1. Chapter 13
Solutions

2. Sect. 13-1: Types of Mixtures
Solution – homogeneous mixture of 2 or more substances with small particle size
Made up of solute (substance being dissolved) and solvent (substance doing the dissolving)
Soluble – can be dissolved
Suspension – a heterogeneous mixture of which the relatively large particles will settle out unless continually stirred
Colloid – heterogeneous mixture with particle size between solutions and suspensions

3. Tyndall effect Used to distinguish between colloids and solutions
Particles in a colloid are large enough that they scatter light as it passes through

4. Electrolyte – substance that when dissolved in water to form a solution will conduct electricity
Non-electrolyte – substance that when dissolved in water to form a solution will not conduct electricity

5. Sect. 13-2: The Solution Process
Factors affecting rate of dissolving:
Increasing surface area of solute
Agitating solution
Heating the solvent

6. Solution equilibrium – physical state in which the dissolving and crystallization of the solute occur in equal rates
Saturated solution – contains maximum amount of solute
Unsaturated solution – contains less than the saturated solution at a given set of conditions
Supersaturated solution – contains more dissolved solute than a saturated solution contains under a given set of conditions

7. Solubility – the amount of a substance required to form a saturated solution with a specific amount of solvent at a specified temperature

8. Solute – Solvent Interactions
“like dissolves like”
During dissolving of ionic compounds, ions are surrounded by the solvent particles and pulled away from the rest of the crystal
Hydration – solution process with water as the solvent
Hydrates have water molecules incorporated in their structures
Ionic compounds are generally not soluble in non-polar solvents

9. Immiscible – liquid solute & solvent that are not soluble in each other
Miscible – liquids that are soluble in each other

10. An increase in pressure increases gas solubility
Henry’s law – solubility of a gas in liquid is directly proportional to the partial pressure of the gas on the surface of the liquid
Effervescence – rapid escape of gas from liquid in which it was dissolved

11. Generally an increase in temperature causes an increase in solubility of a solid in a liquid
An increase in temperature causes a decrease in solubility of a gas in a liquid
See graphs on pg. 408

12. When a solute particle is surround by solvent particles it is said to be Solvated
Heat of solution – the net amount of heat energy absorbed or released when a specific amount of solute dissolves in a solvent
Negative value when heat is released
Positive value when heat is absorbed

13. Sect. 13-3: Concentration of Solutions
Concentration – measure of the amount of solute in a given amount of solvent or solution
Molarity – number of moles of solute dissolved in one liter of solution
Molality – number of moles of solute dissolved per kilogram of solvent

14. Formulas… Molarity (M) = moles solute liters of solution
Molality (m) = moles solute
kg of solvent