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10 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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