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Arrhenius theory
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acids are substances that contains hydrogen and dissociates to produce H+, and a base is any substance that cointains hydroxide and dissociates to produce OH-
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disadvantage of arrhenius theory
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not all bases contain OH, but can produce it when dissolved in water
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Ex: NH3 - NaCO3
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Bronsted-Lowry Theory
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Acids are H+ donors, bases are H+ acceptors
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Conjugate Pairs
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acids that donate H+ and become bases are called conjugate bases, while bases that accept H+ and become acids are called conjugate acids
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acids and bases are both electrolytes
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water can act as an acid and base, so it is amphoteric
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PH = -log[H+]
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POH = -log[OH-]
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PH + POH = 14
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Monoprotic Acid
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can only donate one H+ ion
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Polyprotic Acid
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can donate multiple H+ ions
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Lewis Theory
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acids are an electron pair acceptor, bases are an electron pair donor
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Lewis Acids
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BF3, BCl3, H+, Ag+
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Lewis Bases
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F_, PCl3, NH3, Cl_
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Acidic Anhydrides
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nonmetal oxides that react with water to produce an acid
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Ex: CO2
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Basic Anhydrides
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metal oxides that react with water to form a base
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Ex: CaO
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water dissociation constant (kw)
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[H+] x [OH_] = 10-14
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Neutralization Reaction
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acid + base = water + salt
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Titration
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a method of finding an unknown acid or base's concentration by using a known one (standard solution)
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Equivalence Point
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Moles H+ = Moles OH-
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acid-base indicators
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substances that change color in acidic or basic solutions (bromothymol, phenolphthalein)
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Hydrolysis of salt
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a reaction in which one of the salt's ions reacts with water to produce an acidic or basic solution
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Buffer Solution
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a solution that resists a change in its PH
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Buffer capacity
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the amount of acid or base that can be added without a significant change in PH
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