1. Ch. 13 Solutions
What is a solution?
A homogeneous mixture of 2 or more substances in a single phase.
What is a substance that is capable of being dissolved?
Soluble

2. What is the substance being dissolved called?
Solute
The substance that dissolves the solute is called what?
Solvent

3. Homogenous mixture – can’t distinguish the difference in substances
Ex. Tomato juice, pop, vanilla ice cream
Heterogenous mixture – can distinguish the substances in the mixture.
Ex. Stew, salad, chocolate chip ice cream
Video

4. What is an electrolyte?
A substance that conducts electricity in a solution.
Ex. NaCl in water
A nonelectrolyte is a substance that doesn’t conduct electricity in a solution.
Ex. Sugar in water

5. What is an alloy?
A solid solution with 2 or more metals mixed together.
Ex. Cu + Sn = Bronze
Ex. Cu + Zn = Brass
Ex. 50% Au + 50% Cu = 12 karat Au
Video

6. Suspension – is a heterogeneous mixture of a solvent-like substance with particles that slowly settle out.
Ex. Muddy water (separate by a filter)
Video
Colloids – have particles that are intermediate in size between those in solutions & suspension. Don’t settle.
Ex. Milk (Tyndall Effect)

7. Factors that affect the rate of dissolving
1. Heat the solvent
2. Stir/mix the solution
3. Crush/grind the solution
What is solubility?
The rate at which the solvent dissolves the solute at a given temp.
Video

8. Solutions What is a saturated solution?
A solution that can’t take on any more solute and dissolve it.
What is a unsaturated solution?
A solution that can take on more solute.
What is supersaturated solution?
A solution with more solute than a saturated solution. (over saturated)
Video

9. Polar vs. Nonpolar “Likes dissolve alike”
A polar molecule dissolves a polar molecule.
Ex. Water and salt (both polar)
Ex. Gasoline and benzene (non polar)
Ex. Water and gasoline don’t mix
Polar & nonpolar

10. Immiscible are substances that is not soluble in each other.
Ex. Gas & water, oil & water
Miscible are substances that are soluble in each other.
Ex. NaCl & water, gas & benzene

11. Ethanol & ether both have polar and nonpolar ends on their molecules, thus they are able to dissolve both polar and nonpolar substances.
The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid.  Henry’s Law

12. Example of Henry’s Law
Gas is released in a carbonated pop bottle when opened because the pressure is less.
What is effervescence?
The rapid escape of a gas from a liquid in which it was dissolved in.

13. Table 13-4 Solubility vs. Temperature
Concentration of a solution is the measurement of the amount of solute in a given amount of solvent or solution.
Ex. Concentrated O.J. or Conc. HCl
A concentration of a solution can be diluted by adding H2O.

14. Percent by mass is the number of grams of solute dissolved in 100 g of solution.  Sample Problem 13-1
Ex. 10 g of NaOH in 90 g of H2O
10 g of NaOH /
10 g of NaOH + 90 g of H2O X 100%
= 10% NaOH (by mass)

15. Molarity
Molarity is the number of moles of solute in 1 liter of solution.
To find the molarity of a solution you must know the molar mass of the solute.
Molarity (M) = # of moles of solute / # of liters of solution
Example Problem 13-2

16. Molality
Molality is the concentration of a solution expressed in moles of solute per kilogram of solvent.
Molality (m) = # of moles of solute / mass of solvent (kg)
Sample Problem 13-4

17. Nonvolatile is a substance with little tendency to become a gas under the existing condition.
Ex. A lower freezing point & higher boiling point than water.
Colligative property is a property that depends on the # of solute particles, but is independent of their nature.
Ex. antifreeze