1. Unit 10 – Solutions Lecture 2: Solutions and Solubility

2. Solution: A homogeneous mixture (uniform, no distinct phases)
6.3
Solutions
Solution: A homogeneous mixture (uniform, no distinct phases)
may contain solids, liquids or gasses

3. Solvents and Solutes
A solution is formed when a solute is dissolved in a solvent:
SOLUTE: A substance dissolved in a solution
Ex: Salt dissolved in water, sugar dissolved in iced tea
SOLVENT: The substance that dissolves
Ex: Water in a salt-water solution
AQUEOUS SOLUTION: water is the solvent

4. Solvents and Solutes Types Example Solvent Solute Gas Air
Nitrogen (78%)
Oxygen (21%)
Liquid
Gas in a liquid
Liquid in liquid
Solid in liquid
Solid
Steel
Iron
Carbon

5. Solubility
Solubility: The amount of solute that will dissolve in a solvent at a specified T and P.
A saturated solution contains the maximum amount of dissolved solute.

6. Dissolving Process Water dissolving table salt (NaCl)

7. Dissolving Process
According to the kinetic molecular theory, water molecules are in constant motion and collide with the salt crystals.
The dipoles of the water molecules attract the positive Na+ and negative Cl-.
The water molecules pull apart the salt crystal.

8. “Like Dissolves Like”
Nonpolar solutes dissolve best in nonpolar solvents
Fats
Oils
Gasoline
Polar and ionic solutes dissolve best in polar solvents
Ionic Compounds
Sugars
Water

9. Factors Affecting Solubility
How much solute that can dissolve in a solution depends on:
temperature
pressure (gasses only)

10. Factors Affecting Solubility
Temperature
At higher temperatures, molecules move faster.
Increase in collisions between liquid and solid solutes and solvent => INCREASED SOLUBILITY

11. Solubility of a Gas
Pressure
Increase P, increase solubility of a gas

12. Solubility of a Gas Temperature:
Increased T, increases the motion of gas solute particles so they escape from the liquid => DECREASED SOLUBILITY
What’s more carbonated:
Cold or warm soda?

13. REVIEW
What is the intermolecular bond that affects water’s properties?
Hydrogen Bonds
2. In a salt-water solution, what is the solvent and what is the solute?
Salt: solute water: solvent
3. On a molecular level, how does dissolving of a solute happen?
Molecules are in constant motion. When solvent molecules collide with solute, causes solute to distribute through the solvent.
Changing the temperature usually affects the solubility of a substance. INTERPRETING GRAPHS a. Describe What happens to the solubility of KNO3 as the temperature increases? b. Identify Which substance shows a decrease in solubility as temperature increases? Which substance exhibits the least change in solubility? c. Apply Concepts Suppose you added some solid sodium chloride (NaCl) to a saturated solution of sodium chloride at 20°C and warmed the mixture to 40°C. What would happen to the added sodium chloride?

14. REVIEW
4. How does increased temperature affect solubility of solid and liquid solutes?
Increased solubility for solid and liquid solutes; decreased solubility for gas solutes
Changing the temperature usually affects the solubility of a substance. INTERPRETING GRAPHS a. Describe What happens to the solubility of KNO3 as the temperature increases? b. Identify Which substance shows a decrease in solubility as temperature increases? Which substance exhibits the least change in solubility? c. Apply Concepts Suppose you added some solid sodium chloride (NaCl) to a saturated solution of sodium chloride at 20°C and warmed the mixture to 40°C. What would happen to the added sodium chloride?

15. Solubility Curves
Each line represents the maximum solute that can be dissolved at that temperature.
At 70oC, to make a 100 g saturated solution of KNO3 add 130 g
At 10oC, how many grams of NH3 are required to make a saturated solution?
70 g
Changing the temperature usually affects the solubility of a substance. INTERPRETING GRAPHS a. Describe What happens to the solubility of KNO3 as the temperature increases? b. Identify Which substance shows a decrease in solubility as temperature increases? Which substance exhibits the least change in solubility? c. Apply Concepts Suppose you added some solid sodium chloride (NaCl) to a saturated solution of sodium chloride at 20°C and warmed the mixture to 40°C. What would happen to the added sodium chloride?

16. REVIEW
1. In a salt-water solution, what is the solvent and what is the solute?
Salt: solute water: solvent
2. How does increased temperature affect solubility of a solid in a liquid (salt-water)?
Increased solubility for solid and liquid solutes
3. How does increased temperature affect solubility of a solid in a liquid (CO2-water)?
Decreased solubility for gas solutes in a liquid
Changing the temperature usually affects the solubility of a substance. INTERPRETING GRAPHS a. Describe What happens to the solubility of KNO3 as the temperature increases? b. Identify Which substance shows a decrease in solubility as temperature increases? Which substance exhibits the least change in solubility? c. Apply Concepts Suppose you added some solid sodium chloride (NaCl) to a saturated solution of sodium chloride at 20°C and warmed the mixture to 40°C. What would happen to the added sodium chloride?

17. REVIEW 4. Define a saturated solution?
A solution that contains the maximum amount of solute at a given T.
5. What are two ways to increase solubility?
Temperature and pressure for gases
Changing the temperature usually affects the solubility of a substance. INTERPRETING GRAPHS a. Describe What happens to the solubility of KNO3 as the temperature increases? b. Identify Which substance shows a decrease in solubility as temperature increases? Which substance exhibits the least change in solubility? c. Apply Concepts Suppose you added some solid sodium chloride (NaCl) to a saturated solution of sodium chloride at 20°C and warmed the mixture to 40°C. What would happen to the added sodium chloride?

18. A solution is homogeneous.
Solutions - Summary
A solution is homogeneous.
Solute: substance that is dissolved in the solution.
Solvent: substance that does the dissolving.
“Like Dissolves Like” :
Polar solvents dissolve polar or ionic solutes
Nonpolar solvents dissolve nonpolar solutes.
Solubility: The quantity of solute that will dissolve in a solvent at a given T & P

19. Solutions – Summary (continued)
Saturated solution: contains the maximum amount of solute in a given solvent.
Factors affecting solubility: temperature and pressure (gases only).