1. Chapter 15 Aqueous Solutions – something is dissolved in water
Solvent – what the stuff is dissolved in (is always the larger amount)

2. A Solute dissolves in water (or other “solvent”)
*the solute is dissolved in the solvent*
is always the lesser amount

3. Effect of Temperature
Increasing T will cause more solid to dissolve in the solvent
Increasing T will cause less gas to dissolve – (think soda pop)

4. Effect of surface area
Increasing surface area will cause more solid to dissolve more quickly:
When more of the solid is in contact with the solvent, it can dissolve better
We can increase the surface area by grinding chunks into a powder

5. Using a volumetric flask to make a solution

6. pure water, sugar solution
Electrolytes
Strong - conduct current efficiently
NaCl, HNO3
Weak - conduct only a small current
vinegar, tap water
Non - no current flows
pure water, sugar solution

7. Concentrated solution: has a lot of solute in it
Dilute solution: has very little solute in it
Saturated solution: no more solute can be dissolved

8. Acids Strong acids -dissociate completely to produce H+ in solution
hydrochloric and sulfuric acid
Weak acids - dissociate to a slight extent to give H+ in solution
acetic and phosphoric acid

9. HCl is strong so it’s completely ionized split apart!

10. Acetic acid (HC2H3O2) is weak so it mostly stays together NOT split!

11. Bases Strong bases - react completely with water to give OH ions.
sodium hydroxide
Weak bases - react only slightly with water to give OH ions.
ammonia

12. Mass Percent Mass percent = mass of solute X 100 mass of solution
Mass of solution = solute g + solvent g

13. Question
A solution is prepared by mixing 5.00 g of ethanol with g of water. Calculate the mass percent of ethanol.

14. Question
Cow’s milk contains 4.5% by mass of lactose, C12H22O11. Calculate the mass of lactose present in 175 g of milk.

15. Molarity Molarity (M) = moles of solute
per volume of solution in liters:
3M can be written as 3 mol
1 L

16. Question
Calculate the molarity of a solution prepared by dissolving 1.56 g of HCl in enough water to make 26.8 mL of solution.

17. QUESTION

18. ANSWER

19. Question
How many grams of NaCl would be required to make 500 mL of a 1.5 M solution.

20. Question
What is the concentration of each ion in a solution of 0.25M K3PO4 ?

21. question
How many moles are in 10.2 mL of M AlCl3?

22. question
How many grams are in 1.75 mL of 1.25M CuCl2?

23. Dilution Water is added to lower the concentration
Only one compound is involved
M1(V1) = M2 (V2)

24. QUESTION

25. ANSWER

26. 400 mL of water is added to 150 mL of 0. 45 M NaOH
400 mL of water is added to 150 mL of 0.45 M NaOH. What is the molarity of the resulting solution?

27. Calculate the volume of 0. 1M NaOH needed to react with 150 mL of 0
Calculate the volume of 0.1M NaOH needed to react with 150 mL of 0.35M H2SO4.
Write the reaction
Pick the substance that you know both M and mL for and start with the mL

28. Use reaction to get molemole
H2SO4 + 2NaOH  Na2SO4 + H2O
4. Use the other molarity to get the volume

29. question
What mass of NaCl must be added to 1.5 L of 0.100M AgNO3 solution to precipitate all of the silver as AgCl?

30. question
Calculate the molarity of NaOH if 27.6 mL reacts with 65.4 mL of a 0.15M solution of H2SO4.