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15 Cards in this Set
- Front
- Back
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Bronsted-Lowry Acid
Lewis Acid Arrhenius Acid |
proton donor
e- pair acceptor produces H+ |
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Bronsted-Lowry Base
Lewis Base Arrhenius Base |
proton acceptor
e- pair donor produces OH- |
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If the anion ends in -ite, it has ____ oxygen atoms and its acid should end with ___
If the anion ends in -ate, it has ____ oxygen atoms and its acid should end with ___ |
1 or 2, -ous acid
more than 2, -ic acid |
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definition of pH and its generic equation
definition of pOH and its generic equation |
a measure of H+ concentration
pH=-log[H+] a measure of OH- concentration pOH==log[OH-] |
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Kw definition and equation
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water dissociation constant, a constant that describes an equilibrium reaction.
Kw=[H+][OH-]=10^-14 |
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Rewrite the Kw equation in logarithmic form
and another form |
pH+pOH=14
Kw=Ka x Kb= 1 x 10^-14 |
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Log x^n = _____
Log 10^x = _____ -Log 10^-x = _____ |
nLog x
x x |
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Common strong Acids
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Hydrogen halides:HCl,HBr,HI
Oxyacids of halogens:HClO3,HClO4,HBrO3,HBrO4 ,HIO3,HIO4 Sulfuric acid:H2SO4 Nitric acid:HNO3 |
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Common strong Bases
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NaOH
KOH CsOH Ca(OH)2 *mostly from the alkali group and some alkaline group |
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the difference b/n strong acids/bases and weak acid/bases
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strong acids and bases dissociate completely into their component ions in aq solution.
weaker species partially dissociate. |
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common weak acids
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Formic HCOOH
Acetic CH3COOH Trichloroacetic CCl3COOH Hydrofluoric HF Hydrocyanic HCN Hydrogen sulfide H2S Water H2O Conjugate acids of weak bases NH4+ |
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common weak bases
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ammonia NH3
trimethyl ammonia N(CH3)3 pyridine C5H5N ammonium hydroxide NH4OH water H2O HS- ion HS- conjugate bases of weak acids e.g.: HCOO- |
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HA+H20->H30+ + A-
Ka equation |
[H30+][A-]/[HA]
*only for aq molecules |
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define conjugate acid
define conjugate base |
the acid formed when a base gains a proton
formed when an acid loses a proton |
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Neutralization reaction
The reverse of this is called _____ |
HA + BOH -> BA + H20
hydrolysis |
