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Topic 8 and 18 - Acids and Bases (8.3 The pH Scale (pH is inversely…
Topic 8 and 18 - Acids and Bases
8.1 - Theories of Acids and Bases
Definitions of Acids and Bases
Arrhenius
Acids produce H+ ions
Bases produce OH - ions
Bronsted-Lowry
Bases are proton acceptors
Acids are proton donors
Lewis
Acids are electron pair acceptors
Bases are electron pair donars
Conjugate Acids and Bases
Amphiprotic
Can act either as proton donors or proton acceptors
Amphoteric
Can act either as an acid or base
8.2 Properties of acids and Bases
ACIDS
tart / sour taste
Aqueous solutions are electrolytes
Dissolves in water to produce hydrogen ions
Naming Acids
Anion ends in
-ide
= hydro(stem)-ic acid eg. hydrochloric acid
Anions ends in
-ite
= (stem)-ous acid eg. sulfurous acid
Anion ends in
-ate
= (stem)-is acid. eg. nitric acid
BASES
Bitter taste, feel slippery
Alkalis - Dissolve in water to produce hydroxide ions
All alkalis are bases, not all bases produce OH- ions so not all are alkalis
Naming bases - follow ionic compound naming rules
Reactions
Acid + Base ------> Salt + Water
Neutralization reaction
Neutralization
reactions determine exact conc of acid or base
Equivalence point - where acid and base exactly neutralize
End point - where indicator changes colour
Exothermic
You can backtrack from a salt to find which acid and base where reacted together. Add H+ to anion and OH- to cation.
Acid + Metal ------> Salt + Hydrogen
Acid + Metal oxide ------> Salt + Water
Acid + Carbonate ------> Salt + Water + Carbon dioxide
Acid + Hydrogen carbonate ------> Salt + Water + Carbon dioxide
Indicators
Indicators - weak acids / bases whose conjugates have different colors
8.3 The pH Scale
pH is inversely related to [H+]
pH = - log10 [H+]
pOH = - log [OH-]
pH + pOH = 14
[H+] = 10^-pH
[OH-] = 10^-pOH
increasing pH by one unit decreases the concentration of H+ ions by 10 times
When [H+] = 1 x 10^-y, pH = y
8.4 Strong and Weak Acids and Bases
Completely ionizes or dissociates, equilibrium lies far to the right
Strong acid has weak conjugate base (weaker than water)
Weak acid doesn't dissociate fully, equilibrium lies to the left (still present as acis at equilibrium), has strong conjugate base (stronger than water, successful in pulling off H+ ions)
Strong - High electrical conductors due to full dissociation into ions.
Weak - small dissociation = bad electrical conductors
Strong Acids
HCl
HBr
HI
HNO3
H2SO4
HClO4
Strong Bases
LiOH
NaOH
KOH
RbOH
CsOH
Sr(OH)2
Ba(OH)2
Ca(OH)2
Stronger acids react faster as there are more H+ ions
8.5 Acid Deposition
pH of rainwater = 5.6
carbon dioxide dissolves in water to produce carbonic acid
Acid Deposition
Wet Deposition
Acid Rain
Main contributors - sulfur and nitrogen oxides
secondary pollutant formed when primary pollutant dissolves in water
pH < 5.6
active compounds
HNO3, NHO2, H2SO4, H2SO3
Process by which acidic component (precipitates/ gases) leave atmosphere and fall to earth
Dry Deposition
acidifying particles fall to ground as dust/smoke and dissolve in water on earth
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