1. Acid-Base Chemistry Special Double Replacement Reactions

2. Nature of Solutions –Solutions- homogeneous mixtures Aqueous- water containing dissolved substance(s) (note: not all solutions are aqueous) Solvent- “does the dissolving” Solute- “is dissolved”

3. Suspensions and Colloids (Complete this table using p. 462) PropertySolutionColloidSuspension Size of Particles? Tyndall Effect? Particles Settle? Type of Mixture?

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

5. What is “Dissolving?” Factors Influencing Dissolving Rate of dissolving- influenced by: agitation, temperature, particle size (surface area) Amount that can be dissolved- influenced by: temperature/pressure

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

7. Types of Solutions Unsaturated Solution of NaNO 3 Supersaturated Solution of NaNO 3 Saturated Solution of NaNO 3

8. Interpreting Solubility Curves Solids in water- generally more soluble at higher temperatures (note: Na 2 SO 4 ) Gases in water- solubility decreases with increased temperature

10. Solution Concentration Molarity= moles of solute per Liters of solution (M=n/V) Example: Calcuate the molarity when 75.0 grams of MgCl 2 is dissolved in 500.0 mL of solution.

11. Concentrated vs. Dilute

12. Practice Determine the molarity of the following solutions: –120. grams of calcium nitrite in 240.0 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 Na 2 SO 4 Dissolve 27 g Na 2 SO 4, dilute to 0.75 L

13. Dilution of Solutions: M 1 V 1 = M 2 V 2 (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 H 2 SO 4 ? –5.0 mL

14. 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 0.0250 M? –6800mL

15. 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 NaHCO 3 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 100.0 mL of a 30.0% ethanol solution, what volumes of ethanol and water are in the solution?

16. Acids and Bases

18. Naming Acids and Bases Recall Naming Rules Salicylic Acid

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

20. Types of Acids 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)

21. Strong v. Weak Strong acids –HCl –HBr –HI –HClO 4 –HNO 3 –H 2 SO 4 Strong Bases –Group I or IIA with OH

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. DEMO

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

25. pH pH = -log[H + ]