Precipitation:
When a solvent and solute touch, the solute turns into powder of crystals.

Soluble (in water):
The ability to dissolve into a solvent
Physical change

Insoluble:
Substances that don’t dissolve about 0.1M

Electrolyte:
A substance that breaks apart into ions in solutions, like NaCl

Strong Electrolyte:
The substance completely ionizes/break into the solutions.
The water that surrounds the ions make them more stable, which is why they break up
Ex.
Strong Acid, Strong Base, a soluble compound like NaCl

Weak Electrolytes:
A substance that is mostly intact, but they do break apart a little.

The temperature in solutions:
If the temperature increases, more stuff can be dissolved, as the water and ions can move more freely, so the water can get to more and more ions.

Nonelectrolyte:
Does NOT form ions in solution

Precipitation Reaction:
Two ions in (aq) combine to make a solid in the solution

Precipitate:
The solid stuff that comes out

Complete Ionic Equation:
All the ions break apart and then combine into NEW ions on the right side of the equation.
Solids, liquids, and gasses are together in products, but aq’s disassociate.

Spectator Ion:
When an ion doesn’t react in the equation, so it is just the same on the left side as the right side.

Net Ionic Equation:
When you cancel out the spectator ions into ONLY the stuff that matters.

Table of what ionic compounds will precipitate:

Examples of Precipitation Reactions:
3, 4, 6 have precipitated, but 1, 5, and 2 haven’t

Here two aqueous solutions touching each other, and at the line where they do they create a line of a precipitate.