Today is 18 July 2010 -- Terms needed for the equilibrium exam 

Definitions:

1.  Saturated solution:  A solution which is so concentrated that added solute will not dissolve.

2.  Dynamic equilibrium:  A chemical reaction in which the reverse reaction occurs at the same rate as does the forward reaction, thereby maintaining equilibrium.

3.  Strong acid/weak acid:  Strong acids disassociate completely in solution; weak acids partially disassociate.

4.  Azeotrope:  A mixture of two (or more) substances that cannot be separated by distillation because they form a mixture with a constant boiling point.

5.  pH:  Literally, the "power of Hydrogen."  It relates to the number of hydrogen ions in solution.  The acid/base level.  You can also give the equation pH = - log [H+].

6.  Reversible reaction:  reaction which is reversible due to concentration, temperature or pressure changes

7.  Completion reaction:  reaction which reactants produce products and will not reverse under ordinary conditions

8.  Chemical equilibrium:  condition at which rate of conversion of products to reactants equals rate of conversion of reactants to products.  Referred to as dynamic equilibrium

9.  Complex ion/coordination compound:  metal ions/atoms which reversibly bind to other atoms or molecules.  Best example is reversible binding of oxygen to iron in hemoglobin.

10.  Equilibrium constant, Keq:  Numerical description of the direction (reversibility/non-reversibility) of a chemical reaction.

11.  Solubility product constant, Ksp: Numerical description of how soluble/insoluble is a given substance.

12.  Stalactite:  Ceiling-down mineral formation typically due to calcium carbonate precipitating from water.

13.  Stalagmite: Floor-up mineral formation typically due to calcium carbonate precipitating from water.