Redox - Acid Base reaction We deal with the Bronsted Lowry...

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Acid Base reaction We deal with the Bronsted Lowry definition of acids and bases Acid – proton donor (proton = H+) Base – proton acceptor • Strong acid – Good examples are HCl, HNO 3 Strong base- good examples are NaOH, KOH Rule: a strong acid or base will completely dissociate. A weak acid will not. A strong acid will cause a weak base to dissociate until all the OH- ions are neutralized. A strong base will cause a weak acid to dissociate unil all the H+ ions are neutralized
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Neutralizing reaction Occurs when the amount of base cancels out with the amount of acid Note: concentration = moles / volume = M Example: what volume of .02 M calcium hydroxide is needed to neutralize 35 mL of .05 M nitric acid Calcium hydroxide Ca + 2(OH-) • Nitric acid H+ + NO 3 Number of moles of H+ = .035L * .05 mol/L = .00175 Need .00175 moles of OH- to neutralize Volume = moles/concentration = .00175/2(.02) = .04375 = 43.75 mL (the 2 in the denominator comes from 2 moles of OH / mole of calcium hydroxide
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Redox: my favorite subject ever First things first- oxidation states defined as the “would be charge” In other words, CO 2 is covalent, and thus share electrons, but oxygen wants them more, so it would get a negative oxidation
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This note was uploaded on 04/08/2008 for the course CHEM 112 taught by Professor Jones during the Fall '07 term at Stevens.

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Redox - Acid Base reaction We deal with the Bronsted Lowry...

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