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37 Cards in this Set
- Front
- Back
arrhenius acid
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only aqueous solution
produce H in an aqueous solution, proton donoer |
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arrhenius base
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only aqueous solution
produce OH- Hydroxide ion donor |
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Bronsted-Lowry acid
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donate proton
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Bronsted-Lowry base
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accepts proton
|
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lewis acid
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lectron pair acceptor
electrophile |
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lewis base
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electron pair donnor
nucleophile |
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amphoteric
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can act as either base or acid
H2O |
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The sronger the acid the () its conjugate base
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weaker
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Kw
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eq constant for ionization of water
Kw=[H3O+][OH-]=10^-14 at 25C |
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pH
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-log[H3O] = -log[H+]
=log (1/[H+]) |
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pOH
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-log[OH-] =log(1/[H+])
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if [H+] =1x10^-3 then ph is
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3
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strong acid and base
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sissociate completely into component ions in solution
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strong acid is
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strong electrolyte
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HClO4
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strong acid
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HNO3
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strong acid
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H2SO4
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strong acid
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HCl
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strong acid
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HBr
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strong acid
|
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HI
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strong acid
|
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NaOH
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strong base
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KOH
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strong base
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other soluble hydroxides of group 1A and 2A
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strong base
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weaker acid and base
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do not ionize completely
weak electrolyte |
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Ka (Kb)
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equilibrium constant for acid ionization
measure of the degree to which an acid dissociates weaker the acid lower the Ka Ka= conc product /reactant does not contain pure liq or sol |
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neuralization rxn
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acid and base react to form salt and often water
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titration
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the addition of a solution of known concentration and volume to another solution to determine its unknown concentration
determine the Molarity of an acid or base VaMa =VbMb or VaCa=VbCb C=concentration |
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equivalalence point
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point at which the amt of acid equals the amt of base
located at the center of the stepest region on the tiration curve |
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titration of polyprotic acid
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more than one equivalence point
|
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Normality (N)
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is always equal to the whole number multiple of molarity
equivalent of an acid is the quantity that can supply 1 mole of proton 1M H2SO4 =2N |
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buffer solution
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consists of a mixture of weak acid and its salt (conjugate base) or mixture of weak base and its salt (conjugate acid)
resist pH change when small amoutns of acids or base are added |
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Henderson-hasselbach equation
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PH=PKa+log ([conju base]/[weak acid])
POH = pKb + log([conju acid]/[weak base]) when [cojugate base]=[conjugate acid] PH=Pka bc log 1=0 estimate the ph of a solution in the fugger region where the concentration of the species and its conjugate are present in approximately equal concentration |
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CN-
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stong base
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NH2-
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strong base
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nutralization use
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normality
N1V1 = N2V2 |
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dilution use
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use before and after
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more acidic ph? ka? pka?
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how ph
high ka low pka |