1. Special Double Replacement Reactions
Acid-Base Chemistry
Special Double Replacement Reactions

2. 15.2 & 15.3The Nature of Homogeneous and Heterogeneous Systems
Homogeneous Systems – Solutions
Aqueous- water containing dissolved substance(s)
(note: not all solutions are aqueous)
Solvent- “does the dissolving”
Solute- “is dissolved”
Heterogeneous Systems –
Colloids and Suspensions
Contains a dispersed phase in a dispersion medium
Particles in colloids and suspensions are larger than solute particles

3. Suspensions and Colloids
Property
Solution
Colloid
Suspension
Particle Size
0.1-1nm
1-1000nm
1000nm or larger
Particles Settle? No
Yes
Tyndall Effect?
Type of Mixture
Homogeneous
Heterogeneous
Tyndall Effect: The scattering of light by suspended particles
Emulsion: Colloidal suspension of a liquid in a liquid.
(Mayo, margarine, butter, milk)
Know examples from table 15.3 on page 460

4. What is Dissolving?
Term for solute particles being surrounded by solvent molecules = Solvation

5. Properties of Solutions 16.1 and 16.2
Solubility
Concentration

6. Factors Influencing Dissolving
Rate of dissolving- influenced by:
Agitation, temperature, particle size (surface area)
Amount that can be dissolved- influenced by:
Temperature/Pressure

7. Solubility Curves
Solubility- the maximum amount of solute per a given amount of solvent (usually 100g water)

8. Types of Solutions Supersaturated Solution of NaNO3
Unsaturated Solution of NaNO3

9. Interpreting Solubility Curves
Solids in water- generally more soluble at higher temperatures (note: Na2SO4)
Gases in water- solubility decreases with increased temperature

11. Concentrated vs. Dilute
Concentrated Sugar Solution
Dilute Sugar Solution

12. Solution Concentration
Molarity= moles of solute per Liters of solution (M=n/V)
Example: Calcuate the molarity when 75.0 grams of MgCl2 is dissolved in mL of solution.

13. Practice Determine the molarity of the following solutions:
120. grams of calcium nitrite in mL of solution.
3.79 M
98.0 grams of sodium hydroxide in 2.2 liters of solution.
1.1 M
How many grams of solid are required to make
0.75 L of 0.25 M Na2SO4
Dissolve 27 g Na2SO4, dilute to 0.75 L

14. Dilution of Solutions:
M1V1= M2V2
(note: moles of solute remain constant)
Example: How many mL of a 5.0M stock solution would you need to prepare 100.0mL of 0.25M H2SO4?
5.0 mL

15. Practice
If I have 340 mL of a 0.50 M NaBr solution, what will the concentration be if I add 560 mL more water to it?
0.19 M
To what volume would I need to add water to the solution in the previous problem to get a solution with a concentration of M?
6800mL

16. Percent Solution Percent by Mass
%mass= (mass of solute/mass of solution)*100
What is the percent by mass of NaHCO3 in a solution of 20g NaHCO3 in 600 g of solution?
Percent by Volume (both solute and solvent are liquids)
%volume = (volume of solute/volume of solution)* 100
If you have mL of a 30.0% ethanol solution, what volumes of ethanol and water are in the solution?

17. Acids and Bases

18. Acids and Bases Acids Bases Taste Sour Bitter Feel
Irritating (burning)
Slippery
React with metals
Produce H2 gas NR
Change indicator Colors?
Yes
Characteristic Formula
H in front or COOH at end
OH at the end

19. Types of Acids Oxyacids (H2SO4) - ic acids from ate ions
Mono-, di-, and triprotic acids- have 1, 2, or 3 H atoms that can become ionized
(note: not all compounds that contain H are acidic and not all hydrogens in an acid will necessarily ionize)
Recall Naming Rules for:
Binary Acids (HCl) Hydro _______ ic Acid
Oxyacids (H2SO4) - ic acids from ate ions
- ous acids from ite ions

20. Arrhenius Definition of Acids
Acids- generate H+ ions in water
Bases-generate OH- ions in water

21. Strong v. Weak Strong Bases Strong acids Group I or IIA with OH HCl
Determined by the extent of ionization
Strong Bases
Group I or IIA with OH
Strong acids
HCl
HBr HI
HClO4
HNO3
H2SO4
Small dissociation constants (Ka or Kb) = weak acids and bases
Large dissociation constants = strong acids and bases

22. Neutralization Reactions-
Acid and base react to yield water and a salt

23. Titration-
Slowly adding a solution of known concentration to one of unknown concentration until a neutral solution is formed.

24. Acid-Base Indicators
Used to predict endpoint of titration

25. pH
pH = -log[H+]

26. Strength of Acids – Dissociation constants