Term
| Arrhenius acid-base definition |
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Definition
| -acids and bases classified in terms of their formulas and their behavior in water |
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Term
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Definition
| -a substance that has H in its formula and dissociates in water to yield H30+ |
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Term
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Definition
| -a substance that has OH in its formula and dissociates in water to yield OH- |
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Term
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Definition
| -occurs when the H+ ion from the acid and the OH- ion from the base combine to form H20 |
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Term
| Acids and Bases as Electrolytes |
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Definition
| -acids and bases are electrolytes in water, therefore, strong electrolytes (bases or acids) dissociate completely in water |
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Term
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Definition
-Kc is extremely large for strong acids
-Kc is very small for weak acids |
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Term
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Definition
-HCl, HBr, HI, HClO4, HNO3,H2SO4
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Term
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Definition
-LiOH, NaOH, KOH, RbOH, CsOH, Sr(OH)2, Ba(OH)2
-Ca(OH)2 is NOT for class purposes |
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Term
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Definition
-Hydrohalic Acids: HCl, HBr, HI
-Oxoacids in which the # of O atoms exceeds the # of ionizable protons by two or more |
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Term
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Definition
-Hydrohalic Acid HF
-Acids in which H is not bonded to O or a halogen: e.g. HCN and H2S
-Oxoacids in which the # of O atoms equals or exceeds by one the number of ionizable protons
-Carboxylic Acids (formula-RCOOH) |
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Term
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Definition
-M20 and MOH where M = Group 1A(1) metal
-MO or M(OH)2 where M = Group 2A(2) metal (besides Ca(OH)2)
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Term
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Definition
-electron-rich nitrogen atom are weak bases (and they are not Arrhenius bases)
-Ammonia (NH3)
-Amines (gen. formula RNH2, R2NH, or R3N) |
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Term
| Ion-product Constant for Water, Kw |
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Definition
Kw = [H30+][OH-] = 1.0E-14 (at 25 degrees C)
kw = kc[H20]^2 |
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Term
| Consequences of the Auto-ionization of Water |
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Definition
-A change in [H30+] causes an inverse change in [OH-]
-Both ions are present in all aqueous systems |
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Term
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Definition
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Term
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Definition
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Term
| Equilibrium Constants in pK |
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Definition
pK = -log[K]
-a low pK corresponds to a high K |
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Term
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Definition
| pKw = pH + pOH = 14.00 at 25 degrees C |
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Term
| Bronsted-Lowry Acid Definition |
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Definition
-an acid is a proton donor, any species that donates an H+
-All Arrhenius Acids are Bronsted-Lowry acids |
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Term
| Bronsted-Lowry Base Definition |
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Definition
-A base is a proton acceptor, any species that accepts an H+ ion.
-Base must contain a lone pair of electrons to bind to H+ ion |
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Term
| The Bronsted-Lowry Acid-Base Perspective |
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Definition
-the only requirement for an acid-base reaction is that one species donates a proton and another species accepts it
-an acid-base reaction is a proton-transfer process |
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Term
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Definition
| -a substance that acts as a base(accepts a H+) in one case and as an acid(donates a H+) in the other |
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Term
| Conjugate Acid-Base Pairs |
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Definition
-every acid has a conjugate base and vice-versa
-conjugate base has one fewer H and one more minus charge than the acid
-conjugate acid has one more H and one fewer minus charge than the base |
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Term
| Net Direction of Acid-Base Reaction |
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Definition
-a rxn proceeds to the greater extent in the direction in which a stronger acid and stronger base form a weaker acid and weaker base
-e.g. competition for the proton- stronger base wins and becomes conjugate acid |
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Term
| Why does a weaker acid has a stronger conjugate base? |
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Definition
| -the acid gives up its proton less readily bc its conjugate base holds it more strongly |
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