Unit 5 – Equilibrium
7.1
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dynamic equilibrium, solubility equilibrium, phase equilibrium
simple ICE tables-determining concentrations at equilibrium
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- equilibrium law, equilibrium constant
heterogeneous equilibria
7.2
7.3
Haber Process: N2(g) + 3 H2(g)  2 NH3(g), look at from the perspective of chemistry
and Le Chatelier’s principle, rates, history, economic, diet.
7.4
Le Chatelier’s Principle: a systemic look what happens as a stress is placed upon an
equilibrium: temperature, pressure, volume, concentration
7.5
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Reaction Quotient (Q)
changes in equilibrium (using ICE table)
calculate K, calculate [reactant] using K value
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-heterogenous equilibria extended to solubility – ICE tables
Ksp and molar solubility, common ion effect
Predicting precipitation
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Arrhenius theory, Bronsted-Lowry theory of acids and bases
conj acid and base pairs, introduction to Ka
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strong and weak acids and bases
weak acid (ka), weak base (kb), pH calculations
ion product of water Kw = [H1+][OH1-] = 1 x 10-14; pH + pOH = 14
Kw = Ka Kb
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Calculating pH, pOH, [OH-], [H+] of strong acid and strong base
Calculating pH, pOH, [OH-], [H+] of weak acid using ICE tables
Calculate - % ionization, Ka and pH
Lewis theory of acids and bases
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Calculating pH, pOH, [OH-], [H+] of weak base using ICE tables
Calculate - % ionization, Kb and pH
7.6
8.1
8.2
8.4
8.5
8.6
pH of salts in solution
8.7
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titrations of strong/weak acids and bases
titration curves of strong/weak acids/bases
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buffers, how they minimize pH changes
8.8