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Learn about soluble, insoluble, saturated, unsaturated solutions, and colligative properties in Chapter 15. Understand electrolytes and nonelectrolytes. Practice molarity calculations and dilutions to grasp solution concepts clearly.

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  1. Soluble Insoluble Saturated solution Unsaturated solution Supersaturated solution Concentration Molarity Dilution Terms

  2. Chapter 15 SOLUTIONS

  3. Aqueous Solutions Some solutions contain ELECTROLYTES HCl, MgCl2, and NaCl are strong electrolytes. - dissociate completely into ions. weak electrolytes. - dissociate a little into ions.

  4. Aqueous Solutions Some compounds dissolve in water but do not conduct electricity. They are called: nonelectrolytes. Examples include: sugar ethanol ethylene glycol

  5. Colligative Properties depend on the concentration of particles in a solution, not of the identity of the particles. • Boiling Point Elevation • Freezing Point Depression • Osmotic Pressure

  6. Freezing Point Depression Each mole of solute particles lowers the freezing point of 1 kilogram of water by 1.86 degrees Celsius. Boiling Point Elevation Each mole of nonvolatile solute particles raises the boiling point of 1 kilogram of water by 0.51 degrees Celsius.

  7. Test each sample to see if it is a strong electrolyte, weak electrolyte, or nonelectrolyte. Electrolyte or Nonelectrolyte!

  8. Parts of a Solution • SOLUTE –part that is being dissolved • SOLVENT – part that dissolves the solute • Solute + Solvent = Solution

  9. H H H H O O O H H H H O O H H O O H H H H H H O H O H How Salts dissolve

  10. Dissolving and Solutions

  11. Saturated Solubility curve Supersaturated Unsaturated

  12. Solubility curve • Any point on a line represents a saturated solution. • In a saturated solution, the solvent contains the maximum amount of solute. • Example 

  13. Solubility curve • Any point below a line represents an unsaturated solution. • In an unsaturated solution, the solvent contains less than the maximum amount of solute. • Example 

  14. Solubility curve • Any point above a line represents a supersaturated solution. • In a supersaturated solution, the solvent contains more than the max solute. • It is unstable • Temporary • accomplished in one of two ways: • Warm the solution • Evaporate some of the solvent • Example 

  15. Solubility curve Any solution can be made saturated, unsaturated, or supersaturated by changing the temperature.

  16. Solubility Curve Determine if each of the following is unsaturated, saturated, or supersaturated. • 55g of NH3 at 20oC._________ • 80g of NaNO3 at 10oC. _________ • 10g of Ce2(SO4)3 at 10oC_________ • 145g of NaNO3 at 80oC. _________ • 25g of KNO3 at 60oC. _________ • 35g of NaCl at 100oC. _________ • 65g of NH4Cl at 80oC. _____________ • 12g of NH3 at 90oC. ______________

  17. The concentration of a solution tells you how much solute that is dissolved in a given amount of solvent (water). The molarity is the concentration of a solution. Molarity = Moles Liter 1. 2.255 moles of NaCl is dissolved in 4.0 L of water, calculate the molarity. Molarity = = 0.56 moles/liter = 0.56 M(Molar) where M means moles per 1 liter

  18. 2.5.00 g KOH is dissolved in 250. mL of water, calculate the molarity. Molarity = = 0.356 M

  19. USING MOLARITY What mass of oxalic acid, H2C2O4, is required to make 250. mL of a 0.0500 M solution? Step 1: Change mL to L. = 0.250 L Step 2: Calculate Moles = 0.0125 moles Step 3: Convert moles to grams. = 1.13 g moles = M•V

  20. Molarity Practice • What is the molarity of an aqueous solution containing 40.0 g of glucose (C6H12O6) in 1.5 mL of solution? • What is the molarity of bleach solution containing 9.5 g of NaOCl per liter of bleach?

  21. 3. How many moles are there in 205. mL of a 0.172 M solution? 0.0353 moles

  22. 4. How many gramsNaCl are there in 250.0 mL of 0.500 M solution? 7.31 g

  23. Dilutions

  24. Diluting Solutions Concentrated solutions have a relatively high molarity. Dilute solutions have a relatively low molarity. M1V1 = M2V2 M1= the initial molarityM2 = the final molarity V1 =the initial volumeV2 = the final volume

  25. water NaCl(aq) NaCl(aq) Concentrated solution Diluted solution

  26. Initial Solution 1. 25.0 mL of 0.10 M solution is diluted by adding 75.0 mL of water. Calculate the molarityof the new solution. M1V1 = M2V2 25.0 mL + 75.0 mL M2 = ? M1= 0.10 M V2 = 100.0 mL V1 =25.0 mL (0.10 M)(25.0 mL) = M2(100.0 mL) M2 = 0.025 M

  27. Initial Solution • What volume of 0.250 M CoCl2 solution can be diluted to 100.0 mL in order to make a 0.0150 M solution? M1V1 = M2V2 M2 = 0.0150 M M1= 0.250 M V2 = 100.0 mL V1 = ? (0.250 M) V1 = (0.0150 M)(100.0 mL) V1 =6.00 mL

  28. Initial Solution 3. 50.0 mL of 0.500 M CuSO4 solution is diluted to 250.0 mL. Calculate the new concentration and the number of grams CuSO4 in the new solution. M1V1 = M2V2 M1= 0.500 M M2 = ? V2 = 250.0 mL V1 = 50.0 mL (0.500 M)(50.0 mL) = M2(250.0 mL) M2 =0.100 M 159.6 g 0.0500 L 0.500 mol x x = 3.99g 1 L 1 mol

  29. Practice 1) If I add 25 mL of water to 125 mL of a 0.15 M NaOH solution, what will the molarity of the diluted solution be?  2) If I add water to 100 mL of a 0.15 M NaOH solution until the final volume is 150 mL, what will the molarity of the diluted solution be? 3) How much 0.05 M HCl solution can be made by diluting 250 mL of 10 M HCl?

  30. Practice 4) I have 345 mL of a 1.5 M NaCl solution. If I boil the water until the volume of the solution is 250 mL, what will the molarity of the solution be? 5) How much water would I need to add to 500 mL of a 2.4 M KCl solution to make a 1.0 M solution?

  31. Practice • 734 grams of lithium sulfate are dissolved to make 2500. mL of solution. • 6.70 x 10-2 grams of Pb(C2H3O2)4 are dissolved to make 3.50 mL of solution. • 83 grams of sodium hydroxide to 750 mL of water.

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