1. Aqueous Reactions and Solution Stoichiometry
Chapter 4
Aqueous Reactions and Solution Stoichiometry

2. General Properties of Aqueous Solutions

3. Ionic Compounds in Water

4. Molecular Compounds in Water

5. Strong and Weak Electrolytes
Simulation
Electrolyte activity

6. Precipitation Reactions

7. Solubility Guidelines

8. Double Displacement (Exchange) Reactions

9. Ionic Equations

10. Acid-Base Reactions
Acids and Bases are also common electrolytes, which dissociate in water (soluble/separate)
Acids are substances that ionize in aqueous solutions to form hydrogen ions (H+) thereby increasing the concentration of H+(aq) ions.
Because hydrogen atoms consist of only one proton and one electron, is H+ simply one proton. Thus acids are often called proton donors.
Just like the ionic compounds we have been studying, water also causes the H+(aq) ion to separate from its other half.
Molecules of different acids can ionize to form different numbers of H+(aq) ions. Both HCl and HNO3 are monoprotic acids yeilding only one H+(aq) ion. H2SO4, however, is a diprotic acid that yields two H+(aq) ions. This occurs to two steps however.

11. Acid-Base Reactions cont.
Bases are substances that accept (react with) H+(aq) ions. Bases produce hydroxide ions (OH-) when they dissolve in water. Ionic hydroxide compounds such as NaOH, KOH, and Ca(OH)2 are among the most common bases, separating just as the ions we have been studying separate.
Compounds that do not contain OH- ions can also be bases. For example, ammonia is a common base that when added to water, it accepts an H+ from the water and thereby produces an OH- ion.

12. Strong and Weak Acids and Bases
Acid and bases that completely dissociate in solution (strong electrolytes) are strong acids and bases. (pg 130 in AP Text)
Those that only partially dissociate in solution (weak electrolytes) are weak acid and bases.
Not only strong acids are highly reactive though…
So strong electrolytes include all soluble ionic compounds and strong acids. Weak electrolytes include weak acids and bases.

13. Neutralization Reactions and Salts
When a solution of a strong acid and strong base are mixed a neutralization reaction occurs because the H+ the acid combines with the OH- from the base to make water and a salt (ionic compound whose anion comes from an acid and whose cation comes from an base.
HCl + NaOH H2O + NaCl
Video simulation
Also have net ionic equations…
Sample Exercise 4.7 pg 133

14. Acid-Base Reactions with Gas Formation
Many bases beside OH- react with H+ to for molecular compounds such as the sulfide ion and the carbonate ion. Both of these ions reaction with acids to form gases. See page 134 for net ionic equations.
Net Ionic Equation

15. Oxidation-Reduction Reactions
Reactions in which electrons are transferred between reactants-redox reactions
Most are Single Displacement reactions.
When an atom, ion or molecule has become more positively charged by losing electrons it is oxidized (oxidation). LEO
When an atom, ion or molecule has become more negatively charged by gaining electrons, it is reduced (reduction). GER
The oxidation of one substance is always accompanied by the reduction of another substance. As electrons are transferred between them.
Calcium Water Demo on each table

16. Oxidation Numbers
We need a system to keep track of whether electrons are lost or gained by a substance to determine if a redox reaction has taken place.

17. Oxidation of Metals by Acids and Salts

18. Activity Series of Metals

19. Concentrations of Solutions

20. Converting between Molarity, Moles and Volume

21. Dilutions

22. Solution Stoichiometry

23. Titrations