Acids & Bases Flashcards
Acid Properties
pH below 7
Tastes sour
Metal corrosive - can react with certain metals and create holes in them
Arrhenius Acid
Substances that dissociate to produce hydrogen ions (H+)j or hydronium ions (H3O+) in a water solution
1H + H2O –> 1H30
Dissociate
Separates into ions
Indicators (Acids)
Litmus - Blue turns red in acids, red stays red in acids
Phenolphthalein - Turns colorless in acids
Indicators (Bases)
Litmus - Red turns blue in bases, blue stays blue in bases
Phenolphthalein - Turns pink/purple in bases
Bronsted-Lowry Acid
Acids DONATE “protons”
Bronsted-Lowry Bases
Bases ACCEPT “protons”
Naming Binary Acids
Since acids start with H+ the name starts with HYDRO-
Acids change the name of the 2nd element to -IC
Ex. Hydrofluoric Acid, Hydrochloric Acid, etc.
Naming Non Binary Acids
Drop the HYDRO-
Change polyatomic ion name to -ic
Ex. Sulfuric Acid, Nitric Acid, etc.
Amphiprotic
Means it can donate OR accept an H+
It can act as an acid or a base
Self Ionization of Water
Water is amphiprotic and can react with itself
H2O + H20 <—> H30 + OH
Strong Acids/Bases
Dissociate completely
HX –> H + X
Weak Acids/Bases
Dissociate incompletely
(Can’t make up its mind)
HX <–> H + X
Strong Acids
HCl - Hydrochloric Acid
HBr - Hydrobromide Acid
HI - Hydroiodic Acid
HNO3 - Nitric Acid
H2SO4 - Sulfuric Acid
HClO4 - Perchloric Acid
If it is not one of these acids it is weak
Weak Acid
HC2H3O2 - Acetic Acid
(most common weak acid, vinegar)
