4.7.10.

Sorry the blog took so long to get up, the rain and everything messed with my computer and it kept crashing on me. But here you go.

The seperation of ions that occurs when an ionic compound dissolves is dissociation.
see book for example equations.
review book pg 436 example problem A.

Although no ionic compound is completely insoluble, compounds of very low solubility can be considered insoluble for most practical purposes.

GENERAL SOLUBILITY GUIDELINES -
1. Sodium, potassium, and ammonium compounds are soluble in water.
2. Nitrates, acetates, and chlorates are soluble.
3. Most chlorides are soluble, except those of silver, mercury (I), and lead. Lead(II) chloride is soluble in hot water.
4. Most sulfates are soluble, except those of barium, strontium, lead, calcium, and mercury.
5. Most carbonates, phosphates, and silicates are insoluble, except those of sodium, potassium, and ammonium.
6. Most sulfides are insoluble, except those of calcium, strontium, sodium, potassium, and ammonium.

NOTE:
To decide whether a precipitate can form, you must know the solubilities of those two compounds.

Net Ionic Equation -
includes only those compounds and ions that undergo a chemical change in a reaction in an aqueous solution.
see book pg 439 for example equation.

Spectator Ions -
ions that do not take part in a chemical reaction and are found in solution both before and after the reaction.
see book pg 439 for example equation.

review example problem B, pg 440.

ionization -
ions are formed from solute molecules by the action of the solvent in a process called ionization.

When a molecular compound dissolves and ionizes in a polar solvent, ions are formed where none existed in the undissolved compound.

Hydrogen chlorie, HCl, is a molecular compound that ionizes in aqueous solutions. It contains a highly polar bond. The attraction between a polar HCl molecule and the polar water molecules is strong enough to break the HCl bond, forming hydrogen ions and chloride ions.
see book pg 441 for example equation.

The Hydronium Ion -
some compounds ionize in an aqueous solution to release H+. The H+ ion attracts other molecules or ions so strongly that it does not normally exist alone.
see book for example equation pg 441.

The H3O+ ion is known as the hydronium ion.

Substances that yield ions and conduct an electric current in solution are electrolytes.
Substances that do not yield ions and do not conduct an electric current in solutions are non-electrolytes.

Strong Electrolyte-
is any compound whose dilute aqueous soltions conduct electricity well; this is due to the presence of all or almost all of the dissolved compound in the form of ions.

Weak Electrolyte -
is any compound whose dilute aqueous solutions conduct electricity poorly; this is due to the presence of a small amount of the dissolved compound in the form of ions.

STRONG AND WEAK ELECTROLYTES DIFFER IN **THE DEGREE OF IONIZATION OR DISSOCIATION.**

Have a good night guys.
Colby & Co.