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SOLUTIONS
Chapter 15
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Solution = homogeneous mixture
• Solute = gets dissolved (minor component)• Solvent = dissolving agent (major component)
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A substance that dissolves in a solvent is said to be soluble. These two substances are miscible.
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A substance that does not dissolve in a solvent is insoluble. These two substances are immiscible.
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(See Table 15-1, p.454)
Page 454 in Book
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Water is an excellent solvent. It is the “universal solvent.”Solutions made with water are called
aqueous solutions.
Movie:
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Water is polar and dissolves many ionic and polar substances.
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Solvation = the process of surrounding solute particles with solvent particles to form a solution. Solute particles must separate from one another and the solute and solvent particles must mix.
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Ionic compounds dissolves in waterbecause they have charges (polar).
Animation: Dissolving table salt
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“Like dissolves like.”
• Polar solutes dissolve in polar solvents• Nonpolar solutes dissolve in nonpolar solvents
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Polar covalent compounds dissolve in water; non-polar compounds do not dissolve in water.
Sugar (glucose) is polar and dissolves in water.
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Factors that affect rate of solvation
• Stirring the mixture• Increasing the surface area of the solute• Increasing the temperature of the solvent
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Solubility = maximum amount of solute that will dissolve in a given amount of solvent at a specified
temperature and pressure • Saturated = maximum amount of solute is
dissolved• Unsaturated = more solute can be dissolved• Supersaturated = contains more dissolved
solute than a saturated solution at the same temperature.
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Factors that affect solubility
• Increased Temperature – solubility of solids increases; solubility of gases decreases.
• Increased Pressure – solubility of gases increases. (This process is called aeration)
• Henry’s Law –at a given temperature, the solubility (S) of a gas in a liquid is directly proportional to the pressure (P) of the gas above the liquid.
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Ch.15.2- Solution Concentration• The concentration of a solution is a measure
of how much solute is dissolved in a specific amount of solvent or solution.
solute or solute solvent solution
(solution = solute + solvent)
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Expressing Concentration
• Concentration may be described qualitatively as concentrated or dilute.
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Concentration= solute or solute solvent solution
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Percent by Mass (p.463 #8)
• What is the percent by mass of NaHCO3 in a solution containing 20 g NaHCO3 dissolved in 600 mL H2O?
• Density of H2O = 1.00 g/mL• % by mass = 20 g x 100 = 3.2% 620 g
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Percent by Mass (p.463 #9)
• You have 1500.0 g of a bleach solution. The percent by mass of the solute sodium hypochlorite, NaOCl, is 3.62%. How many grams of NaOCl are in the solution?
• % Mass = mass solute x 100 mass solution 3.62 = x g X 100 1500.0 g x = 54.3 g NaOCl
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Percent by Volume (p.464 #12)
• If you have 100.0 mL of a 30.0% aqueous solution of ethanol, what volumes of ethanol and water are in the solution?
• % Volume = volume of solute x 100% volume of solution 30.0 % = x mL x 100 100.0 mL x = 30 mL ethanol 70 mL water
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Molarity (p.465 #14)
• What is the molarity of an aqueous solution containing 40.0 g of glucose (C6H12O6) in 1.5 L of solution?
• 1 mole C6H12O6 = 180.16 g
• 40.0 g C6H12O6 x 1 mole = 0.222 mol
180.16 g• Molarity = 0.222 mol = 0.15 M C6H12O6
1.5 liter
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Molarity (p.465 #15)
• What is the molarity of a bleach solution containing 9.5 g NaOCl per liter of bleach?
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Molarity (p.465 #16)
• Calculate the molarity of 1.60 L of a solution containing 1.55 g of dissolved KBr.
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Molarity (p.466 #17)
• How many grams of CaCl2 would be dissolved in 1.0 L of a 0.10 M solution of CaCl2?
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Molarity (p.466 #18)
• A liter of 2M NaOH solution contains how many grams of NaOH?
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Molarity (p.466 #19)
• How many grams of CaCl2 should be dissolved in 500.0 mL of water to make a 0.20M solution of CaCl2?
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Molarity (p.466 #20)
• How many grames of NaOH are in 250 mL of a 3.0M NaOH solution?
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Diluting Solutions- p.467
• In the laboratory, you may use concentrated solutions called stock solutions.
• For example, concentrated hydrochloric acid (HCl) is 12 M.
• You can dilute the stock solution by adding more solvent.
• Would you still have the same number of moles of solute particles that were in the stock solution?
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Diluting Solutions- p.467
• Molarity (M) = moles solute liters solution• moles solute = Molarity x liters solution• Because the total number of moles of solute
does not change during dilution,moles solute in stock solution = moles solute after dilution
M1V1 = M2V2
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Diluting Solutions- p.468 #21
• What volume of a 3.00 M KI stock solution would you use to make 0.300 L of a 1.25 M KI solution?
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Diluting Solutions- p.468 #23
• If you dilute 20.0 mL of a 3.5 M solution to make 100.0 mL of solution, what is the molarity of the dilute solution?
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Molality- p.469
• Molality (m) = moles solute = moles solute kilogram solvent 1000 g solvent
• What is the molality of a solution containing 10. 0 g Na2SO4 dissolved in 1000.0 g of water?
• What is the molality of a solution containing 30.0 g of naphthalene dissolved in 500.0g of toluene?
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Mole Fraction- p.470
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Mole Fraction- p.470 #26
• What is the mole fraction of NaOH in an aqueous solution that contains 22.8% NaOH by mass?
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Mole Fraction- p.470 #27
• An aqueous solution of NaCl has a mole fraction of 0.21. What is the mass of NaCl dissolved in 100.0 mL of solution?
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Parts per million (ppm)