lecture7_031107 - poisoning reversed? a) decrease O 2...

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Equilibrium Consider the formation of HF from its elements: H 2 (g) + F 2 (g) 2HF(g) At equilibrium, what will be the relative concentrations of reactants and products? K c is large, there are more products Now, the concentrations of all species is 2.0 M. Is the system at equilibrium? If not, what directions will it shift? What will be the new concentrations once equilibrium is reached?
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Le Chatlier’s principle What will happen in the following cases for the reaction: H 2 (g) + F 2 (g) 2HF(g) H is positive 1. Add HF(g) 2. Decrease volume 3. Add heat 4. Add xenon
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Le Châtliers Principle A competition experiment involves O2 and CO vying for hemoglobin (Hb) sites, defined by the equilibrium Hb(O 2 ) 4 + 4CO Hb(CO) 4 + 4O 2 From Le Châtelier's principle, how is CO
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Unformatted text preview: poisoning reversed? a) decrease O 2 pressure, b) increase O 2 pressure, c) remove Hb Acid-base equilibria What is the dissociation expression and pH of the following solutions: 1. 0.05 M HCl 2. 0.20 M HNO 2 K a = 4.0 x 10-4 3. 0.10 M Ca(OH) 2 4. 0.30 M NH 3 K b = 1.8 x 10-5 pH calculations How many mL of concentrated HNO 3 (17 M) are required to produce 12.5 L of a pH 2.10 solution? 5.84 mL pH calculations How many moles of ethylamine (CH 3 CH 2 NH 2 ) should you dissolve to make 1.0 L of a pH = 9.5 solution? K b = 5.6 x 10-4 3.34 x 10-5 moles Buffers Calculate the pH of a solution containing 0.75 M lactic acid, HC 3 H 5 O 3 (K a = 1.4 x 10-4 ), and 0.25 M sodium lactate. pH = 3.37...
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lecture7_031107 - poisoning reversed? a) decrease O 2...

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