CH369.lecture2 - Aqueous chemistry Hydrogen bond 1H2O 2H2O...

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Aqueous chemistry
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Hydrogen bond 1 H 2 O 2 H 2 O In Water
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Relative bond strength in biological molecules
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Figure 2.08 Hydration of a nonpolar molecule. Hydrophilic Hydropholic (water loving) vs. (Water fearing)
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Figure 2.10 A micelle formed by amphiphilic molecules. Membrane formation is the result of hydrophobic interaction
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pH Scale
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pH in nature pH-dependent plant pigments that can be used as pH indicators occur in many plants, including hibiscus, marigold and red cabbage
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Compartm ent pH Gastric acid 0.7 Cytosol 7.2 Blood 7.34-7.45
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pH H 2 [H + ] + [OH - ] K =  [H + ][OH-] [H 2 O] Kw = K[H 2 O] =  Kw is water ionization constant = 10 -14  at 25 °C [H + ][OH - ] =10 -14 [H + ][OH - ]  [H 2 O]=55.5 M, it’s a constant. 
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[H + ] and [OH - ] are inversely related Since [H+] and [OH-] are related, only one is need to describe the ionization state of water
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A solution is - Neutral, if [H + ] = [OH - ] = 10 -7 M Acidic , if [H + ] > 10 -7 M ([OH - ] < 10 -7 M) Basic , if [H + ] < 10 -7 M ([OH - ] > 10 -7 M)
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  [ ][ ] [ ] [ ] [ ] [ ] log[ ] log log[ ]/[ ] log[ ]/[ ] A H Ka HA Ka HA H A H Ka HA A pH pKa A HA + - - + - + = = - - = - - = + pH = -log [H+] For an acid: Henderson-Hasselbalch equation
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The lower the pH, the easier that acid ionizes, the stronger the acid.
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Problems Calculate the pH of 1 L of water to which is added (a) 10 mL of 5 M HCl. Complete dissociation: [HCl] = [H + ] = [Cl - ] Final [HCl] =
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Problems Calculate the pH of 1 L of water to which has been added 6 mL of 1.5 M acetic acid and 5 mL of 0.4 M sodium acetate. .
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Buffers A buffer solution is one which resists changes in pH when small quantities of an acid or an alkali are added to it.
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Titration of acetic acid Small amount of Base added
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Blood pH
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This note was uploaded on 03/09/2010 for the course CH 369 taught by Professor Kbrowning during the Spring '07 term at University of Texas.

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CH369.lecture2 - Aqueous chemistry Hydrogen bond 1H2O 2H2O...

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