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39 Cards in this Set
- Front
- Back
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Arrhenius definition of acid/base
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ACID is something that releases H+ in solution. (acid, acid species)
BASE is something that releases OH- in solution (base, base species) |
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Compound that results from neutralization reaction
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H20
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Why does NH3 not clearly fit the Arrhenius definition of a base?
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It doesn't not have OH- in its formula
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Bronsted-Lowry: acid/base
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ACID is a proton (H+) donor (acid, conjugate base)
BASE is a proton (H+) acceptor (base, conjugate acid) transfer of H+/H30+/proton good definition for aqueous chemistry |
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Conjugate pair
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acids and bases appear in conjugate pair, which differ by one H+
eg. H20 has 2 H+, OH- has 1 H+ |
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Do equilibria favor weaker or stronger acids and bases?
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Equilibria favor weaker acids and bases.
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What K value drives a reaction forward?
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A small K value.
Recall k=[products]/[reactants] |
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What is the strongest acid (solvent cation) that can exist in water?
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H3O+
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What is the strongest base (solvent anion) that can exist in water?
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OH-
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Name H3O+
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hydronium ion
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solvent cation
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strongest acid in solution
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solvent cation
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strongest acids (HH4+)
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solvent anion
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strongest base (HH2-)
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leveling effect
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solvent levels the effect of a strong acid or base dissolved in it. the strength of acids or bases added to water are leveled to the strength of H30+ and OH-.
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Strong acids correlate to
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weak conjugate base
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Strong bases correlate to
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weak conjugate acid
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Who's your favorite man?
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Nanner.
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Name oxyacids:
ate-> |
-ic acid
eg. nitrate -> nitric acid |
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Name oxyacids:
ite-> |
-ous acid
eg. nitrite -> nitrous acid |
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List the 6 strong acids
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HCl
HNO3 H2SO4 HBr HI HClO4 |
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Characteristic of strong acids
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100% dissociation (completely dissociate into ions)
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Strong bases
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hydroxides (-OH) in Group I and II
eg. NaOH, KOH, Mg(OH)2 |
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Common weak acid
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NH3 (ammonia)
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HClO4
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perchloric acid
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HClO3
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chloric acid
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HClO2
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chlorous acid
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HClO
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hypochlorous acid
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amphoteric/amphiprotic
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a compound that can be an acid or a base (i.e. water)
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autoionization
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a process by which the solvent ionizes itself (i.e. water)
2 H20 (l) -><- H30+ (aq) + OH- (aq) |
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water's dissociation constant at 25 degrees C
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1.0 X 10^-14
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polyprotic acid
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acids that can donate more than one proton (H+) per molecule
i.e. H2SO4 |
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pKa
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pKa=-log (Ka)
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relationship btw pKa, Ka, and acid/base
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lower pKa value, higher Ka value = strong acid/base
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Low pKa = _____ acid, Ka will be ____
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strong acid, high Ka
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High pKb = ______ base, Kb will be ______
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weak base, low Kb
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Binary acid
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H+ with one other element
eg. HI, HCl |
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Lewis definition of acid/base
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Focuses on electron transfer
LEWIS ACID accepts electrons LEWIS BASE donates electrons ( |
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Conjugate base
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acid in which a proton has been removed
* HCl (aq) + H2O (l) -> H3O+ (aq) + Cl- (aq) * (Acid) +(Base) -> (Conj Acid) + (Conj Base) |
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Conjugate acid
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base in which a proton has been added
* HCl (aq) + H2O (l) -> H3O+ (aq) + Cl- (aq) * (Acid) +(Base) -> (Conj Acid) + (Conj Base) |
