1. Unit 7: Solution Chemistry Chapter 13 Chemistry CPA April 2014

2. Water: The “Universal Solvent” Water is referred to as the “universal solvent” because it’s really good at dissolving a vast variety of substances.

3. Water is a Polar Molecule Water is a polar molecule which means it has a “negative” end and a “positive” end The “charged” ends of water help “dissociate” (pull apart) other molecules through attractive forces

4. Hydrogen Bonding Hydrogen bonding: helps water dissociate covalent compounds When atoms of hydrogen are strongly attracted to electronegative atoms on another molecule (specifically oxygen, nitrogen, and fluorine) they make a connection to one another that acts as a bond.

5. Solution Formation A solution consists of a solute and a solvent Solute: lesser amount of particles that gets dissolved Solvent: greater amount of particles that “do” the dissolving. Examples include: Sugar and tea– sugar is the solute, water/tea the solvent Medicine and your blood stream – medicine is the solute, blood is the solvent

6. What affects the rate of a solution’s formation? Solution formation is chemical term for “dissolving” 1.Stirring – aka “agitation” Stirring continually brings solutes into contact with solvent, speeding up solution formation. 2.Temperature Higher temperature means higher kinetic energy – particles move more quickly and collide with one another to speed up solution formation 3.Particle Size Smaller particle size = quicker solution formation

7. Solubility – How does it work? Dissolving all happens due to the kinetic energy of ALL particles involved in the solution. Solvent particles are constantly “bumping into” solute particles, breaking their bonds, and ultimately separating the solute into smaller pieces. Solubility – amount of solute that dissolves in a given quantity of a solvent at a specified temperature and pressure. Solubility is expressed in grams of solute per 100g of solvent.

8. Concentration Is the ratio of solute to solvent If something is very concentrated, there is much more solute than solvent. If something is very un-concentrated (i.e., “watered down” kool-aid), there is much more solvent than solute.

9. Three expressions of solution concentration: 1.Saturated 2.Unsaturated 3.Supersaturated

11. Saturated Solution contains the maximum amount of solute for a given quantity of solvent at standard temperature and pressure.

12. Unsaturated Contains less solute than a saturated solution at standard temperature and pressure.

13. Supersaturated Contains more solute than a solvent can theoretically hold. You will have solid particles left over at the bottom of the container that won’t dissolve.

14. Miscible vs. Immiscible Miscible two liquids that dissolve in each other in all proportions. “Like dissolves Like” – polar and polar dissolve one another; nonpolar and nonpolar dissolve on another. Example – ethanol and water, both polar molecules Immiscible liquids that are not soluble. Polar and nonpolar substances repel one another and do not dissolve Example – oil (nonpolar) and water (polar), oil (nonpolar) and vinegar (polar)

15. Miscible vs. immiscible

16. Solubility Curve x-y graph showing solubility vs. temperature Solubility is on the y-axis, expressed in grams/100g. of solvent Temperature is on the x-axis, expressed in °C On the curve = saturated solution. Under the curve = unsaturated solution. Above the curve – supersaturated solution.

17. Solubility Curve Calculations Solubility is grams of solute/100 g of solvent. Solubility = g. solute 100 g. of solvent What if a problem asked you to find how many grams of a solute you would need to dissolve into 200 g of solvent? 300 g of solvent?

18. 1.What is the solubility of KNO 3 at 20⁰C? 2.You dissolve 30 g of KCl in water at a temperature of 20⁰C. Is the solution unsaturated, saturated, or supersaturated? 3.Suppose you wanted to make a perfectly soluble solution of NaCl in 200 grams of water at 90⁰C. How many grams of NaCl would you need? 4.Which salt shows the least change in solubility from 0 ⁰C to 100 ⁰C? 5.Which salt shows the greatest change in solubility from 0 ⁰C to 100 ⁰C? 6.What general affect does increasing temperature have on the solubility of a substance?

19. Concentration of Solutions Used to describe the ratio of solute to solvent. Three common ways to express concentration in chemistry: Molarity – overall, molar mass-based concentration. Used on stock chemicals. molality – can use just a scale! % solution – used on household products; doesn’t use molar masses.

20. Molarity Defined as moles of solute per 1 liter of solution *Note that the volume is the total volume that results, not the volume of the solvent alone. Equation: M = moles of solute_ Volume (Liters of solution) M moles L

21. Molarity Defined as moles of solute per 1 liter of solution *Note that the volume is the total volume that results, not the volume of the solvent alone. Equation: M = moles of solute_ Volume (Liters of solution)

22. Molarity Practice #1 – Finding M What is the molarity of a 5.00 liter solution that was made with 10.0 moles of KBr ?

23. Molarity Practice #2 – Finding M A 0.250 L solution is made with 0.50 moles of NaCl. What is the Molarity of the solution?

24. Molarity Practice #3 – Finding V (L) What would be the volume of a 2.00 M solution made with 6.00 moles of LiF?

25. Molarity Practice #4 – Finding moles & grams How many moles of NaI would be used to produce a 2.0 M solution with a volume of 1.00 L? Challenge – convert moles  grams!

26. Molarity by Dilution Dilution is the process of decreasing the concentration of a stock solution by adding more solvent (usually water).

27. Dilution Equation M 1 V 1 = M 2 V 2 Where: M 1 is the Molarity of the stock solution V 1 is the volume of the stock solution M 2 is the Molarity of the diluted solution V 2 is the volume of the diluted solution The general purpose of the dilution equation is to find out the volume needed to dilute a stock solution to a desired (lower) concentration. But - You will be given any three (3) of the four variables and be asked to solve for the missing one.

28. Dilution Example #1 A stock solution of 1.00M of NaCl is available. How many milliliters are needed to make a 100.0 mL of 0.750M? M 1 = ______ M x _____ L = ______M x ______ L V 1 = ______ = ______ x ______ M 2 = _____ V 2 = ______

29. Dilution Example #2 Concentrated HCl is 12M. What volume is needed to make 2 L of a 1 M solution? M 1 = ______ M x _____ L = ______M x ______ L V 1 = ______ = ______ x ______ M 2 =_____ V 2 = ______

30. Dilution Example #3 Calculate the final concentration of a solution that was made by adding a 6 M/1L solution of NaOH to 2.5 L of water. M 1 = ______ M x _____ L = ______M x ______ L V 1 = ______ x ______ = ______ M 2 = _____ V 2 = ______