1. Reading for Wednesday Reading for Wednesday Chapter 5: Sections 1-3 Chapter 5: Sections 1-3 HOMEWORK – DUE Wednesday 2/17/16 HOMEWORK – DUE Wednesday 2/17/16 BW 4.1 (Bookwork) CH 4 #’s 3, 7, 9, 16, 17-31 odd, 42, 44, 46, 56, 62, 64, 66, 70, 72, 149 BW 4.1 (Bookwork) CH 4 #’s 3, 7, 9, 16, 17-31 odd, 42, 44, 46, 56, 62, 64, 66, 70, 72, 149 WS 5 (Worksheet) (from course website) WS 5 (Worksheet) (from course website) HOMEWORK – DUE Wednesday 2/17/16 HOMEWORK – DUE Wednesday 2/17/16 BW 4.2 (Bookwork) CH 4 #’s 78-81 all, 83-89 odd, 90, 93, 95, 104-112 even, 116, 156 BW 4.2 (Bookwork) CH 4 #’s 78-81 all, 83-89 odd, 90, 93, 95, 104-112 even, 116, 156 WS 6 (Worksheet) (from course website) WS 6 (Worksheet) (from course website) Lab Monday/Tuesday Lab Monday/Tuesday No lab Monday/open lab on Tuesday No lab Monday/open lab on Tuesday Lab Wednesday/Thursday Lab Wednesday/Thursday Finish EXP 5 Finish EXP 5

2. Solutions Solution – A system in which one or more substances are mixed or dissolved in another substance. Solution – A system in which one or more substances are mixed or dissolved in another substance. Solute – The substance that is being dissolved, or the least abundant component, of a solution. Solute – The substance that is being dissolved, or the least abundant component, of a solution. Solvent – The dissolving agent or the most abundant component in a solution. Solvent – The dissolving agent or the most abundant component in a solution. A solute goes into a solvent to make a solution (solute + solvent = solution) A solute goes into a solvent to make a solution (solute + solvent = solution)

3. A liquid composed of polar molecules is a polar solvent. Water and ethanol are polar solvents. A liquid composed of polar molecules is a polar solvent. Water and ethanol are polar solvents. A liquid composed of nonpolar molecules is a nonpolar solvent. Hexane is a nonpolar solvent. A liquid composed of nonpolar molecules is a nonpolar solvent. Hexane is a nonpolar solvent. Polar and Nonpolar Solvents

4. Polar solvents dissolve in one another. Polar solvents dissolve in one another. Nonpolar solvents dissolve in one another. Nonpolar solvents dissolve in one another. This is the like dissolves like rule. This is the like dissolves like rule. Methanol dissolves in water, but hexane does not dissolve in water. Methanol dissolves in water, but hexane does not dissolve in water. Hexane dissolves in toluene, but water does not dissolve in toluene. Hexane dissolves in toluene, but water does not dissolve in toluene. Like Dissolves Like

5. Polar and Nonpolar Solvents

6. Two liquids that completely dissolve in each other are miscible liquids. Two liquids that completely dissolve in each other are miscible liquids. Two liquids that are not miscible in each other are immiscible liquids. Two liquids that are not miscible in each other are immiscible liquids. Miscible & Immiscible

7. Polar water and nonpolar oil are immiscible liquids and do not mix to form a solution. Polar water and nonpolar oil are immiscible liquids and do not mix to form a solution. Miscible & Immiscible

8. When a solid substance dissolves in a liquid, the solute particles are attracted to the solvent particles. When a solid substance dissolves in a liquid, the solute particles are attracted to the solvent particles. When a solution forms, the solute particles are more strongly attracted to the solvent particles than other solute particles. When a solution forms, the solute particles are more strongly attracted to the solvent particles than other solute particles. Solids in Solution

9. 23.00 grams of hydrogen chloride is added to 55.00 grams of water. solvent = solute = solution = water hydrogen chloride hydrogen chloride solution hydrochloric acidSolutions

10. A potassium permanganate solution contains 1.223 grams of solute solvent = solute = solution = water potassium permanganate potassium permanganate solutionSolutions

11. 59.88 mL of benzene has 12.4 mL of chloroform dissolved into it. solvent = solute = benzene chloroformSolutions

12. We can also predict whether a solid will dissolve in a liquid by applying the like dissolves like rule. We can also predict whether a solid will dissolve in a liquid by applying the like dissolves like rule., are soluble in polar solvents and insoluble in nonpolar solvents. Ionic compounds, are soluble in polar solvents and insoluble in nonpolar solvents. Solids in Solution

13. There are three ways we can speed up the rate of dissolving for a solid compound: There are three ways we can speed up the rate of dissolving for a solid compound: Heating the solution: Heating the solution: This increases the kinetic energy of the solvent, and the solute is attacked faster by the solvent molecules. This increases the kinetic energy of the solvent, and the solute is attacked faster by the solvent molecules. Stirring the solution: Stirring the solution: This increases the interaction between solvent and solute molecules. This increases the interaction between solvent and solute molecules. Grinding the solid solute: Grinding the solid solute: There is more surface area for the solvent to attack. There is more surface area for the solvent to attack. Rate of Dissolving

14. A solution containing exactly the maximum amount of solute at a given temperature is a saturated solution. A solution containing exactly the maximum amount of solute at a given temperature is a saturated solution. A solution that contains less than the maximum amount of solute is an unsaturated solution. A solution that contains less than the maximum amount of solute is an unsaturated solution. Saturated Solutions

15. Under certain conditions, it is possible to exceed the maximum solubility of a compound. A solution with greater than the maximum amount of solute is a supersaturated solution. Under certain conditions, it is possible to exceed the maximum solubility of a compound. A solution with greater than the maximum amount of solute is a supersaturated solution. Saturated Solutions

16. Supersaturation

17. The concentration of a solution tells us how much solute is dissolved in a given quantity of solution. The concentration of a solution tells us how much solute is dissolved in a given quantity of solution. There are several measurements for the concentration of a solution: There are several measurements for the concentration of a solution: mass/mass percent mass/mass percent mass/volume percent mass/volume percent volume/volume percent volume/volume percent molarity molarity ppm (parts-per-million) ppm (parts-per-million) osmolarity osmolarity Concentration of Solutions

18. Mass percent concentration compares the mass of solute to the mass of solution. Mass percent concentration compares the mass of solute to the mass of solution. Concentration – Mass Percent mass of solute mass of solution × 100% = m/m % mass solute mass solute + mass solvent × 100% = m/m %

19. Mass/volume percent concentration compares the mass of solute to the volume of solution. Mass/volume percent concentration compares the mass of solute to the volume of solution. Concentration – m/v Percent mass of solute vol of solution × 100% = m/v %

20. Percent by volume concentration compares the volume of solute to the volume of solvent. Percent by volume concentration compares the volume of solute to the volume of solvent. Concentration – Volume Percent vol of solute vol of solution × 100% = v/v % vol solute vol solute + vol solvent × 100% = v/v %

21. Concentration – Mass Percent A student prepares a solution from 5.00 g NaCl dissolved in 97.0 g of water. What is the concentration in m/m %? Given: solute (NaCl) and solvent (water) (solution not given) A student prepares a solution from 5.00 g NaCl dissolved in 97.0 g of water. What is the concentration in m/m %? Given: solute (NaCl) and solvent (water) (solution not given) A student prepares a solution from 5.00 g NaCl dissolved in 97.0 g of water. What is the concentration in m/m %? Given: solute (NaCl) and solvent (water) (solution not given)

22. Concentration – Mass Percent What is the mass percent of a solution that is made up of 75.0 grams of lithium fluoride and 125 grams of water? given:75.0 g LiF  solute 125 g water  solvent asked:mass %of solution What is the mass percent of a solution that is made up of 75.0 grams of lithium fluoride and 125 grams of water?

23. What is the mass percent of a solution which weighs 625 grams and contains 100.0 grams of potassium bromide? Concentration – Mass Percent given:625 g solution  solution 100.0 g KBr  solute asked:mass % of the solution

24. What is the volume percent of a solution which contains 30.0 mL ethanol and 720.0 mL of water? Concentration – Volume Percent given:720.0 mL water  solvent 30.0 mL ethanol  solute asked:volume % of the solution

25. Solutions When water is the solvent, write as (aq). NaCl (aq) for example. The (aq) means MIXED with water!!! Each solute is a pure substance Solution – A system in which one or more substances are mixed or dissolved in another substance. Solute – The substance that is being dissolved, or the least abundant component, of a solution.

26. We can write several unit factors based on the concentration 4.00% by volume (v/v) ethanol: We can write several unit factors based on the concentration 4.00% by volume (v/v) ethanol: ________ Percent Unit Factors

27. We can write several unit factors based on the concentration 8.11% by mass (m/m) ethanol: We can write several unit factors based on the concentration 8.11% by mass (m/m) ethanol: ________ Percent Unit Factors

28. Concentration – Molarity A 0.125 M solution of sodium chloride ADVICE! Cross out the M and write A 0.125 solution of sodium chloride When given to you, molarity is ALWAYS per 1 L bad better BEST!!!

29. The mole mole Avogadro’s # particles mole molar mass mass mole molar volume volume Only 3 options of what to do with the mole: mole “X” mole-to-mole ratio mole “Y” L solution molarity mole solute

30. We can write 2 conversion factors based on the concentration 6.00 M NaOH: Molarity Unit Factors

31. Concentration – Molarity How many moles of NaCl are in 2.5 L of a 0.355 M solution of sodium chloride?

32. What volume of a 1.250 M potassium hypoiodite solution will contain 0.00456 moles of potassium hypoiodite? Concentration – Molarity

33. How many grams of Li 2 CrO 4 are in 250.0 mL of 0.100 M Li 2 CrO 4 solution? = 3.25 g Li 2 CrO 4 Concentration – Molarity

34. What volume of 12.0 M HCl contains 9.15 g of HCl solute (36.46 g/mol)? What volume of 12.0 M HCl contains 9.15 g of HCl solute (36.46 g/mol)? We want volume; we have grams HCl. We want volume; we have grams HCl. = 20.9 mL HCl solution Concentration – Molarity

35. How would you make 0.0250 L of a 0.0998 M solution of rubidium carbonate (230.95 g/mol)? Concentration – Molarity = 0.576 g Rb 2 CO 3 Add 0.576 grams of rubidium carbonate to 0.0250 L (25.0 mL) of water.

36. What is the molarity of a solution containing 24.0 g of NaOH in 0.100 L of solution? What is the molarity of a solution containing 24.0 g of NaOH in 0.100 L of solution? We also need to convert grams NaOH to moles NaOH (M = 40.00 g/mol). We also need to convert grams NaOH to moles NaOH (M = 40.00 g/mol). = 6.00 M NaOH× 24.0 g NaOH 0.100 L solution 1 mol NaOH 40.00 g NaOH Concentration – Molarity

37. What volume of 6.0 M NaOH needs to be diluted to prepare 5.00 L if 0.10 M NaOH? What volume of 6.0 M NaOH needs to be diluted to prepare 5.00 L if 0.10 M NaOH? We want final volume and we have our final volume and concentration. We want final volume and we have our final volume and concentration. M 1 × V 1 = M 2 × V 2 (6.0 M) × V 1 = (0.10 M) × (5.00 L) V 1 == 0.083 L (0.10 M) × (5.00 L) 6.0 M Dilution Problem

38. Solution Stoichiometry Problem THIS IS HOMEWORK. IT IS DUE NEXT CLASS! What is the mass of all products and reactants after the following reaction finishes: 37.5 mL of 0.100 M aluminum bromide solution reacts with 80.1 mL of 0.133 M silver nitrate solution?

39. What mass of solid is produced from the reaction of 37.5 mL of 0.100 M aluminum bromide solution with 80.1 mL of 0.133 M silver nitrate solution? = 2.11 g AgBr = 2.00 g AgBr AlBr 3(aq) + 3 AgNO 3(aq)  Al(NO 3 ) 3(aq) + 3 AgBr (s) Theoretical yield

40. Oxidation and Reduction Oxidation is the process that occurs when Oxidation is the process that occurs when the oxidation number increases (gets more positive) the oxidation number increases (gets more positive) an element loses electrons an element loses electrons a compound adds bonds to oxygen a compound adds bonds to oxygen a compound loses bonds to hydrogen a compound loses bonds to hydrogen a half-reaction has electrons as products a half-reaction has electrons as products Reduction is the process that occurs when Reduction is the process that occurs when the oxidation number of an element decreases (gets more negative) the oxidation number of an element decreases (gets more negative) an element gains electrons an element gains electrons a compound loses bonds to oxygen a compound loses bonds to oxygen a compound gains bonds to hydrogen a compound gains bonds to hydrogen a half-reaction has electrons as reactants a half-reaction has electrons as reactants

41. Types of Reactions Decompositionone reactant A  B + C + … TypeLook forGenericRedox? depends CaCO 3(s) CaO (s) + CO 2(g) 2 KClO 3(s) 2 KCl (s) + 3 O 2(g) Combination multiple reactants/one product reactants typically elements A + B + …  C YES 3 Mg (s) + N 2(g)  Mg 3 N 2(s) 2 Na (s) + Se (s)  Na 2 Se (s) Combustion Reactant with only C, H, and sometimes O.* A + O 2(g)  CO 2(g) + H 2 O (g) YES 2 CH 4(g) + 3 O 2(g)  2 CO 2(g) + 2 H 2 O (g) *Other things can burn C 2 H 6 O (l) + 3 O 2(g)  2 CO 2(g) + 3 H 2 O (g)

42. Types of Reactions Single replacement an element reacting with a compound (or ion)* A + BX  B + AX TypeLook forGenericRedox? YES 3 Mg (s) + 2 FeCl 3(aq)  3 MgCl 2(aq) + 2 Fe (s) Al(NO 3 ) 3 (s) + Co (s)  N.R. Double replacement typically 2 aqueous solutions reacting AX + BY  AY + BX NO AgNO 3(aq) + NaCl (aq)  AgCl (s) + NaNO 3(aq) 3 K 2 S (aq) + 2 CrCl 3(aq)  6 KCl (aq) + Cr 2 S 3(s) Neutralizationacid and base HA (aq) + BOH (?)  HOH (l) + BA (?) NO HF (aq) + LiOH (aq)  HOH (l) + LiF (aq) *check activity series Ni(OH) 2(s) + H 2 SO 4(aq)  NiSO 4(aq) + 2 HOH (l)

43. An acid is any substance that, H +, into water. An acid is any substance that releases hydrogen ions, H +, into water. Acids are in water and therefor need and (aq) Acids are in water and therefor need and (aq) A base is a substance that, into water. A base is a substance that releases hydroxide ions, OH –, into water. An acid and a base react with each other in a neutralization reaction. An acid and a base react with each other in a neutralization reaction. When an acid and a base react, water and a salt are produced. When an acid and a base react, water and a salt are produced. Acids and Bases

44. HCl (aq) + NaOH (aq)  NaCl (aq) + H 2 O (l) H 2 SO 4(aq) + 2 KOH (aq)  K 2 SO 4(aq) + 2 H 2 O (l) H 2 SO 4(aq) + 2 KOH (aq) + 2 H 2 O (l) 2 H 3 PO 4(aq) + 3 Ba(OH) 2(aq)  Ba 3 (PO 4 ) 2(s) + 6 H 2 O (l) 2 H 3 PO 4(aq) + 3 Ba(OH) 2(aq) + 6 H 2 O (l) HNO 3(aq) + NH 3(aq)  NH 4 NO 3(aq) 2 HBr (aq) + K 2 CO 3(aq)  2 KBr (aq) + H 2 CO 3(aq) + H 2 O (l) + CO 2(g) HI (aq) + NaHCO 3(aq)  NaI (aq) + H 2 CO 3(aq) + H 2 O (l) + CO 2(g)  2 KBr (aq) 2 HBr (aq) + K 2 CO 3(aq)