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Part I: Solubility, Factors Affecting Solubility  

Part I: Solubility, Factors Affecting Solubility  . CHM 102 Friday, July 6th. Practice: Solubility and Saturation.

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Part I: Solubility, Factors Affecting Solubility  

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  1. Part I: Solubility, Factors Affecting Solubility   CHM 102 Friday, July 6th

  2. Practice: Solubility and Saturation • If the solubility of sodium acetate is 65 g per 100 mL H2O at 100oC, then will any sodium acetate remain undissolved if we pour 140 g of sodium acetate into 200 mL of water? What is the condition of the solution (saturated….unsaturated)?

  3. Practice: Solubility and Saturation • If the solubility of potassium chloride is 42.1 g per 100 mL H2O at 100oC, then will any sodium acetate remain undissolved if we pour 81 g of sodium acetate into 150 mL of water? What is the condition of the solution (saturated….unsaturated)? How much more (if any) could we dissolve into the solution?

  4. Factors Affecting Solubility • Solute-Solvent Interactions • Pressure Effects (dissolving gases) • Temperature Effects (for both gaseous and solid solutes)

  5. Solute-Solvent Interactions • The formation of solute-solvent interactions is the only exothermic contribution to the heat of solution. • Exothermic (negative DH) values for the solute-solvent interaction term points towards a solution process that is spontaneous. • So the stronger the solute-solvent interactions, the more exothermic the overall solution process will be.

  6. Solute-Solvent Interactions • This idea breaks into the classic “like dissolves like” principle. • Water, the “universal solvent” is really not entirely universal. Water is polar, and will tend to dissolve polar and ionic substances, but will not dissolve nonpolar substances (i.e. oil) readily.

  7. NaCl Dissolves in Water

  8. Example: Water and Alcohol • Do water and alcohol mix? What’s an example? These two liquids are said to be miscible. If they didn’t, they’d be termed imiscible.

  9. Practice: Alcohols and Solvent-Solute Interactions • Which is more soluble in water, ethanol (C2H3OH), butanol (C4H9OH), or hexanol (C6H13OH)? Why?

  10. Pressure Effects • When dissolving a gas in water, Henry’s Law shows that when pressure of a gas above a solution goes up, its solubility in the solution increases: S = k P • S is solubility, k is Henry’s gas constant (which is solute and solvent AND temperature dependent).

  11. Practice: Pressure Effects • What is the solubility of carbon dioxide in coke if the soda is at 25oC and the pressure of CO2 above the solution is 0.025 atm? (henry’s law constant is 3.1*10-2 mol/L*atm) S = k P

  12. More Practice: Pressure Effects • What is the henry’s law constant for CO2 at 298 K when the solubility of carbon dioxide is known to be 0.12 mol/L when the pressure of CO2 above the liquid is 4.0 atm? S = k P

  13. Temperature Effects-Gases • When dissolving gases, the solubility of a gas in a substance tends to go DOWN as the temperature goes up. • Think of a cold soda sitting outside open on a hot day. What happens?

  14. Temperature Effects-Solids • When dissolving solids, the solubility of a solid in a substance tends to go UP as the temperature goes up. • Think of making sweet tea or kool-aid. If you want the sugar buzz of your life, you don’t dissolve sugar in cold water, you dissolve it in HOT water. The solubility of the sugar goes up as the temperature gets hotter.

  15. Part II: Ways of Expressing Concentration CHM 102 Friday, July 6th

  16. Ways of Expressing Concentration • Mass Percentage • Parts-per-million (ppm) • Parts-per-billion (ppb) • Mole Fraction • Molarity • Molality

  17. Mass Percentage • Mass Percentage is just as it sounds. It is the percent of what component you’re interested in compared to the whole: • Practice: What is the mass percent sugar in a 2.07 kg solution with 350 g of sugar in it?

  18. Parts-per-million (and –billion) • Parts-per-million and parts-per-billion are often used for very dilute solutions to express concentration: • If 16.5 mg of NaCl is dissolved in 1.6 kg of water, what is the concentration of NaCl in ppm? ppb?

  19. More Practice: ppm and ppb • What is the ppm of Na+ if 24.2 mg of NaCl is added to 1.78 kg of water? (hint: use mass percentage first!) ppb of Na+?

  20. Mole Fraction • Mole fraction is also just as it sounds. It is the number of moles of what component you’re interested in compared to the total moles: Practice: If you’ve got 73 g of HCl in 162 g of water, what is the mole fraction of HCl in the solution?

  21. Molarity and Molality • Do not get these two mixed up! VERY COMMON MISTAKE! • The following two definitions for molarity and molality should be memorized!!! • Molarity is given in moles of solute per liter of solution. • Molality is given in moles of solute per kilogram of solvent.

  22. Molarity • What is the concentration of sodium carbonate (MW = 106 g/mol) in molarity when 26.5 g Na2CO3(s) is dissolved to a total volume of 2 L? What is the molarity of sodium ions, K+?

  23. Molality What is the concentration of sodium carbonate (MW = 106 g/mol) in molality when 53 g Na2CO3(s) is dissolved in 1896 g of DI water?

  24. Moving Between Concentrations • An aqueous solution of NaCl is 10% sodium chloride by mass. What the concentration of NaCl in molarity? • 50.0 g of sucrose (MW = ) is dissolved in 1375 g of ethanol (MW = , density = 0.79 g/mL). What is the molarity of this solution? What is the mass percent sucrose in the solution?

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