Chemistry: 1-3

Solution

Homogeneous mixture that when dissolved the particles re mixed uniformly

Solute

The substance that is dissolved

Solvent

The substance that does the dissolving

Solubility

The measure of the maximum amount of solute that can dissolve in a given solvent at a specific temperature

Solvated

Surrounded by solvent particles and move randomly around solution

How does water dissolve ionic compounds?

Water forms ion–dipole attractions that pull ions apart and keep them separated.

What are ion–dipole forces?

Attractions between an ion and a polar molecule (like water).

Like dissolves like

• Polar solvents dissolve polar or charged solutes

• Nonpolar solvents dissolve nonpolar solutes

Miscible

• Two liquids that can mix in any proportion → no limit

• No matter how much you mix, it forms a single solution

Immiscible

• Two liquids that cannot mix to form a solution

• They separate into layers because their molecules don’t interact well

• Usually happens when polar + nonpolar liquids are combined

How to tell solubility of covalent compound?

It has to do with polarity.

Solubility and Entropy

The solute particles spread out → increases entropy (much more freedom of movement for ions or molecules)

Dissolution

is the process in which a solute (solid, liquid, or gas) mixes uniformly with a solvent to form a solution.

• In simple terms: it’s when something “dissolves.”

Sphere of Hydrogen

So the “sphere” is:

• A cluster of water molecules surrounding the hydrogen ion

• Held together by electrostatic attraction

• Sometimes called a hydration shell

Electrolytes

Conduct electricity

• They form ions in solution

• Ions move → carry electric current

• Examples: acids, bases, salts

Non-electrolytes

• They do NOT form ions (stay as neutral molecules)

• No charged particles → no current

• Examples: sugar, alcohol

Network Covalent (Solubility and Conduction)

Does not conduct and does not dissolve

Agaitate

To stir

Dissolves

• Just means a substance mixes evenly in water

• It may stay as whole molecules

• 👉 Happens with both electrolytes AND non-electrolytes

Dissociates

Means a substance breaks into ions in water

Unsaturated Solution

• Contains LESS solute than it can hold

• You can still add more and it will dissolve
  👉 “Not full yet”

Saturated solution

• Contains the MAXIMUM amount of solute at that temperature

• Any extra solute will not dissolve
  👉 “Full”

Supersaturated solution

• Contains MORE solute than it should be able to hold

• Unstable → can crystallize suddenly
  👉 “Overfilled”

Saturation and Graph Relationship

Position on the graph:

• Below the curve → Unsaturated

• On the curve → Saturated

• Above the curve → Supersaturated