Glossary
- Acid: Made up of H+ ions, proton donor, electron pair acceptor.
- Alkali: A base that dissolves in water.
- Arrhenius Theory: Acid produces H+ ions, Bases produce OH- ions.
- Base: Made up of OH- ions, proton acceptor, electron pair donors.
- Bronsted-Lowry Theory: Acids are proton donors, bases are proton acceptors.
- Buffers: A solution which resists small amount of change in pH.
- Concentration: Amount of substance per unit volume.
- Conjugate Acids: A substance created after a base receives a proton (H+).
- Conjugates Bases: A substance left over after an acid loses its proton (H+).
- Dissociates: To split into separate or smaller molecules.
- Exact Titration: Measures the exact amount of acid or base to neutralize its respective counterpart.
- H+ : Hydrogen ion.
- Indicator: Something that indicates if a solution is a base or acid.
- Lewis Theory: Acids are electron pair acceptors, bases are an electron pair donors.
- Log: Function on a graphing calculator used for pH/pOH calculations.
- Molarity: Measure of concentration.
- Moles: Amount of amount of chemical substance.
- Neutralize: To make an acidic or basic solution chemically neutral (pH of 7)
- OH-: Hydroxide ion
- pH: Potential of Hydrogen, measures how acidic or basic something is
- pOH: Potential of Hydroxide, measures how acidic or basic something is
- Rough Titration: Generalization of how much base or acid is needed to neutralize their respective counterpart.
- Second log: Function on a graphing calculator that is equal to 10^(x)
- Strength (for an acid): The ability of an acid to dissociate hydrogen ions
- Strength (for a base): The ability of a base dissociate hydroxide ions
- Titration: A methods where a standard solution with a known concentration is used to determine the concentration of another unknown solution.
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