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Unit 6 vocabulary
Term | Definition |
---|---|
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 ironic 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 Ion |
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 yields hydronium ions in water solution. |
Concentration | The amount of solute in a given amount of solvent in a solution. |
Boiling Point Elevation Kb | The difference between the boiling points and the pure solvent and a non-electrolyte solution of that solvent and is directly proportional to the molal concentration of the solution. |
Freezing Point Depression | The difference between the freezing points and a solution of a non electrolyte in that solvent, and is directly proportional to the molal concentration of the solution. |
Solvation | The process of dissolving. |
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 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. |
OH- | Hydroxide ion. |