(©2007, François G. Amar, All rights reserved)

Summary for Weeks 5&6

Exam: Wednesday, October 3

Reading:

For these weeks: Chapter 4.1 to 4.6 in BLB

A look ahead to Week 7: Chapter 5

Homework problems:

Beginning of Chapter 4: 5, 7, 9, 14, 16, 20, 23, 25, 28

End of Chapter 4: 31,33, 35, 39, 40, 41, 43, 45, 50, 51, 53, 55, 56, 67, 70, 80, 83

OWL Assignment for Week 5&6:

Chapter 4 assignment (called Ch 5 in OWL) on ions in solution, molarity: due October 14, 2007

Key concepts:

solution composition and concentration

molarity, [Na⁺]

ionic and molecular compounds in aqueous solution

acids, bases, and salts

strong acids and bases

weak acids and bases

Working with acids and bases

equilibrium concept

neutralization reactions

ionic equations & net ionic equations

metathesis reactions

precipitation reactions

solubility rules

gas forming reactions

oxidation and reduction reactions always occur together

activity series for oxidation of metals

solution stoichiometry

quantitative calculations with molarity

titration

equivalence point

indicators

Key equations:

M = [ ] =(moles solute)/(L solution) molarity

M_iV_i = M_fV_f dilution equation

MX (aq) is same as M+ (aq) + X- (aq) if strong electrolyte

example: NaCl (aq) ---> Na⁺ (aq) + Cl^- (aq)

but

MX M⁺ (aq) + X^- (aq) equilibrium for weak electrolyte

example: H₃C-COOH (aq) H₃C-COO^- (aq) + H⁺ (aq)

acid + base ---> a salt and water

AX + BY ---> AY + BX metathesis or "change your partner"

precipitation may occur

M ---> M⁺ + e^- oxidation half reaction

example: Na ---> Na⁺ + e^-

 

X + e^- ---> X- reduction half reaction

example: O + 2 e^- ---> O^2-

 

Molarity (analyte) = Molarity (titrant) x Volume(titrant)/Volume(analyte)  

 (titration equation careful in applying this to diprotic acids etc)