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18 Cards in this Set
- Front
- Back
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Definition of acid/base: Arrhenius
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acid=ionizes in water and produce H+
HCl -> H+ + Cl- base=ionizes in water and produce OH- NaOH -> Na+ + OH- |
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Definition of acid/base: Bronsted-Lowry
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acid= donate a proton (H+)
base= accepting a proton NH3 + H2O <-> NH4+ + OH- NH3 and OH- are bases H2O and NH4+ are acids |
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Definition of acid/base: Lewis
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acid= electron pair acceptor
base= electron pair donor Exclusively lewis acid-base: NH3 + BCl3 -> H3NBCl3 NH3 base, BCl3 acid. |
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Increasing pH means decreasing
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[H+]
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Strong acids?
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HCl, HBr, HI, HNO3, HClO4, H2SO4
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Strong Bases
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LiOH, NaOH, KOH, Ba(OH)2, Sr(OH)2
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K constant for strong acid/bases?
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does not exist since they dissociate completely
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With an oxoacid like HClOx which would be stronger acid...HClO3 or HClO2
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HClO3 since there are more O atoms attached to central atom, weakening the attraction the central atom has for the H+
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The salt...NaCl..acidic, neutral or basic?
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neutral
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The salt...NH4Cl..acidic, neutral or basic?
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acidic
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The salt...NaC2H3O2..acidic, neutral or basic?
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basic
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conjugates of strong base/acid...what will happen in water?
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weak and unreactive
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Weak base, weak acid salt, pH?
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depend on relative strengths of conjugate acid and base of the specific ions in the salt
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Properties of buffers...
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-pH remains unchanged if diluted or concentrated
-weak acid/base with its conjugate |
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Henderson-Hasselbalch Equation
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pH = pKa - log [Acid]/[base]
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Polyprotic acids
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more willing to give up first protons...so H3PO4 is stronger acid than H2PO4-
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Amphoteric
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act as acid or base
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anhydride
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combine with water to form acid (formed by oxides of nonmetals) or base (formed by oxides of metals)
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