An unlabeled bottle contained an aqueous solution made by dissolving a solute into distilled water. Was the solute a ionic or covalent compound? The testing light did not come on, meaning the solution did not contain electrolytes. Explain fully.

1. To observe the electrical conductivity of various pure liquids, ionic solids, metals and aqueous

solutions using a conductivity probe and LED conductivity indicator.

2. To classify substances as strong, weak or nonelectrolytes.

3. To observe the changes in conductivity during the course of double displacement reactions.

a. Ionic compounds, in the solid state, are composed of ions that are not free to move. The ions

become mobile after the compound is heated to its melting temperature, becomes fluid, and the ions are

freed from their positions in their crystalline lattice. The large number of mobile ions then causes the

molten compounds to become good electrical conductors.

b. Covalent compounds do not conduct electricity even when molten because the resultant mobile

particles are neutral molecules. Their movement cannot be used to carry an electric charge.

Metals conduct electricity in the solid state because the valence electrons of the atoms generate a mobile

“sea” of electrons.

Water is a good solvent for many covalent and ionic compounds. Substances that dissolve in water to

form electrically conducting solutions are electrolytes. Substances that dissolve to form nonconducting

solutions are known as nonelectrolytes. All soluble ionic compounds are electrolytes. Water molecules

are able to pull the positively and the negatively charged ions away from each other in the solid state, and

carry them along to be distributed throughout the solution.

NaCl (s)

!"#

Na+

(aq) + Cl- (aq)

Most covalent compounds are nonelectrolytes. When dissolved, molecules of covalent compounds are

separated from each other by water molecules. The separated molecules are not charged species and will

not conduct electricity. However, some covalent compounds actually react with water to form ions. The

process of forming ions in this manner is known as ionization.

HCl (g) + H2O (l) à H3O+

(aq) + Cl- (aq)

If all dissolved molecules react to form ions, the solution becomes strongly conducting and the solutes are

referred to as strong electrolytes. If only a fraction of the dissolved molecules ionizes the solution

becomes weakly conducting and the compound is known as a weak electrolyte.

HC2H3O2 (aq) + H2O (l) à H3O+

(aq) + C2H3O2

- (aq)

Explanation:

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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