LT#6: Acid Theories and Neutralization Reactions Flashcards
Define Arrhenius Acid
A substance that produces hydrogen ions (H1+) when dissolved in water.
Define Arrhenius Base
A substance that produces hydroxide ions (OH1-) when dissolved in water.
Define Strong
Ionizes (dissociates) 100%
Define Weak
Low percent ionization
Define pH
The strength of hydrogen ions in solution (based on molar concentration of H1+)
One increment on the pH scale means that there are…
10 times more H1+ in the solution
How does acid strength affect pH?
The stronger the acid the more it ionizes, which increases the H1+ concentration and lowers the pH.
How does acid concentration affect pH?
The more concentrated the acid the more acid per unit water, which increases the H1+ concentration and lowers the pH.
Arrhenius Acid + Base –>
Salt + Water
Define Equivalence Point
When acid and base are mixed in amounts that completely neutralize each other.
Define Titration
A lab technique used to determine the unknown concentration of an acid or base by performing a controlled neutralization reaction.
Define Titrant
The opposite reactant added into a titration to determine the concentration of an unknown solution. If unknown acid, then titrant is a base.
Define End Point
When indicator changes colour during a titration and titrant is stopped being added.
When do you use Arrhenius Theory to complete Acid-Base equations?
When you have a base that contains OH1- and you can do a double displacement reaction.
When do you use Bronsted-Lowry Theory to complete Acid-Base equations?
When you don’t have a base that contains OH1-, and you can only transfer an H1+ between chemicals.
