var nc = 39, fc = new Array(nc); fc[0] = {t:"Acid (Brønsted-Lowry Acid)",d:"A proton donor."}; fc[1] = {t:"Amphiprotic",d:"A substance that can behave as either a proton acceptor or a proton donor."}; fc[2] = {t:"Base (Brønsted-Lowry Base)",d:"A proton acceptor."}; fc[3] = {t:"Electrolyte",d:"A substance that dissociates into ions when it dissolves, enhancing the conductivity of the solvent."}; fc[4] = {t:"End Point",d:"The point in a titration that is reached when just enough standard solution has been added to cause the indicator to change color."}; fc[5] = {t:"Equivalence Point",d:"The point in a titration where the number of moles of titrant added is stoichiometrically equal to the number of moles of the substance being analyzed."}; fc[6] = {t:"Half-reactions",d:"One of the two halves of an oxidation–reduction reaction; one half-reaction is the oxidation component, and the other is the reduction component."}; fc[7] = {t:"Hydronium Ion (H3O+)",d:"An H+ ion plus a water molecule,H2O; the form in which the hydrogen ion is found in an aqueous solution."}; fc[8] = {t:"Ion Exchange",d:"A process by which one ion is displaced by another."}; fc[9] = {t:"Molarity (M)",d:"The number of moles of solute divided by solution volume in liters: M = n/V. A 1.0 M solution contains 1.0 mol of solute per liter of solution; also known as molar concentration."}; fc[10] = {t:"Molecular Equation",d:"A balanced equation that describes a reaction in solution in which the reactants are written as undissociated molecules."}; fc[11] = {t:"Net Ionic Equation",d:"A balanced equation that describes the actual reaction taking place in aqueous solution; it is obtained by eliminating the spectator ions from the overall ionic equation."}; fc[12] = {t:"Neutralization Reaction",d:"A reaction that takes place when an acid reacts with a base and produces a solution of a salt in water."}; fc[13] = {t:"Nonelectrolyte",d:"A substance that does not dissociate into ions and therefore does not enhance the conductivity of water when it dissolves."}; fc[14] = {t:"Overall Ionic Equation",d:"A balanced equation that shows all the species, both ionic and molecular, present in a reaction occurring in aqueous solution."}; fc[15] = {t:"Oxidation",d:"A chemical change in which a species loses electrons; the oxidation number of the species increases."}; fc[16] = {t:"Oxidation Number (O.N.)",d:"(also called oxidation state)
A positive or negative number based on the number of electrons the atom gains or loses when it forms an ion, or that it shares when it forms a covalent bond with another element; pure elements have an oxidation number of zero."}; fc[17] = {t:"Oxidizing Agent",d:"A substance in a redox reaction that accepts electrons from another species, thereby oxidizing that species; the oxidizing agent is reduced in the reaction."}; fc[18] = {t:"Precipitate",d:"A solid product formed from a reaction in solution."}; fc[19] = {t:"Reducing Agent",d:"A substance in a redox reaction that gives up electrons to another species, thereby reducing that species; the reducing agent is oxidized in the reaction."}; fc[20] = {t:"Reduction",d:"A chemical change in which a species gains electrons; the oxidation number of the species decreases."}; fc[21] = {t:"Salt",d:"The product of a neutralization reaction; it is made up of the cation of the base in the reaction plus the anion of the acid."}; fc[22] = {t:"Saturated Solution",d:"A solution that contains the maximum concentration of a solute possible at a given temperature."}; fc[23] = {t:"Solubility",d:"The maximum amount of a substance that dissolves in a given quantity of solvent at a given temperature."}; fc[24] = {t:"Solute",d:"Any component in a solution other than the solvent. A solution may contain one or more solutes."}; fc[25] = {t:"Solvent",d:"The component of a solution that is present in the largest amount."}; fc[26] = {t:"Spectator Ion",d:"An ion that is present in a reaction vessel when a chemical reaction takes place but is unchanged by the reaction; spectator ions appear in an overall ionic equation but not in a net ionic equation."}; fc[27] = {t:"Standard Solution",d:"A solution of known concentration used in titrations."}; fc[28] = {t:"Stock Solution",d:"A concentrated solution of a substance used to prepare solutions of lower concentration."}; fc[29] = {t:"Strong Acid",d:"An acid that completely dissociates into ions in aqueous solution."}; fc[30] = {t:"Strong Base",d:"A base that completely dissociates into ions in aqueous solution."}; fc[31] = {t:"Strong Electrolyte",d:"A substance that dissociates completely into ions when it dissolves in water."}; fc[32] = {t:"Supersaturated Solution",d:"A solution that contains more than the maximum quantity of solute predicted to be soluble in a given volume of solution at a given temperature."}; fc[33] = {t:"Titrant",d:"The standard solution added to the sample in a titration."}; fc[34] = {t:"Titration",d:"An analytical method for determining the concentration of a solute in a sample by reacting the solute with a standard solution of known concentration."}; fc[35] = {t:"Weak Acid",d:"An acid that only partially dissociates in aqueous solution and so has a limited capacity to donate protons to the medium."}; fc[36] = {t:"Weak Base",d:"A base that only partially dissociates in aqueous solution and so has a limited capacity to accept protons in the medium."}; fc[37] = {t:"Weak Electrolyte",d:"A substance that only partly dissociates into ions when it dissolves in water."}; fc[38] = {t:"Zeolites",d:"Natural crystalline minerals or synthetic materials consisting of three-dimensional networks of channels that contain sodium or other 1+ cations."};