CHEMISTRY 161 Revision Chapters 4-6 chem.hawaii/Bil301/welcome.html
CHEMISTRY 161 Chapter 4
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Transcript of CHEMISTRY 161 Chapter 4
CHEMISTRY 161
Chapter 4
REVISION
1. solution, solvent, and solute
2. experimental definition of strong/weak/non-electrolyte
3. dissociation and hydration of solute in solvent
(solutions conduct electricity)
4. precipitation reaction
(molecular equation, ionic equation, spectator ions)
CHEMICAL REACTIONS
1.properties of solutions
2. reactions in solutions
a) precipitation reactions
b) acid-base reactions (proton transfer)
c)redox reactions (electron transfer)
2.2. ACIDS AND BASES
Arrhenius (1883)
ACIDS
BASES
NaOH (s) → Na+ (aq) + OH- (aq)
MOH → M+ (aq) + OH- (aq)
HCl (g) → H+ (aq) + Cl- (aq)
HAc → H+ (aq) + Ac- (aq)
ACIDS
1. acids have a sour taste
vinegar – acetic acidlemons – citric acid
2. acids react with some metals to form hydrogen
2 HCl(aq) + Mg(s) → MgCl2(aq) + H2(g)
3. acids react with carbonates to water and carbon dioxide
2 HCl(aq) + CaCO3(s) → CaCl2(aq) + [H2CO3]H2CO3 → H2O(l) + CO2(g)
BASES
1. bases have a bitter taste
2. bases feel slippery
soap
3. aqueous bases and acids conduct electricity
Bronsted (1932)
ACIDS
HAc → H+ (aq) + Ac- (aq)
proton donors
BASES
proton acceptor
B + H+ (aq) → BH+ (aq)
H+ ≈ 10-15 m
Na+ ≈ 10-10 m
(aq) (l) (aq) (aq)
hydronium ion
acid base
cation hydronium ion
weak electrolyte
CH3COOH(aq) + H2O(l) H3O+(aq) + CH3COO-(aq)
NH3(aq) + H2O(l) NH4+ + OH-
strong electrolyte
HCl(aq) + H2O(l) → H3O+(aq) + Cl-(aq)
HNO3(aq) + H2O(l) → H3O+(aq) + NO3-(aq)
monoprotic acids
CH3COOH(aq) + H2O(l) H3O+(aq) + CH3COO-(aq)
NH3(aq) + H2O(l) NH4+(aq)+ OH-(aq)
H2O(l) + H2O(l) H3O+(aq) + OH-(aq)
water can be either an acid or a base
monoprotic acids
diprotic acid
HF, HCl, HBr, HNO3, CH3COOH
H2SO4 → H+(aq) + HSO4-(aq)
HSO4-(aq) H+(aq) + SO4
2-(aq)
triprotic acid
H3PO4 H+(aq) + H2PO4-(aq)
H2PO4-(aq) H+(aq) + HPO4
2-(aq)
HPO42-(aq) H+(aq) + PO4
3-(aq)
Acids in the Solar System
Venus
H2SO4(g)
Europa
H2SO4(s)
Acids in the Interstellar Medium
Orion
NH3, H2O, H2S
CH3COOH
HCOOH
HF, HCl
ACID-BASE REACTION
acid + base → salt + water
(neutralization reaction)
HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
molecular equation – ionic equation – spectator ions
SUMMARY
1.acids and bases
1.1. Arrhenius and Bronsted
1.2. strong and weak acids and bases
1.3 acids in extraterrestrial environments
2. acid-base neutralization reactions
Homework
Chapter 4, p. 111-116problems