1. Aqueous Reactions and Solution Stoichiometry
Mr. Kinton
Honors Chemistry

2. Ionic Equations Complete Net Ionic
Show all of the ions present in a chemical reaction
Anything that is aqueous can be written as an ion
Allows us to identify the driving force within a reaction
Shows only the ions responsible for the reaction
Will have 2 ions and either a (s), (l), or (g) product
Spectator ions: Ions that do not participate in the reaction

3. Example

4. Example
Write the complete ionic and net ionic equations for each of the following reactions:
3 (NH4)2CO3 (aq) + 2 Al(NO3)3 (aq) --> 6 NH4NO3 (aq) + Al2(CO3)3 (s)

5. Answer
Complete Ionic Equation: 6 NH4+ (aq) + 3 CO32- (aq) + 2 Al3+ (aq) + 6 NO3- (aq)  6 NH4+ (aq) + 6 NO3- (aq) + Al2(CO3)3 (s) Net Ionic Equation: 2 Al3+ (aq) + 3 CO32- (aq)  Al2(CO3)3 (s)

6. Driving Forces Formation of a gas or precipitate
Formation of a weak or nonelectrolyte
Transfer of electrons during the reaction

7. Metathesis Reactions
Reaction where positive and negative ions appear to change partners
Precipitation reactions generally follow this pattern as well
Examples- Pb(NO3)2(aq) + KI(aq)

8. Oxidation-Reduction Reactions
Reaction where electrons are transferred between reactants
Mainly in the form of single replacement reactions where a metal replaces another.
Example- Aluminum with hydrobromic acid

9. Acid Base Reactions
Neutralization reactions lead to the formation of a salt and water (weak or nonelectrolyte formed)
With bases that do not contain hydroxide, gases are formed

10. Acids Substances that ionize to produce hydrogen ions (Arrhenius)
Called proton donors (Bronsted-Lowry)
Can also be an electron-pair acceptor (Lewis)
Can donate many hydrogens depending on the acid
Sour taste
Turn litmus paper red
Forms hydronium ion

11. Strength of Acids Strong Weak
Only 7: HCl, HBr, HI, HClO3, HClO4, HNO3, and H2SO4
Strong electrolytes
Every other acid is a weak acid
Weak electrolytes
Strong
Weak

12. Bases Form hydroxide ions in solution (Arrhenius)
Proton acceptor (Bronsted-Lowry)
Electron pair donor (Lewis)
Bitter taste
Slippery feel
Turn litmus paper blue
Accept hydrogen ions

13. Strength of Bases Strong Weak Every other base is weak
Weak electrolytes
Only 8 Strong Bases: alkali and the bottom of the alkaline earth metal hydroxides
Strong electrolytes
Strong
Weak

14. Autoionization of Water
Water has the ability to act as an acid or base
Occurs at chemical equilibrium
Kw= [H+][OH-] = 1.0 x at 25o C

15. pH Scale Molar concentration of H+ -log[H+] Acids: pH< 7.00
Bases: pH> 7.00
Neutral: pH =7.00

16. Calculate the pH of lemon juice, which has a concentration of [H+] of 3.8 x 10-4
Sig figs: based on the number of places after the decimal
Calculating pH

17. Solution Stoichiometry
We typically want to determine the number of moles of a substance
Also useful in determining acid-base neutralizations

18. Examples
How many grams of chloride ion are in a sample of water if 20.2 mL of .100 M Ag+ is needed to react with all the chloride?
45.7 mL of .500 M H2SO4 is required to neutralize a mL sample of NaOH solution. What is the NaOH concentration?

19. Titrations
Practical application for how to determine the concentration of a particular solute
Combining a sample of known concentration (standard solution)
Equivalence point: where the values are equivalent
Indicator: used to determine the equivalence point
Methyl Red- pH range of
Phenonlpthlaein- pH range of 8.3 to 10.0

20. Examples
How many grams of Ca(OH)2 are needed to neutralize mL of .100 M HNO3?
How many liters of .500 M HCl are needed to completely react with .100 mol of Pb(NO3)2?