Acids & Bases Flashcards
Arrenhenius acid
Gives excess H+ in solution
Arrhenius base
Gives excess OH- in solution
Is water considered an acid in Arrhenius?
No, just aqueous
Bronstead-Lowery acid
Donates H+ ions
Bronstead-Lowery base
Accepts H+ ions (OH-, F-, NH3)
Lewis acid
Electron pair acceptorq
Lewis base
Electron pair donor
What is an electrophile
Lewis acid (attacked by Lewis base neucleophile)
Amphoteric species
Acts as an acid in basic conditions, as a base in acidic conditions (water)
Zwitterion
Intermediate of amino acids that are amphoteric
What hydroxides of metals are amphoteric?
Al, Zn, Pb, Cr
CH3COO-
Acetate
-ide in acid form
-ic
-ite means
less an oxygen
-ite in acid form
-ous acid
-ate means
plus an oxygen
-ate in acid form
-ic acid
Autoionization
Reacts with itself as an amphoteric species (water)
Water dissociation constant
Kw=[H30+][OH-] x 10^-14
Each equal [10^-7]
What it the only thing that can change Kw/water dissociation constant?
Temperature
p=
-log
pH
-log[OH-]=log1/[H+]
pOH
-log[OH-]= log1/[OH-]
pH + pOH =
14
log(xy)
log(x) +log(y)
-log(n x 10^-m)
-log(n)-log(10^-m) = m-log(n)
n
from 1 to 10
p value=
m-0.n
When is pH 7 valid
at 25 degrees Celcius
If the concentration of an acid is less than 10^-7, then the water autoionization is
Significant
What does the Ka or Kb value equal for weak acids and bases?
Less than 1
Strong acids
HCl Hbr HI H2SO4 HNO3 HClO4
Strong bases
NaOH
KOH
Soluble hydroxides of IA metals
Finding Ka or Kb
Use the 10^-14 to find the remaining to find Ka or Kb
Conjugates of strong acids & bases
Basically inert
More electronegative means
Increasing pKa, stronger acid
Weak acis & bases make
Weak conjugate acids & bases