1. CHAPTER 14 SOLUTIONSAndMixtures

2. Immiscible = 2 liquids that can be mixed but separate shortly after you stop mixing (oil and vinegar) Immiscible = 2 liquids that can be mixed but separate shortly after you stop mixing (oil and vinegar) Miscible = two liquids that are soluble in each other (water and antifreeze) Miscible = two liquids that are soluble in each other (water and antifreeze)

3. Soluble = if a substance dissolves in a solvent (homogeneous) Soluble = if a substance dissolves in a solvent (homogeneous) Insoluble = doesn’t dissolve (heterogeneous) Insoluble = doesn’t dissolve (heterogeneous)

4. Mixtures: Heterogeneous Heterogeneous Mixture: two or more substances physically combined, but is not uniform throughout Heterogeneous Mixture: two or more substances physically combined, but is not uniform throughout –Suspension: mixture that contains large particles that will settle out if left undisturbed (oil/vinegar)-can be filtered –Colloid: mixture of intermediate sized particles that will not settle out (like milk, blood)-can’t be filtered –Both disperse light in Tyndell effect

5. Types of Colloids Gas dispersed in liquid- foam (whipped cream) Gas dispersed in liquid- foam (whipped cream) Liquid dispersed in gas (fogs-mist), Liquid dispersed in liquid (emulsion-milk, mayo,blood) Liquid dispersed in gas (fogs-mist), Liquid dispersed in liquid (emulsion-milk, mayo,blood) Solid dispersed in gas (smokes), liquid dispersed in liquid (gelatin) Solid dispersed in gas (smokes), liquid dispersed in liquid (gelatin)

6. Tyndell effect (light is reflected off the particles in the mixture)

7. Mixtures: SOLUTION DEF = homogeneous mixture containing two or more substances, uniform throughout (solute dissolved in a solvent) DEF = homogeneous mixture containing two or more substances, uniform throughout (solute dissolved in a solvent)

8. Solvation = the process of surrounding solute particles with solvent particles to form a solution Solvation = the process of surrounding solute particles with solvent particles to form a solution Video Video Video “like dissolves like” “like dissolves like”

9. TYPES OF SOLUTIONS GAS IN GAS =AIR GAS IN GAS =AIR GAS IN LIQUID = SODA GAS IN LIQUID = SODA LIQUID IN GAS= humid air LIQUID IN GAS= humid air LIQUID IN LIQUID =ANTIFREEZE LIQUID IN LIQUID =ANTIFREEZE (ethylene glycol/water) VINEGAR (acetic acid/water) SOLID IN LIQUID=OCEAN WATER (salt/water) SOLID IN LIQUID=OCEAN WATER (salt/water) LIQUID IN SOLID=DENTAL FILLING (Ag in Hg) LIQUID IN SOLID=DENTAL FILLING (Ag in Hg) SOLID IN SOLID=STEEL (Fe in Carbon) SOLID IN SOLID=STEEL (Fe in Carbon) GAS IN A SOLID – pop rocks (mythbuster) (spangler) GAS IN A SOLID – pop rocks (mythbuster) (spangler)mythbusterspanglermythbusterspangler

10. SOLUBILITY Def= the maximum amount of solute that will dissolve in a given amount of solvent at a specific temperature and pressure Def= the maximum amount of solute that will dissolve in a given amount of solvent at a specific temperature and pressure Three types of solutions: Three types of solutions: –Saturated –Unsaturated –supersaturated

12. SATURATED SOLUTION Contains the maximum amount of dissolved solute for a given amount of solvent Contains the maximum amount of dissolved solute for a given amount of solvent

13. UNSATURATED SOLUTION Contains less dissolved solute than a saturated solution (more solute can still be dissolved) Contains less dissolved solute than a saturated solution (more solute can still be dissolved)

15. SUPERSATURATED SOLUTION Contains more solute than a saturated solution, made by increasing the temperature and allowing the solution to cool slowly Contains more solute than a saturated solution, made by increasing the temperature and allowing the solution to cool slowly Very unstable Very unstable Example: rock candy Example: rock candy

16. SEEDING IN A SUPERSATURATED SOLUTION Sodium acetate seeding Sodium acetate sculptures

17. For those about to dissolve, we solute you For those about to dissolve, we solute you For those about to dissolve, we solute you For those about to dissolve, we solute you

18. FACTORS AFFECTING SOLUBILITY TEMPERATURE- as temperature increases the solubility of a gas solute decreases TEMPERATURE- as temperature increases the solubility of a gas solute decreases –Note: most solids increase in solubility w/an increase in temperature PRESSURE- the solubility of a gas in a solvent increases as it’s external pressure increases PRESSURE- the solubility of a gas in a solvent increases as it’s external pressure increases –ex: fizz keeper/soda

19. Mentos and diet soda Mentos and diet soda Mentos and diet soda Mentos and diet soda Experiment 2- domino effect Experiment 2- domino effect Experiment 2 Experiment 2 Mythbusters explain Mythbusters explain Mythbusters explain Mythbusters explain Merry Blastmus (mythbusters) Merry Blastmus (mythbusters) Merry Blastmus Merry Blastmus Why?: It’s a process called "nucleation," in which the particular chemistry of the Mentos candy (mint kind, not- glazed) interacts with the chemistry of the carbonated Diet Coke, causing the carbon dioxide gas, or CO2, to suddenly come out of suspension in the liquid and make a break for freedom. (diet coke instead of regular- no sugary mess for the ants will be left behind) Why?: It’s a process called "nucleation," in which the particular chemistry of the Mentos candy (mint kind, not- glazed) interacts with the chemistry of the carbonated Diet Coke, causing the carbon dioxide gas, or CO2, to suddenly come out of suspension in the liquid and make a break for freedom. (diet coke instead of regular- no sugary mess for the ants will be left behind)

20. MOLARITY (M) Def = concentration of a substance Def = concentration of a substance Used to express the ratio between solute and solvent Used to express the ratio between solute and solvent Specifically, molarity is the ratio between: Specifically, molarity is the ratio between: Moles of solute Liters of solvent M = moles liters

21. Remember: 1000ml = 1 L = 1000cm 3 = 1 dm 3 1. Grams to Molarity 1. Grams to Molarity What is the molarity of a solution if you dissolved 35.2 g of NaCl in 500.0 ml of H2O? Steps: 1. first find molar mass of solute: NaCl = 58.5 g/mole

22. 2. Convert grams to moles 3. use M = mole/liter (convert if needed) 35.2 g NaCl 58.5 g NaCl 1 mole NaCl.602 mol M =.602 mole.5000 L = 1.20 M or 1.20 mole/liter

23. 2. Molarity to grams 2. Molarity to grams How many grams of KBr do you need to make 250 ml of a 0.725 M solution? Steps: 1. convert molarity to moles M = mole liter.725 M = mole.25 L =.18 moles

24. 2. convert moles to grams (molar mass of KBr = 119.1 g/mole) 2. convert moles to grams (molar mass of KBr = 119.1 g/mole).18 mole 119.1 g 1 mole = 21 g

25. PREPARING SOLUTIONS 1. Going from molarity to grams (review) 1. Going from molarity to grams (review) How many grams of CaCl 2 would be dissolved in 1.0 L of a 0.10 M solution? M = mole liter.10 M = mol =.10 mol 1.0 L.10 mol 111.1 g = 11 g 1 mol

26. 2. DILUTION: using concentrated stock solutions and diluting them down to other concentration needed 2. DILUTION: using concentrated stock solutions and diluting them down to other concentration needed The total number of moles does NOT change during dilution The total number of moles does NOT change during dilution

27. M = mole/V M = mole/V moles (concentrate) = M 1 V 1 moles (concentrate) = M 1 V 1 moles (dilute) = M 2 V 2 moles (dilute) = M 2 V 2 Moles concentrate =moles diluted Moles concentrate =moles dilutedSo Dilution formula M 1 V 1 = M 2 V 2

28. What volume of a 3.00 M KI solution would you need to make 0.300 L of a 1.25 M KI solution? What volume of a 3.00 M KI solution would you need to make 0.300 L of a 1.25 M KI solution? V 1 = ? V 1 = ? V 2 =.300 L M 1 V 1 = M 2 V 2 M 1 = 3.00 M M 1 = 3.00 M M 2 = 1.25 M M 2 = 1.25 M (3.00 M)(V 1 ) = (1.25 M)(.300 L) V 1 = (1.25 M) (.300 L) = 0.125 L OF 3.00 M KI 3.00 M 3.00 M So: You would add.125 L of 3.00M KI to.175 L of water to make a 1.25 M solution

30. FREEZING POINT DEPRESSION As a pure solvent reaches freezing point, the molecules KE slows down and the attractive forces between particles take over As a pure solvent reaches freezing point, the molecules KE slows down and the attractive forces between particles take over –It freezes

31. BUT…….. When a solute is mixed in, the solute particles interfere w/the attractive forces, preventing the solvent from freezing at its normal point (lowers the freezing point) When a solute is mixed in, the solute particles interfere w/the attractive forces, preventing the solvent from freezing at its normal point (lowers the freezing point) FREEZING POINT DEPRESSION = the difference in temp. between a solution’s freezing point and the freezing point of the pure solvent FREEZING POINT DEPRESSION = the difference in temp. between a solution’s freezing point and the freezing point of the pure solvent Simulation Simulation Simulation http://www.worsleyschool.net/science/files/saltandfreezing/ofwater. html http://www.worsleyschool.net/science/files/saltandfreezing/ofwater. html http://www.worsleyschool.net/science/files/saltandfreezing/ofwater. html http://www.worsleyschool.net/science/files/saltandfreezing/ofwater. html

33. Types of road salt Types of road salt Types of road salt Types of road salt Making Ice Cream (spangler) Making Ice Cream (spangler) Making Ice Cream Making Ice Cream

34. How its made- ice cream treats http://www.youtube.com/watch?v=SiICaH AOrGE http://www.youtube.com/watch?v=SiICaH AOrGE http://www.youtube.com/watch?v=SiICaH AOrGE http://www.youtube.com/watch?v=SiICaH AOrGE

36. BOILING POINT ELEVATION When a pure solvent reaches its boiling point it has enough kinetic energy to break free from the attractive forces and atmospheric pressure When a pure solvent reaches its boiling point it has enough kinetic energy to break free from the attractive forces and atmospheric pressure BUT….when a solute is added to the solution it must be heated to a higher temp. to supply the additional kinetic energy for the solution to boil BUT….when a solute is added to the solution it must be heated to a higher temp. to supply the additional kinetic energy for the solution to boil

37. BOILING POINT ELEVATION = the temp. difference between a solution’s boiling point and a pure solvent’s boiling pt. BOILING POINT ELEVATION = the temp. difference between a solution’s boiling point and a pure solvent’s boiling pt. Simulation Simulation Simulation

38. Quest 12 multiple choice/short answer 12 multiple choice/short answer –Know vocab –Solution types –Ways to increase/decrease solubility 4 calculations 4 calculations –Grams to molarity –Molarity to grams –Dilution –Formulas/periodic table will be given

39. Song- For those about to dissolve- we solute you For those about to dissolve- we solute youFor those about to dissolve- we solute you Review quiz Review quiz Review quiz Review quiz Hangman Hangman Hangman Jeopardy Jeopardy Jeopardy