1. Solutions of Electrolytes
Students will identify electrolytes and explain why they are more affective in lowering the freezing points than non-electrolytes

2. C12H22O11 and C2H6O2

3. What is an Electrolyte? Pure water does not conduct electricity
An electrolyte is substance that when dissolved in water the resulting solution conducts electricity.
They do this by breaking into ions.

4. Weak Electrolytes
When these compounds are added to water they do not ionize (breakup) completely

5. Non-electrolytes
Are compounds such as sugar and ethylene glycol that do not ionize in water.
Since they do not breakup into ions they do nothing to help water carry a charge.

6. Strong Electrolytes Breakup Completely.

7. Colligative Properties
Are properties that depend only on the # of dissolved particles not on the type of particle.
The two properties we are concerned about are boiling and freezing points.

8. Electrolytes almost always contain a metal in the formula
Which are electrolytes?
NaCl C12H22O11 C2H5OH KNO3 LiF

9. Ionic compounds and molecular Compounds
For every molecule of compounds like antifreeze and sugar you add to water, you get one solute particle.
But for every NaCl unit added to water, you get two solute particles because they break into positive and negative ions.

10. Adding non electrolytes to water

11. The “i” factor
The “i” factor is the number of particles the unit becomes when it dissolved in water.
For non-electrolytes the value is one.
For strong electrolytes, it is the number of ions that make up the compound.
For example, Ba(NO3)2 has one barium ion and two nitrate ions. The “i” factor is 3

12. 25 grams NaCl in 100 grams of water
Sodium Chloride is an electrolyte
NaCl  Na Cl-
1.00 mole NaCl = 58.5 grams
Moles NaCl = 25/58.5 = 0.427
Moles of particles = 2 x = 0.855