2. 1 Chapter 8 Solutions Solubility Percent Concentration Colloids and Suspensions

3. 2 Solute and Solvent Solutions are homogeneous mixtures of two or more substances Solute The substance in the lesser amount Solvent The substance in the greater amount

4. 3 Formation of solutions

5. 4 Nature of Solutes in Solutions Spread evenly throughout the solution Cannot be separated by filtration Can be separated by evaporation Not visible, solution appears transparent May give a color to the solution

6. 5 Types of Solutions air O 2 gas and N 2 gas gas/gas soda CO 2 gas in water gas/liquid seawater NaCl in water solid/liquid brass copper and zinc solid/solid

7. 6 Formation of solutions - solvation Cl - Na + Cl - Na + H2OH2O H2OH2O Cl - solute Dissolved solute Hydration

8. 7 Formation of solutions - creating like-like interactions Water Most common solvent A polar molecule O  - a hydrogen bond H  +

9. 8 Formation of solutions - creating like-like interactions

10. 9 When NaCl(s) dissolves in water, the reaction can be written as H 2 O NaCl(s) Na + (aq) + Cl - (aq) solid separation of ions in water

11. 10 Formation of solutions - creating like-like interactions Solid LiCl is added to some water. It dissolves because A. The Li + ions are attracted to the 1) oxygen atom(  -) of water 2) hydrogen atom(  +) of water B.The Cl - ions are attracted to the 1) oxygen atom(  -) of water 2) hydrogen atom(  +) of water Solid LiCl is added to some water. It dissolves because A. The Li + ions are attracted to the 1) oxygen atom(  -) of water B.The Cl - ions are attracted to the 2) hydrogen atom(  +) of water

12. 11 Solubility The maximum amount of solute that can dissolve in a specific amount of solvent usually 100 g. g of solute 100 g water

13. 12 Saturated and Unsaturated A saturated solution contains the maximum amount of solute that can dissolve. Undissolved solute remains. An unsaturated solution does not contain all the solute that could dissolve

14. 13 Learning Check At 40  C, the solubility of KBr is 80 g/100 g H 2 O. Indicate if the following solutions are (1) saturated or (2) unsaturated A. ___60 g KBr in 100 g of water at 40  C B. ___200 g KBr in 200 g of water at 40  C C. ___25g KBr in 50 g of water at 40  C

15. 14 Solution At 40  C, the solubility of KBr is 80 g/100 g H 2 O. Indicate if the following solutions are (1) saturated or (2) unsaturated A. 2 Less than 80 g/100 g H 2 O B. 1 Same as 100 g KBr in 100 g of water at 40  C, which is greater than its solubility C. 2 Same as 60 g KBr in 100 g of water, which is less than its solubility

16. 15 Temperature and Solubility of Solids TemperatureSolubility (g/100 g H 2 O) KCl(s)NaNO 3 (s) 0°27.6 74 20°C34.0 88 50°C42.6114 100°C 57.6182 The solubility of most solids (decreases or increases ) with an increase in the temperature.

17. 16 Temperature and Solubility of Solids TemperatureSolubility (g/100 g H 2 O) KCl(s)NaNO 3 (s) 0°27.6 74 20°C34.0 88 50°C42.6114 100°C 57.6182 The solubility of most solids increases with an increase in the temperature.

18. 17 Temperature and Solubility of Gases TemperatureSolubility(g/100 g H 2 O) CO 2 (g)O 2 (g) 0°C0.340.0070 20°C0.170.0043 50°C0.0760.0026 The solubility of gases (decreases or increases) with an increase in temperature.

19. 18 Temperature and Solubility of Gases TemperatureSolubility(g/100 g H 2 O) CO 2 (g)O 2 (g) 0°C0.340.0070 20°C0.170.0043 50°C0.0760.0026 The solubility of gases decreases with an increase in temperature.

20. 19 Learning Check A. Why would a bottle of carbonated drink possibly burst (explode) when it is left out in the hot sun ? B. Why would fish die in water that gets too warm?

21. 20 Solution A. Gas in the bottle builds up as the gas becomes less soluble in water at high temperatures, which may cause the bottle to explode. B. Because O 2 gas is less soluble in warm water, the fish may not obtain the needed amount of O 2 for their survival.

22. 21 Soluble and Insoluble Salts A soluble salt is an ionic compound that dissolves in water. An insoluble salt is an ionic compound that does not dissolve in water

23. 22 Solubility Rules 1. A salt is soluble in water if it contains any one of the following ions: NH 4 + Li + Na + K + orNO 3 - Examples: soluble salts LiCl Na 2 SO 4 KBr Ca(NO 3 ) 2

24. 23 Cl - Salts 2. Salts with Cl - are soluble, but not if the positive ion is Ag +, Pb 2+, or Hg 2 2+. Examples: solublenot soluble(will not dissolve) MgCl 2 AgCl PbCl 2

25. 24 SO 4 2- Salts 3. Salts with SO 4 2- are soluble, but not if the positive ion is Ba 2+, Pb 2+, Hg 2+ or Ca 2+. Examples: solublenot soluble MgSO 4 BaSO 4 PbSO 4

26. 25 Other Salts 4. Most salts containing CO 3 2-, PO 4 3-, S 2- and OH - are not soluble. Examples: solublenot soluble Na 2 CO 3 CaCO 3 K 2 SCuS

27. 26 Learning Check Indicate if each salt is (1)soluble or (2)not soluble: A. ______ Na 2 SO 4 B. ______ MgCO 3 C. ______ PbCl 2 D. ______ MgCl 2

28. 27 Solution Indicate if each salt is (1) soluble or (2) not soluble: A. _1_ Na 2 SO 4 B. _2_ MgCO 3 C. _2_ PbCl 2 D. _1_ MgCl 2

29. 28 Molarity (M) A concentration that expresses the moles of solute in 1 L of solution Molarity (M) = moles of solute 1 liter solution

30. 29 Units of Molarity 2.0 M HCl = 2.0 moles HCl 1 L HCl solution 6.0 M HCl= 6.0 moles HCl 1 L HCl solution

31. 30 Molarity Calculation NaOH is used to open stopped sinks, to treat cellulose in the making of nylon, and to remove potato peels commercially. If 4.0 g NaOH are used to make 500. mL of NaOH solution, what is the molarity (M) of the solution?

32. 31 Calculating Molarity 1) 4.0 g NaOH x 1 mole NaOH = 0.10 mole NaOH 40.0 g NaOH 2) 500. mL x 1 L _ = 0.500 L 1000 mL 3. 0.10 mole NaOH = 0.20 mole NaOH 0.500 L 1 L = 0.20 M NaOH

33. 32 Learning Check A KOH solution with a volume of 400 mL contains 2 mole KOH. What is the molarity of the solution? 1) 8 M 2) 5 M 3) 2 M Drano

34. 33 Solutions A KOH solution with a volume of 400 mL contains 2 moles of KOH. What is the molarity of the solution? 2) 5 M M = 2 mole KOH = 5 M 0.4 L Drano

35. 34 Learning Check A glucose solution with a volume of 2.0 L contains 72 g glucose (C 6 H 12 O 6 ). If glucose has a molar mass of 180. g/mole, what is the molarity of the glucose solution? 1)0.20 M 2)5.0 M 3)36 M

36. 35 Solution A glucose solution with a volume of 2.0 L contains 72 g glucose (C 6 H 12 O 6 ). If glucose has a molar mass of 180. g/mole, what is the molarity of the glucose solution? 1)72 g x 1 mole x 1 = 0.20 M 180. g 2.0 L

37. 36 Molarity Conversion Factors A solution is a 3.0 M NaOH.. Write the molarity in the form of conversion factors. 3.0 moles NaOH and 1 L NaOH soln 1 L NaOH soln 3.0 moles NaOH

38. 37 Learning Check Stomach acid is a 0.10 M HCl solution. How many moles of HCl are in 1500 mL of stomach acid solution? 1) 15 moles HCl 2) 1.5 moles HCl 3) 0.15 moles HCl

39. 38 Solution 3) 1500 mL x 1 L = 1.5 L 1000 mL 1.5 L x 0.10 mole HCl = 0.15 mole HCl 1 L (Molarity factor)

40. 39 Learning Check How many grams of KCl are present in 2.5 L of 0.50 M KCl? 1) 1.3 g 2) 5.0 g 3) 93 g

41. 40 Solution M4 3) 2.5 L x 0.50 mole x 74.6 g KCl = 93 g KCl 1 L 1 mole KCl

42. 41 Learning Check How many milliliters of stomach acid, which is 0.10 M HCl, contain 0.15 mole HCl? 1) 150 mL 2) 1500 mL 3) 5000 mL

43. 42 Solution 2) 0.15 mole HCl x 1 L soln x 1000 mL 0.10 mole HCl 1 L (Molarity inverted) = 1500 mL HCl

44. 43 Learning Check How many grams of NaOH are required to prepare 400. mL of 3.0 M NaOH solution? 1)12 g 2)48 g 3) 300 g

45. 44 Solution 2) 400. mL x 1 L = 0.400 L 1000 mL 0.400 L x 3.0 mole NaOH x 40.0 g NaOH 1 L1 mole NaOH (molar mass) = 48 g NaOH

46. AmountVolumeConcentration 12mol100L 6mol5.0L 1.2mol0.100molL -1 0.0023mol4.30molL -1 300mL0.632molL -1 100mL8molL -1 1.25mol20L 0.010mol0.38L Learning Check

47. ChemicalMolar mass MassAmountVolumeConcentration NaCl 100g1.00L HCl 5.00g1.33L HNO 3 1.20mol3.00molL -1 NaOH 2.00mol0.101molL -1 Ca(OH) 2 1.32kg500mL K 2 Cr 2 O 7 100mg20mL KMnO 4 20g6.00x10 - 2 mol 1.00molL -1 Na 2 S 2 O 3 0.38g1.22x10 -4 mol 0.225molL -1 Learning Check