1. Solutions

2. Solutions – homogenous mixture: one substance dissolved in another
solute – the substance being dissolved (fewer particles)
solvent – the substance in which the solute is being dissolved in (more particles)
ex. sugar water: sugar = solute & water = solvent

3. Water A solution w/ water as the solvent is an aqueous solution
Water: the universal solvent
Water is not always the solvent, it can also be the solute if there are fewer water molecules

4. Dissolving – particles spread out evenly
Likes dissolve likes
polar dissolves polar (and ionic, charges)
nonpolar dissolves nonpolar (no charges)
 Gases are more soluble in cold solvents, under high pressure ex. soda bottles

5. Ionization & Dissociation
Ionic cmpds dissolve in a solvent & form ions
Ionic solutions conduct electricity

6. Solubility
The amount of solute that can be dissolved in a specific amount of solvent
The amount of solid dissolved in water is given in units of grams of solid per 100 grams of water.

7. The amount of solid which dissolves in water at a particular temperature is different for different substances. You can plot a graph of the maximum amount of dissolved solid against temperature. Called a solubility curve
Potassium Nitrate
Solubility in grams per 100 grams of water
Sodium chloride
Temperature in °C

9. Concentration The amount of solute per unit volume of solvent
Concentration = mass of solute (g)
volume of solution (L)
1mL of H2O has a mass of 1 gram

10. Types of Solutions Unsaturated – will dissolve more solute
Saturated – won’t dissolve more solute
Supersaturated – has more solute dissolved than solution can normally hold

11. Increase Rate of Dissolving
Increase surface area of solute
Heat solvent (if dissolving a solid, gases dissolve better at lower temperatures)
Stir the solute as it dissolves in the solvent
Increase pressure for dissolving gases