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40 Cards in this Set
- Front
- Back
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Hydrogen ion donors
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Acids
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Hydrogen ion acceptors
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Bases
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Strong Acid/Base
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100% ionization in water
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Weak Acid/Base
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< 5% ionization inwater
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Ionization of weak acid/base is a _____-favored process
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Ionization of weak acid/base is a _reactant_-favored process
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Ionization of a strong acid/base is a _____-favored process
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Ionization of a strong acid/base is a _product_-favored process
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Amphiprotic
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A substance that can both accept of donate a proton (act as either acid or base). e.g. water
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Conjugate acid-base pair
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A pair of molecules or ions related to each other by the loss or gain of a single H+ (one has lost H+ and the other has gained)
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One member of a conjugate acid-base pair is always a _______ and the other is always a ________
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One member of a conjugate acid-base pair is always a _reactant_ and the other is always a _product_
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Stronger acids are better H+ ion ____ than weak acids
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Stronger acids are better H+ ion _donors_ than weak acids
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Strong bases are better H+ ion _______ than weak bases
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Strong bases are better H+ ion _acceptors_ than weak bases
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Stronger acids have _____ conjugate bases
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Stronger acids have _weaker_ conjugate bases
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Weaker acids have _____ conjugate bases
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Weaker acids have _stronger_ conjugate bases
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Stronger bases have _______ conjugate acids
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Stronger bases have _weaker_ conjugate acids
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Weaker bases have ________ conjugate acids
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Weaker bases have _Stronger_ conjugate acids
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As acid strength decreases, conjugate base strength _________
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As acid strength decreases, conjugate base strength _increases_
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As base strength decreases, conjugate acid strength ________
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As base strength decreases, conjugate base strength _increases_
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Acid-base reactions favor going from the ______ to the _____ member of each conjugate acid-base pair
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Acid-base reactions favor going from the _stronger_ to the _weaker_ member of each conjugate acid-base pair
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Autoionization
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water molecules react to produce hydronium ions and hydroxide ions in very low concentrations
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Equilibrium constant expression for the autoionization of water
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Kw = [H₃O+][OH-]
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Ionization constant for water
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Kw
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Neutral solution
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equal concentration of H+ & OH-
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pH - formula
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pH = -log([H₃O+])
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pH - definition
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scale for measuring very small concentrations of H₃O+
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pOH - formula
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pH = -log([OH- ])
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pOH - definition
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scale for measuring very small concentrations of OH-
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In relation to pOH, pH =
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. . . 14 - pOH
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in relation to pH, pOH =
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. . . 14 - pH
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The larger the equilibrium constant for an acid's ionization, the ______ the acid
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The larger the equilibrium constant for an acid's ionization, the _stronger_ the acid
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acid ionization constant expression: Kₐ
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Kₐ =
[H₃O+][conj. base] [H₃O+][A-] --------------------------- = ---------------- [conj. acid] [HA] |
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Acid ionization constant - Symbol
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Kₐ
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Acid ionization constant - definition
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measure of the strength of an acid in solution. It is the equilibrium constant for a chemical reaction known as dissociation in the context of acid-base reactions.
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acid ionization constant expression: Kb
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Kb =
[OH-][conj. acid] [OH-][AH] --------------------------- = ---------------- [conj. base] [A-] |
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Polyprotic Acids
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Can donate more than one H+ per molecule
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Oxoacid
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Acid in which the acidic hydrogen is bnonded directly to oxygen in an H-O- bond
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The concentrations in the acid ionization or base ionization expression, mol/L, are . . .
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. . . at equilibrium
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The magnitude of the Ka or Kb value indicates . . .
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. . . how far the forward reaction occurs at equilibrium
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Strong bases and weak acids react to form . . .
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. . . basic salts
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Strong Acids and weak bases react to form . . .
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. . . acidic salts
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Hydrolysis reaction
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A reaction in which a water molecule is split
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