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CH110 Chapter 8: Solutions

CH110 Chapter 8: Solutions. Types & Formation of Solutions Solubility Electrolytes Solution Concentration Dilution Colloids & Suspensions Osmosis & Dialysis. Solutions. A solution = A homogeneous mixture components. Sugar in water Saline Oxygen in water Air Dental fillings.

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CH110 Chapter 8: Solutions

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  1. CH110 Chapter 8: Solutions • Types & Formation of Solutions • Solubility • Electrolytes • Solution Concentration • Dilution • Colloids & Suspensions • Osmosis & Dialysis

  2. Solutions • A solution = • A homogeneousmixture components. Sugar in water Saline Oxygen in water Air Dental fillings

  3. Na+ Cl- Na+ Cl- Na+ Cl- Solutions • Solvent : • component in greater amount • (The dissolver) • Water • Alcohol • Solute: • component in lesser amount • (The dissolved) • NaCl • Sugar

  4. Solutions • solute evenly dispersed • always stays mixed • the solute can’t be filtered out • particles are always in motion • volumesnot additive

  5. Gas in Gas Gas in Liquid Liquid in Liquid Solid in Liquid Liquid in Solid (Hg in Ag) Solid in Solid Solutions Gaseous solutions Air, Liquid solutions Soda, Vodka, Saline, • Solid solutions • dental fillings, • 14K gold (58% Au ), • Brass (Zn in Cu), • Steel (C in Fe),

  6. d- d- d- d- O O O O d+ d+ d+ d+ H H H H H H H H d+ d+ d+ d+ Hydrogen Bonding of Water Polar Attraction Hydrogen Bonds

  7. Hydrogen Bonding of Water Hydrogen Bonds

  8. Hydrogen Bonding of Water Frozen H2O: Slow moving molecules H-Bond in patterns

  9. Hydration Polar water attracts to Na+ and Cl- ions “Like Dissolves Like”

  10. + H H O - + H d+ d+ H O d- d- - H - + O d+ d+ H - - - - H H H H H H O O O O O O + + + + H H H H H H Hydration

  11. + H H O - + H H O - H - + O H - - - - - - - - - - - - - - - H H H H H H H H H H H H H H H O O O O O O O O O O O O O O O + + + + + + + + + + + + + + + H H H H H H H H H H H H H H H Hydration

  12. + H H O - + H H O - H - + O H - - - - - - - - - - - H H H H H H H H H H H O O O O O O O O O O O + + + + + + + + + + + H H H H H H H H H H H Hydration

  13. + H H O - + H H O - H - + O H - - - - - - - - - - - - - - - - - - - - - - H H H H H H H H H H H H H H H H H H H H H H O O O O O O O O O O O O O O O O O O O O O O + + + + + + + + + + + + + + + + + + + + + + H H H H H H H H H H H H H H H H H H H H H H Hydration

  14. + + + + + + + + + + + H H H H H H H H H H H H H H H H H H H H H H O O O O O O O O O O O - - - - - - - - - - - + H H O - H - + O H - - - - - H H H H H O O O O O + + + + + H H H H H Hydration

  15. + H H O - + H H O - H - + O H - - - - - - - - - - - - - H H H H H H H H H H H H H O O O O O O O O O O O O O + + + + + + + + + + + + + H H H H H H H H H H H H H Hydration

  16. + + + + + + H H H H H H H H H H H H O O O O O O - - - - - - + H H O - H - + O H - - - - - - - - - - - - - - - - - - - - H H H H H H H H H H H H H H H H H H H H O O O O O O O O O O O O O O O O O O O O + + + + + + + + + + + + + + + + + + + + H H H H H H H H H H H H H H H H H H H H Hydration

  17. + H H O - + H H O - H H H H H H H H H H H - - - - - - - - - - - + + + + + + + + + + + O O O O O O O O O O O H H H H H H H H H H H - - - - - H H H H H O O O O O + + + + + H H H H H Hydration

  18. + H H O - + + + + + + + + + + H H H H H H H H H H H H H H H H H H H H O O O O O O O O O O - - - - - - - - - - H - + O H - - - - - H H H H H O O O O O + + + + + H H H H H Hydration

  19. + H H O - + + + + + H H H H H H H H H H O O O O O - - - - - H H H H H - - - - - + + + + + O O O O O H H H H H - - - - - - - - - H H H H H H H H H O O O O O O O O O + + + + + + + + + H H H H H H H H H Hydration “Like Dissolves Like”

  20. Saturation • Unsaturated: • Can dissolve more. • Saturated • Have dissolved all possible Undissolved Solids in equilibrium w/ dissolved particles

  21. Solubility How muchsolute will dissolve in a solvent grams solute mls solution • Factors affecting solubility • Polarity • Temperature • Pressure

  22. Polarityvs Solubility Like Dissolves Like Polar Attracts Polar Nonpolar Attracts Nonpolar NaCl dissolves in H2O But not in C6H14 Oil dissolves in C6H14 But not in H2O

  23. Temperature vs Solubility Gas NaCl Solubility (g/100ml water) Temperature (oC)

  24. Temperature vs Solubility when T increases T Sol • Gases & mostliquids less soluble Solids more soluble T Sol

  25. T S T S T S Temperature vs Solubility The solubility of a gas in a liquid is inversely related to the temperature . If T goes up Gas solubility goes down (gases escape) Gas Solubility

  26. Temperature vs Solubility Carbonated beveragesbottled cold. Divers with bends often packed in ice for transport to hyperbaric chamber.

  27. Temperature vs Solubility Cold H2O holds more gas than warm H2O If hot rivers lose too much dissolved O2 the fish can’t survive.

  28. P Sol Pressure vs Solubility when P increases • Gases • More soluble Solids & Liquids unaffected Sol P

  29. T P Sol HENRY’S LAW The solubility of a gas in a liquid is directly related to the pressure on the liquid. Gas solubility goes up (more gas will dissolve) If P goes up

  30. T P Sol HENRY’S LAW If P goes down Gas solubility goes down (gases escape) Example: opening a soda. Soda under high pressure Soda under low pressure

  31. The “Bends” Lower P Less dissolved gases Quick ascent Get bubbles in blood & joints  extreme pain High P Lots of dissolved N2

  32. The “Bends” Lower P N2accumulates in brain, spinal cord, and peripheral nerves. Bubbles here can cause paralysis and convulsions. Effects often irreversible. Less dissolved gases High P Lots of dissolved gases

  33. C6H12O6 NaCl C6H12O6 Cl- Na+ C6H12O6 Na+ Cl- Electrolytes Ionic Covalent No Ions Dissolved Ions NaCl  Na+ + Cl-

  34. NaCl HF F1- HF Cl- Na+ H+ H+ F1- Na+ Cl- HF Electrolytes Ionic Weak Strong Lots of Ions Only a few Ions NaCl  Na+ + Cl- HF  H+ + F-

  35. NaCl Cl- Na+ Na+ Cl- Electrolytes in Blood Serum Electrolytes Eq/mol sodium Na1+ 1 potassium K1+ 1 calcium Ca2+ 2 magnesium Mg2+ 2 chloride Cl1- 1 Sulfate SO42- 2 Phosphate PO43- 3 Equivalent = mols of charge Liter

  36. NaCl Cl- Na+ Na+ Cl- Electrolytes in Blood • Serum Electrolytes meq/l • sodium Na1+ 135 - 145 • potassium K1+ 3.5 - 5.0 • calcium Ca2+ 4.5 - 5.5 • magnesium Mg2+ 1.5 - 2.5 • chloride Cl1- 95 - 105 • bicarbonate, HCO31- • venous 19 - 25 • arterial 22 - 26 1000 mEq = 1 Eq

  37. Concentration of solutions How much solute is in a solution • Percent = % mass percent = m/m % mass = # g solute 100 g solution Volume percent = v/v % volume =# ml solute 100 ml solution mass percent = m/v % volume = # g solute 100 ml solution • Molarity = M

  38. Concentration of solutions How much solute is in a solution • Percent = % • Molarity = M • # mol solute = M • 1 L solution

  39. Mass/Volume % If 5 grams of NaCl is dissolved in water to make 200 ml of solution, what is the concentration? 5 g NaCl 200 ml sln x 100 100 = # g solute 100 ml solution 2.5 =2.5 m % v Mass solute x 100 = m/v % Total Volume Part x 100 = % Whole Saline is a 0.9 m % solution of NaCl in water. v

  40. % as Conversion Factor • How many grams of glucose does it take to make 2.00 L of a 5% m/v Glucose solution. = g Glu 2.00 L sln 1000 mL sln 1 L sln 5 g Glc 100 mL sln 100 5 g Glu 100 mL sln 100 mL sln 5 g Glu or

  41. Molarity M = moles solute = mol liters of solution L A 1 Mglucose solution contains the same # molecules as 1 M ethanol. [ ] = special symbol which means mols L

  42. Molarity • Calculate the molarity of a 2.0 L solution that contains 10 moles of NaOH. M = moles solute = mol liters of solution L MNaOH = 10 mol NaOH 2.0 L = 5 M NaOH

  43. Molarity What’s the molarity of a solution that has 18.23 g HCl in 2 liters? • 1 mol HCl • g HCl 18.23 g HCl 2 L sln = # mol solute liters of sln 0.25 = 0.25 M • 36.46 FW of HCl = 1 H x 1.008 + 1 Cl x 35.45 36.46 g/mol

  44. Solution preparation • Solutions are typically prepared in 2 ways: • mixing the proper amount of solute and solvent. • dilution of a concentrated solution.

  45. Making a solution Prepare 100 ml of a 0.5 M solution of sodium chloride. • How many g’s of NaCl do you need to weigh out? 100 ml sln 1 L sln 1000 ml sln 0.5 mol NaCl 1 L sln 58.44 g NaCl 1 mol NaCl = grams NaCl 2.922 0.5 mol NaCl 1 L sln 1 L sln 0.5 mol NaCl or

  46. Making a solution Prepare 100 ml of a 0.5 M solution of sodium chloride. • To make the solution: Weigh out 2.922 gramsNaCl and transfer to a volumetric flask. Fill flask about 1/3 of the way with water and gently swirl until the salt dissolves. Dilute exactly to the mark, cap and mix.

  47. Dilution moles in soln 1 = moles in soln 2 C1V1 = C2V2

  48. Dilution C1V1 = C2V2 What is the concentration of a solution produced by diluting 100.0 ml of 1.5 M NaOH to 2.000 liters? • C1 = 1.5 MC2 = ? • V1 = 100.0 mlV2 = 2000 ml C2 = C1V1 V2 • C2 = (1.5 M) (100.0 ml) = 0.075 M • (2000. ml)

  49. Colloids & Suspensions • Colloid: Homogeneous mix • But not a solution. Particles larger (10-7 to 10-5 cm) than in a sln (<10-7 cm). But still don’t settle out. Suspension: Heterogeneous mix Large particles may settle out & can be filtered.

  50. Liquid dispersed in Gas = Aerosol Solid in Gas = Aerosol Gas in Liq = foam Liquid in Liquid = emulsion Solid in Liquid = sol Gas in Solid = foam Liquid in Solid = Gel Solid in Solid = solid sol Colloids • Gaseous Medium • Fog, • Smoke Liquid Medium Cool whip, milk, paint,blood • Solid Medium • Styrofoam • Jelly,Opals • Pearls, • Concrete

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