071408 - { Bile: pH = 6.9 { Urine: pH = 4.8 to 8.3 Using pH...

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ACIDS AND BASES Zumdahl Chapter 14
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Arrhenius Concept y Acid – y Base – Svante Arrhenius 1859 – 1927 Swedish Chemist Noble Prize 1903
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Bronsted – Lowry Definition y Acid – y Base – Johannes Bronsted 1879 – 1947 Danish Chemist Thomas Lowry 1874 – 1936 English Chemist
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Acid Dissociation
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Acid Dissociation
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Acid Strength
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Relative Acid Strength
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Acid Strength
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Different Types of Acids y Polyprotic – y Oxyacid – y Organic –
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Water y Amphoteric – y Autoionization –
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Water
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Using K w y For each of the following solutions calculate [OH - ] from [H + ], or [H + ] from [OH - ]. Classify each solution as acidic or basic. { [H + ] = 3.4 x 10 -9 M { [OH - ] = 0.010 M { [H + ] = 1.0 x 10 -7 M { [OH - ] = 1.2 x 10 -10 M
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pH y pH scale –
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Calculating pH and pOH y Calculate the pH and pOH for the following solutions: { [H + ] = 2.0 x 10 -5 M { [OH - ] = 4 x 10 -3 M { [H + ] = 3.56 x 10 -9 M { [H + ] = 10 -3 M
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Using pH y Given the following pH’s for various biological fluids, calculate the concentration of H + and OH - present: { Gastric Juice: pH = 2.0 { Spinal Fluid: pH = 7.4
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Unformatted text preview: { Bile: pH = 6.9 { Urine: pH = 4.8 to 8.3 Using pH y The pH of 0.040 M hypobromous acid (HOBr) is 5.05. Set up the equilibrium equation for the dissociation of HOBr, and calculate the value of the acid dissociation constant. Calculating pH y Phenol (C 6 H 5 OH) is a weak acid used as a general disinfectant and in the manufacture of plastics. Calculate the pH and the concentrations of all species present in a 0.10 M solution of phenol, K a = 1.3 x 10-10 . Percent Dissociation Percent Dissociation y Calculate the pH and the percent dissociation in 1.5 M HNO 2 , K a = 4.5 x 10-4 . Steps for Solving a Acid Equilibrium Problem A Solution Containing 2 or more Weak Acids y Find the pH of a mixture that contains 0.150 M HF (K a = 3.5 x 10-4 ) and 0.100 M HClO (K a = 2.9 x 10-8 ). What is the hypochlorite ion concentration at equilibrium?...
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071408 - { Bile: pH = 6.9 { Urine: pH = 4.8 to 8.3 Using pH...

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