1. Solutions
Chapters 13 and 14

2. Solutions Solution Homogeneous mixture All looks the same Solute
Being dissolved
Solvent
Doing the dissolving
end

3. Solutions Polar Molecule: Do not share equally…
Negative and Positive side
Water (H2O)
end

4. Solutions Nonpolar Molecule : Share equally No charge
Carbon Dioxide (CO2)
end

5. Solutions Polar Molecules ONLY dissolve Polar Molecules
“Like Dissolves Like”
Oil and Water don’t mix!
Pen stains do not wash off with water
end

6. Solutions Ionic Compounds Mixed with Water = Dissociation
Cations and Anions separate and are surrounded by water
NaCl(s) + H2O(l)  Na+(aq) + Cl-(aq)
end

7. Solutions Molecular Compounds Mix with Water = Dispersion
Each molecule surrounded by water
C12H22O11(s) + H2O(l)  C12H22O11(aq)
end

8. Solutions Acids Mix with Water = Ionization Create into H+ and anions
HCl(g) + H2O(l)  H+(aq) + Cl-(aq)
end

9. Properties of Solutions
Solids/Liquids dissolve faster by:
Add more solvent
Increase surface area
Grind solid into a powder
Stir
Increase Temperature
Gases dissolve faster by:
Decreasing Temperature
Increasing Pressure
end

10. Properties of Solutions
Conductivity
Ionic Compounds(aq) and Acids(aq) conduct electricity
Electrolytes
Covalent Molecules will NEVER conduct electricity
Nonelectrolytes
Pure water WILL NOT conduct electricity
end

11. Pure Water= No Electricity Pure NaCl= No Electricity Water + NaCl=
end

12. Properties of Solutions
Electrolytes
Conduct when dissolved
Strong Electrolyte
Completely Dissolves into IONS
Weak Electrolyte
Small Amount Dissolves into IONS
Nonelectrolyte
Does NOT Dissolve into IONS
end

13. end

14. Colligative Properties
Vapor Pressure
Amount of liquid particles that become a gas
More Ions = Lower
end

15. Colligative Properties
B/c the V.P. changes…
Freezing Point
More Ions = Lower
Salt put on icy roads
Boiling Point
More Ions = Higher
Radiators have ethylene glycol dissolved in water
end

16. Determining Solubility of a Substance
Solubility Curve

17. Solubility Solubility
Particles more attracted to solvent than each other
Measured in:
Changes with temperature
At 50 °C, the solubility of KNO3 is 80 g.
Can dissolve up to 80 g of KNO3 in 100 g of water
end

18. Solubility Solubility Curve Solubility at different temps.
What is the solubility of NH3 at 10 °C?
~ ___ g of NH3 / 100 g of H2O
60 g of NH4Cl can be dissolved in 100 g of water at what temperature?
___ °C
How many grams of KClO3 can be dissolved in 200 g of water at 30 °C
~ 22 °C
end

19. Solubility
The amount of solute determines how a solution is classified:
Unsaturated
Saturated
Supersaturated
end

20. Solubility Unsaturated Solutions Can dissolve more solute
BELOW the Line
60 g of KNO3 are dissolved in 100 g of water at 50 °C?
Unsaturated Solution of KNO3
end

21. Solubility Saturated Solution Cannot dissolve any more ON the Line
80 g of KNO3 are dissolved in 100 g of water at 50 °C?
Saturated Solution of KNO3
end

22. Solubility Supersaturated Solution
Supersaturated Solution of KNO3
Supersaturated Solution
Dissolved more than normally possible
ABOVE the Line
130 g of KNO3 are dissolved in 100 g of H2O at 50 °C?
end

23. Concentrations Concentration
The amount of solute in a given amount of solvent
Concentrated
lots of solute
Dilute
little solute
end

24. Concentrations Molarity (M)
You have 0.8 L of a 0.5 M HCl solution. How many moles of HCl does this solution contain?
end

25. Concentrations
You have 3.50 L of solution that contains 90.0 g of sodium chloride, NaCl. What is the molarity?
end

26. Concentrations
You need 23.4 g of potassium chromate in solution for a reaction. If you have a 6.0 M K2CrO4, what volume is needed for the reaction?
end