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Acids and Bases 2024
Vocabulary for Acids and Bases
Term | Definition |
---|---|
Alkaline | Means the same as BASE. A solution in which there are more OH- ions than H+ ions |
Arrhenius Acid | A substance that increases the concentration of hydrogen ions, H+, in aqueous solution |
Arrhenius Base | A substance that increases the concentration of hydroxide ions, OH-, in aqueous solution |
Binary Acid | An acid that contains only two elements: Hydrogen and either Fluorine, Chlorine, Bromine, Iodine, or Sulfur |
Oxyacid | An acid that is a compound of hydrogen and a polyatomic ion containing oxygen |
Strong Acid | An acid that ionizes completely in aqueous solution |
Weak Acid | An acid that does not ionize completely in aqueous solution |
Amphoteric | Any species that can react as either an acid or a base |
Bronsted-Lowry Acid | A molecule or ion that is a proton donor |
Bronsted-Lowry Acid-Base Reaction | The transfer of protons from one reactant (the acid) to another (the base) |
Bronsted-Lowry Base | A molecule or ion that is a proton acceptor |
Conjugate Acid | The species that is formed when a Bronsted-lowry base gains a proton |
Conjugate Base | The species that remains after a Bronsted-Lowry acid has given up a proton |
Diprotic Acid | An acid that can donate two protons per molecule, such as H2SO4 |
Monoprotic Acid | An acid that can donate only one proton (hydrogen ion) per molecule. Example: HBr |
Polyprotic Acid | An acid that can donate more than one proton per molecule such as H2SO4 and H3PO4 |
Triprotic Acid | An acid able to donate three protons per molecule such as H3PO4 |
pH | The negative log of the hydrogen ion concentration of a solution |
pOH | The negative log of the hydroxide ion concentration of a solution |
Self-Ionization of Water | A process in which water molecules break apart to form hydrogen ions and hydroxide ions |
Neutralization | The reaction of hydrogen ions and hydroxide ions to form water molecules |
Salt | An ionic compound |
End Point | The point in a titration at which an indicator changes color |
Equivilance Point | The point at which the two solutions used in a titration are present in equivalent amounts (H+ = OH-) |
Acid-Base Indicator | A compound whose color changes when the pH changes |
Titration | The controlled addition and measurement of the amount of a solution of known concentration required to react completely with a measured amount of a solution of unknown concentration |
Neutral | a substance that has an equal amount of hydrogen ion and hydroxide ion (H+ = OH-) |