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Aqueous solution
A solution in which water is the solvent.
Solvent
The dissolving medium of a solution; it is normally the component of a solution present in the greater concentration.
Solute
A substance dissolved in a solvent to form a solution; it is normally the component of a solution present in the smaller amount.
Electrolyte
A solute that produces ions in solution; an electrolytic solution conduct an electric current.
Nonelectrolyte
A substance that does not ionize in water and consequently gives a nonconducting solution.
Solvation
The clustering of solvent molecules around a solute particle.
Strong electrolyte
A substance (strong acids, strong bases, and most salts) that is completely ionized in solution.
Weak electrolyte
A substance that only partly ionizes in water.
Chemical equilibrium
A state of dynamic balance in which the rate of formation of the products of a reaction from the reactants equals the rate of formation of the reactants from the products; at equilibrium the concentrations of the reactants and products remain constant.
Precipitation reaction
A reaction that occurs between substances in solution in which one of the products is insoluble.
Precipitate
An insoluble substance that forms in, and separates from, a solution.
Solubility
The amount of a substance that dissolves in a given quantity of solvent at a given temperature to form a saturated solution.
Exchange (metathesis) reaction
A reaction between compounds that when written as a molecular equation appears to involve the exchange of ions between the two reactants.
Metathesis (exchange) reaction
A reaction in which two substances react through an exchange of their component ions: AX + BY -> AY + BX. Precipitation and acid-base neutralization reactions are examples of metathesis reactions.
Molecular equation
A chemical equation in which the formula for each substance is written without regard for whether it is an electrolyte or a nonelectrolyte.
Complete ionic equation
A chemical equation in which dissolved strong electrolytes (such as dissolved ionic compounds) are written as separate ions.
Spectator ions
Ions that go through a reaction unchanged and that appear on both sides of the complete ionic equation.
Net ionic equation
A chemical equation for a solution reaction in which soluble strong electrolytes are written as ions and spectator ions are omitted.
Acid
A substance that is able o donate a H+ ion (a proton) and here increase the concentration of H+(aq) when it dissolves in water.
Base
A substance that is an H+ acceptor, a base produces an excess of OH- (aq) ions when it dissolves in water.
Strong acid
An acid that ionizes completely in water.
Strong base
A base that ionizes completely in water.
Weak acid
An acid that only partially ionizes in water.
Weak base
A base that only partially ionizes in water.
Neutralization reaction
A reaction in which an acid and a base react in stoichiometrically equivalent amounts; the neutralization reaction between an acid and a metal hydroxide produces water and a salt.
Salt
An ionic compound formed by replacing one or more hydrogens of an acid by other cations.
Oxidation-reduction (redox) reaction
A chemical reaction in which the oxidation states of certain atoms change.
Redox (oxidation-reduction) reaction
A reaction in which certain atoms undergo changed in oxidation states. The substance increasing in oxidation state is oxidized; the substance decreasing in oxidation state is reduced.
Oxidation
A process in which a substance loses one or more electrons.
Reduction
A process in which a substance gains one or more electrons.
Oxidation number (oxidation state)
A positive or negative whole number assigned to an element in a molecule or ion on the basis of a set of formal rules; to some degree it reflects the positive or negative character of that atom.
Activity series
A list of metals in order of decreasing ease of oxidation.
Concentration
The quantity of solute present in a given quantity of solvent or solution.
Molarity
The concentration of a solution expressed as moles of solute per liter of solution; abbreviated M.
Dilution
The process of preparing a less concentrated solution from a more concentrated one by adding solvent.
Titration
The process of reacting a solution of unknown concentration with one of known concentration.
Standard solution
A solution of known concentration.
Equivalence point
The point in a titration at which the added solute reacts completely with the solute present in the solution.
Indicator
A substance added to a solution that changed color when the added solute had reacted with all the solute present in solution.
