Acids - Bases - Salts Flashcards
special group of compounds
Electrolytes
Electrolyte
Acid, base, salt
Characteristics of electrolytes
Dissociate in water
Conduct electricity in water
Aqueous
Dissociates in water
Dissociate
Dissolves into ions
2 reactions so far
Dehydration polymerization
Fermentation
Why do metals conduct electricity
Sea of mobile electrons
Why do electrolyte solutions conduct electricity
Mobile ions
What does the detailed table look like
Theory. Acid. Base
Arrhenius. H+. H3O+ OH- alkali
Accepted theory proton
Acid =____=_____
Proton, H+
Proton=____=____
Acid, H+
H+=____=____
Acid, proton
Base=____=____
Alkali solution, OH-
Alkali solution=____=____
Base, OH-
OH-=____=____
Base, alkali solution
Hydronium ion
H3O+
What does a proton have to do the be acid-y
Dissociate in water
Arrhenius theory is a.k.a.
Accepted theory (or Acid-base theory)
pH is
The negative log of the hydrogen ion concentration
Range of pH scale
0-14
Strongest acid #
0
Strongest base #
14
Water pH
7
Why does water have a pH of 7
Equal number of H+ and OH-
Acid + metal =
Salt + hydrogen
Salt + hydrogen=
Acid + metal
Neutralization reaction
Acid + base = salt + water
Buffer
Neutralizes an acid or a base
NaHCO3
Baking soda
Baking soda
NaHCO3
Titration
A technique where a solution of known concentration is used to determine the concentration of an unknown solution (Ma•Va=Mb•Vb)
Alternate acids/base theory
Bronsted - Lowery
Bronsted - Lowery theory
Acid is a proton donor
Base is a proton acceptor
Even more detailed table
Not even going to try this one
Similarities between Arrhenius and B - L theory
Both say acid is a proton donor
Differences between Arrhenius and B - L theories
Base
Are - only OH-
B - L - any proton acceptor
Normalizing titration
N•Ma•Va=Mb•Vb•N
What does conjugate base / acid mean
When water reacts with an acid it becomes a conjugate base because it accepts a proton when water reacts with a base it becomes a proton donor AKA a conjugate acid
