Acids and bases
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| Arrhenius acid | anything that produces hydrogen ions in aqueous soln
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| Arrhenius base | anything that produces hydroxide ions in aqueous soln
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| Bronsted and Lowry acids | anything that donates a proton
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| Bronsted and Lowry base | anything that accepts a proton
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| Lewis acid | anything that accepts a pair of e's
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| Lewis base | anything that donates a pair of e's
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| the stronger the acid, the _____ the conjugate base | weaker
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| the stronger the base, the _____ the conjugate acid | stronger
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| amphoteric | a substance that can act as either an acid or base
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| strong acids | HI, HBr, HCl, HNO3, HClO4, HClO3, H2SO4
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| strong bases | NaOH, KOH, NH2-, H-, Ca(OH)2, Na2O, CaO
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| polyprotic acid | acids that can donate more than 1 proton
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| diprotic acid | acids that can donate 2 protons, the second proton is usually so weak and often negligible
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| acid dissociation____ with acid concentration, but acid strength ____ with an acid concentration | decreases, increases
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| 3 factors determining whether H containing molecule will release its H and act as an acid | (1) strength of bond holding H (2) polarity of the bond (3) stability of the conjugate base
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| ___ conjugate base stability will increase acidity | increasing
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| ___ polarity will increase acidity | decreasing
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| ___ bond strength will increase acidity | decreasing
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| in a series of oxyacids, more oxygens means a __ acid | stronger (hypochlorous acid < chlorous acid < chloric acid < perchloric acid)
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| hydride | cmpd with only 2 elements and 1 being hydrogen; can be acidic, basic, or neutral (where acidity increases down and to the right of the periodic table)
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| metal hydrides are ____ | basic or neutral
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| nonmetal hydrides are ___ | neutral or acidic
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| acidity of nonmetal hydrides tends to ___ going down the table | increase (H2O < H2S < H2Se < H2Te
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| autoionization of water | H2O + H2O --> H3O+ + OH-, equilibrium constant Kw
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| Kw | [H+][OH-] = Ka*Kb = 10^-14
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| pKw | =pH + pOH = 14
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| acid dissociation constant | Ka, equilibrium constant for acid dissociating in water, = [H+][A-]/[HA]
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| Kb | equilibrium constant for the reaction of the conjugate base with water, =[OH-][HA]/[A-]
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| salts | ionic cmpd's that dissociate in water and often create acidic or basic conditions; pH of such son can be predicted qualitatively by comparing conjugates of the respective ions
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| titration | drop-by-drop mixing of an acid and a base
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| equivalence point | for a monoprotic acid, is the point in the titration when there are equal equivalents of acid and base in solution
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| equivalence point for equally strong acid-base titrations | pH= 7
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| half equivalence point | point where we could add the largest mat of acid or base w/ the least amt of change in pH (most well buffered); where there is 50% A- and 50%HA; point where half of the acid has been neutralized by the base
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| Henderson-Hasselbach eqn | pH = pKa + log([A-]/HA]); when at the half equivalence point, the pH = pKa
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| indicator | usually a weak acid whose conjugate base is a different color
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| endpoint of indicator | point where the indicator changes color, but it is not the same as the equivalence point
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