of HCl ?

15. Oxidation-reduction reactions
Redox
Oxidation-loss of electrons
Oxidation number increases
Reduction-gain of electrons
Oxidation number decreases
Oxidizing agent
The element that undergoes reduction
Reducing agent
The element that undergoes oxidation

16. Balancing Balance the atoms Break the equation into two half reaction
Oxidation
Reduction
Balance O’s with H20
Balance H’s with H+
Balance the charge with electrons
If confused do not use the book’s method!

17. Balance using half reactions
Oxidizing agent
Use pen as pointer to assign oxidation numbers
Reducing agent

19. In a basic solution
Balance all redox in acidic solution unless stated

20. Balance in a basic solution
Oxidizing agent
Use pointer pen to assign ox numbers
Reducing agent

22. 10 OH- +
+ 10 OH-
= 10 H2O
=8 H2O

24. What volume of M KMnO4 solution is required to completely react with mL of M Fe(NO3)2