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By: Heidi & Courtni
In strong bases OH- separates easily.
LiOH
NaOH
KOH Alkali Metals w/ OH
RbOH
CsOH
Ca(OH)2
Sr(OH)2 Earth Alkali Metals
Ba(OH)2
Arrhenius- OH- ions present
Lithium Diisopropylamide
In a strong acid the H+ separates easy
Strong acids include:
Arrhenius - H+ ions are present
HCl
HBr
HI
H2SO4
HNO3
HClO3 (Sometimes)
In weak acids H+ stay on for the most part.
Every other acid is a weak acid.
Methane is one of the weakest acids
In a weak base the OH- stay on for the most part.
Every other base is a weak base.
Ammonia is an example of a weak base
Buffers resist large pH changes in a solution.
Consists of either
-A weak acid and it's conjugate base
-A weak base and it's conjugate acid
Examples: Blood, Lemonade
Turns red on blue Litmus paper
and is sour in taste.
Turns blue litmus paper red. Bitter in taste.
Equal amounts of acid and base
pH= 7.00
pOH= 7.00 at any temperature
[H+]=[OH-]
equilibrium changes at different temperatures
Neutral is not a lack of acid or base, it's the same amount of each.
Bronsted focuses on P+
HCl+H20 Cl-+H3O+
A CB
H2O+NH3 OH-+NH4+
A CB
Anything that donates a H+
is an acid
Bronsted focuses on protons
Base accepts H+ (H3O+)
+
Acid Base
HCl + H2O Cl- +H30+
B CA
One of Mrs. Young's favorite things... deodorant!
Cleaners, Laxatives, Baking Soda, Detergents (Then we are able to have clean clothes), Bleach is also a base one of the stronger ones too. Lithium Diisopropylamide.
Example: Stomach acids break down our food in our stomach. Also, Vinegar,
Asprin, Batteries, Explosives, Soft Drinks, Vitamin C,
Fertilizer. Hydrofluoric Acid.
Acids accepts electrons
Typically things with a + is an acid
Lewis Focuses on lone pairs
When added to water acids increase the
concentration of H+ ions present
Example: Soap is a base
that is both polar and non-polar. It breaks down polar and non-polar substances by forming micelles.
Lewis structures focuses on lone pairs
Bases are electron donors
Bases with a - are a base
A Conjugate pair is pairs of acids and bases where the acid is the one with more H+'s.
The formulas differ by one H+ ion.
H2Y-+H2Z H3Y+HZ-
Example: Acid: NH4+
Conjugate Base: NH3
A conjugate is a pair of acids and bases. The bases where the bases have less H+.
The formulas differ by one H+ ion.
H2Y-+H2Z H3Y+HZ-
Example:
Base: NH3
Conjugate Acid: NH4+