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pH hydrogen ion concentration
Titration method used to determine the concentration of a substance in a solution
Dissociation The separation of ions that occur when an ionic compound dissolves
Electrolyte A substance that dissolves in water to give the solution the ability to conduct electricity.
Base proton acceptors identified by release of hydroxide ions.
H3O+ Hydronium
Molarity Number of moles of solute in one liter of solution
Molality The concentration of a solution expressed in moles of solute per kilogram of solvent
Colligative Properties Depend on the concentration of solute particles but not on their identity.
Acid proton donors that yield hydronium ions in water solution
Concentration The amount of solute in a given amount of solvent in a solution.
Boiling Point Elevation The difference between the boiling points of the pure solvent and a nonelectrolyte solution of that solvent and is directly proportional to the molal concentration of the solution.
Freezing Point Depression The difference between the freezing points of the pure solvent and a solution of a non electrolyte in that solvent, and is directly proportional to the molal concentration of the solution.
Kf Molal Freezing point constant
Kb Molal Boiling point constant
Buffer solutions that are used as a means of keeping pH at a nearly constant value in a wide variety of chemical applications
Solubility The capability to dissolve.
End point The point in a titration at which no more titrant should be added. It is determined, for example, by a color change in an indicator or by the appearance of a precipitate.
Neutralization a chemical reaction in which an acid and a base react to form a salt.
pOH hydroxide ion concentration
Created by: brandon.dartez