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