1. Solution Chemistry

2. Warm-Up 2/8/17
Solutions are all around us, can you think of what some solutions are?
Think about your labs? Did you have to make a solution? What do you think made that a solution? Do you think of anything like that, that might be a solution?
Who has contacts? Do you use something to wash or clean them?
Are solutions always liquid, can you think of something that might be a solid? Or a gas? Think about what you breath in? is that a solution?
Talk to your partner for a couple of minutes

3. Some Examples What do you think makes these a solution?
Gatorade- what does it have it in? Pennies same thing? What about CuSO4? What was in that solution when you made it? How do you think what you did causes a solution? Are all solutions harmful to eat or drink?
What commonality do you think all of these things have? Is it what they look like? Their phase? How they are made? What they are made of?
How is soda a solution? What makes it carbonated? What does the word carbonated sound like??

4. Definition Solute Solvent
Solutions are homogeneous mixtures that contain two or more substances. Solutions consist of solutes and solvents. Solutes are the dissolved substance in a solution. Solvents are the dissolving medium in a solution.
Solute
Solutes- in CuSO4 what was the solute? What about for the soda example?
Solvent

5. Solutions
Even though most solutions are liquid, solutions do exist as solids, liquids, and gases.
Golf clubs- Zn and Al putters
Irons- stainless steel- carbon and iron
Anyone know what air is made of?
Gases: Air
Solid Alloys
Liquids

6. Soluble versus Insoluble
Some substances readily combine to form solutions, others do not. A substance that dissolves in a solvent is said to be soluble.
A substance that will not dissolve in a solvent is said to be insoluble.
Salt and Water Soluble
Sand and Water Insoluble

7. Miscible versus immiscible
When a liquid dissolves in another liquid it is said to be miscible. Immiscible is when two liquids don’t dissolve.
Oil and Water: Immiscible
Water and alcohol: Miscible

8. Concept Check
What is the difference between soluble and miscible? How are they similar? Write this down in your notebook.

9. Solvation Solvation is the process of dissolving.
Solute particles are surrounded by solvent particles.
Solute particles are separated and pulled into solution.

10. Concept Check
Will KF undergo solvation in water? Why or why not? If it does, describe what will happen.

11. Warm-Up 2/9/17
Get out half a sheet of paper and write and answer the following question: Will NaF undergo solvation? Why or why not? If yes, explain the process.

12. The substance dissolved in a solution is the:
Mixture C) Solvent
Solute D) Solution

13. What is the processes of dissolving?
Mixture C) Solvation
Solvent D) Solution

14. When a liquid dissolves in another, it is said to be
Soluble C) insoluble
Immiscible D) miscible

15. Electrolytes
A solution is said to be an electrolyte when the solution conducts electricity. This happens when there are charged particles in the solution.

16. Electrolytes
There are three types: Non-electrolyte- when the solution does not conduct electricity Weak electrolyte- when the solution conducts some electrical current (but not a lot) Strong electrolyte- when the solution conducts electricity

17. Electrolytes (Continued)
Strong electrolytes are ionic compounds. Weak or non-electrolytes are covalent compounds.
ethanol
NaCl
Acetic acid

18. Solubility Unsaturated solution More solute dissolves
No more solute dissolves
Supersaturated solution
Unstable solution and crystals form

19. Supersaturated Solutions
Diet coke and Mentos
Heat Packs

20. Concentrated and Dilute
A concentrated solution contains more solute than solvent A dilute solution contains more solvent than solute

21. Concept Check
Explain the difference between a supersaturated solution and an unsaturated solution. Give an example of each.

22. When a relatively small amount of solute is dissolved in a solution, it is said to be:
insoluble C) dilute
concentrated D) immiscible

23. A substance that dissolves in water to give a solution that does not conduct an electric current:
electrolyte C) solvation
concentrated D) non-electrolyte

24. Solubility Trends Solids
Solubility of most solids increase with temperature (the higher the temp, the faster the solid dissolves.
Solids dissolve quicker with increasing surface area of the solid (the smaller the size, the faster it dissolves)
Stirring will help dissolve the solid faster

25. Solubility Trend (Cont.)
Gases
Solubility of gases decreases with increasing temperature (the colder the temp, the faster the gas dissolves)
Solubility of gases increases with pressure (higher the pressure, the more the gas will dissolve)

26. Math Time!
Concentration of a solution has 4 main 1. Molarity (M) M= moles liters 3. Percent composition a) %mass/volume = mass of solute X100 %m/v volume of solution b) % volume/volume = volume of solute X100 %v/v volume of solution
measurements:
2. Grams per Liter
g/L = grams liters
4. Parts per million
ppm= mass of solute X106
mass of solution

27. Problems on Molarity
If you have 2 moles of glucose in 8 liters of solution, find the molarity of the solution. Equation: M=moles liters 2 moles = 0.25 M 8 liters

28. Problems on Molarity
A salt solution has a volume of 250 mL and contains moles of NaCl. What is the molarity?

29. Problems on Molarity
A saline solution contains 0.90 grams of NaCl per 100 mL of solution. What is the molarity?