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Name & describe each of the 7 crystal structures

Name & describe each of the 7 crystal structures. Solutions. Solution. Homogeneous mixture made up of at least one solute dissolved in the solvent. Solute. Substance being dissolved Portion in lesser molar amount. Solvent. Substance doing the dissolving Portion in greatest molar amount.

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Name & describe each of the 7 crystal structures

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  1. Name & describe each of the 7 crystal structures

  2. Solutions

  3. Solution • Homogeneous mixture made up of at least one solute dissolved in the solvent

  4. Solute • Substance being dissolved • Portion in lesser molar amount

  5. Solvent • Substance doing the dissolving • Portion in greatest molar amount

  6. Colloid • Slightly larger particles • Light passes & particles stay suspended

  7. Suspension • Even larger particles • Particles block or reflect light

  8. Tyndall Effect • Because light reflects off suspended particles, the light ray can be seen from the side

  9. Size Comparison • Solution < Colloid • Colloid < Suspension

  10. Soluble • When one substance (solute) dissolves in another (solvent)

  11. Solubility • The amount of one substance (solute) dissolved in another (solvent)

  12. ConcentratedSolution • A solution with a relatively large amount of solute dissolved

  13. Concentration • The amount of solute dissolved into solution

  14. Dilute Solution • A solution with a relatively small amount of solute dissolved

  15. Saturated Solution • A solution with the maximum amount of solute dissolved in the solution

  16. Unsaturated Solution • A solution with less than the maximum amount of solute dissolved in solution

  17. Supersaturated Solution • A solution with greater than the maximum amount of solute dissolved in solution

  18. Solution Measures • Concentration • Molarity • Molality • Mole Fraction

  19. Percent Solution • Mass of one portion per the total mass, all times 100 % • %soln = ma/mtotal x 100 %

  20. Molarity • Moles of solute per liter of solution • M = molessolute/Lsoln

  21. Molality • Moles of solute per kilogram of solvent • mo = molessolute/kgsolvent

  22. Mole Fraction • Moles of one portion per total number of moles in the solution • X = molesa/molessoln

  23. Calculate the molarity of a 250 mL solution containing 5.0 g NaOH dissolved in water

  24. Drill: Calculate: • mass of NaCl required to make 1.5 L of 2.0 M NaCl:

  25. Calculate the molality of 69 g of C2H5OH dissolved in 500.0 mL of water

  26. Calculate the mole fraction of each portion when 92 g of C2H5OH dissolved in 144 mL of water

  27. Calculate the molality & mole fraction of a solution containing 46 g of C2H5OH dissolved in 1782 mL of water

  28. Colligative Properties • Properties dependent only on the concentration of particles in solution

  29. Examples • Vapor pressure • Boiling & Freezing points • Osmotic pressure

  30. Drill: • Calculate the VP of a solution containing 36 % glucose (C6H12O6) in water at 29oC: • (VPwater = 30.0 mm Hg)

  31. Vapor Pressure • VPsolution = (VPsolvent)(Xsolvent) • X = mole fraction • VP = vapor pressure

  32. Boiling & Freezing DT = imoK DT = change in BP or FP i = ionic activity K = BP or FP constant

  33. Osmotic Pressure p = iMRT p = osmotic pressure i = ionic activity M = Molarity

  34. Calculate the vapor pressure of a solution containing 150 g C5H10O5 in 162 mL of water at 30oC

  35. Calculate BP & FP of 60.0 g of NaOH in 250 mL waterKBP = 0.512oC/moKFP = -1.86oC/mo

  36. Calculate the osmotic pressure of a solution containing 12 g of NaOH dissolved in 250 mL solution at 27oC

  37. Calculate the vapor pressure of a solution containing 120 g C3H7OH in 144 mL of water at its BP.

  38. Calculate the osmotic pressure of a solution containing 12 g of C4H8O4 dissolved in 750 mL solution at 27oC

  39. Clausius-Claperon Eq (T2)(T1) P2 (T2 – T1) P1 Hv= R ln

  40. VPbenzene Temp (oC) 24.5 27 73.5 127Calculate Hv for benzene:

  41. Drill: Calculate BP & FP of 88 g of CO2 in 750 mL waterKBP = 0.512oC/moKFP = -1.86oC/mo

  42. Calculate the osmotic pressure of a solution containing 29.9 g of CoBr3 dissolved in 7500 mL solution at 27oC

  43. Calculate the vapor pressure of a solution containing 12.0 g C3H8O in 14.4 mL of water at its BP.

  44. 180 g C3H8O was dissolved in 180 mL H2O at 27oC making a 1.5 g/mL solution. Calculate X, mo, M, p, VP, BP, & FP.

  45. Drill: Calculate the mass of lead(II)nitrate required to make 250 mL of 0.40 M Pb(NO3)2

  46. 300 g C3H6NF was dissolved in 500 g C6H12O at 27oC making a 0.800 g/mL solution. Calculate X, mo, M, p, VP, BP, & FP.

  47. Calculate the molality of a solution that is 33.1 % by mass Pb(NO3)2

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