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Concentration Units Continued

moles of solute. liters of solution. moles of solute. m =. mass of solvent (kg). M =. Concentration Units Continued. Molarity (M). Molality (m). 12.3. moles of solute. M = molarity =. How many moles of KI are required to make 500. mL of a 2.80 M KI solution?.

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Concentration Units Continued

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  1. moles of solute liters of solution moles of solute m = mass of solvent (kg) M = Concentration Units Continued Molarity(M) Molality(m) 12.3

  2. moles of solute M = molarity = How many moles of KI are required to make 500. mL of a 2.80 M KI solution? liters of solution Solution Stoichiometry The concentration of a solution is the amount of solute present in a given quantity of solvent or solution.

  3. mass of solute Mass %= What is the mass percentage of 2 moles of NaOH dissolved in 358 ml of water? mass of solution Solution Stoichiometry The concentration of a solution is the amount of solute present in a given quantity of solvent or solution. Another way this can be expressed is in mass percentage. X 100

  4. moles of solute m =molality = What is the molality of a solution that has contains 83.05g of KI dissolved in 500ml of water? kg of solvent Solution Stoichiometry The concentration of a solution can also be expressed as the moles of solute per kg of solvent.

  5. moles of solute m= mass of solvent (kg) What is the molality of a solution made from 155g of sodium chloride and 1500g of water? 155g of NaCl = 2.65 mol NaCl 1500g of water = 1.5kg of water 2.65 moles NaCl ____________________ = 1.8m 1.5kg water

  6. Change in Boiling Point Common Applications of Boiling Point Elevation

  7. 12.6

  8. 0 DTf = T f – Tf moles of solute m= mass of solvent (kg) = 3.202 kg solvent 1 mol 62.01 g 478 g x 0 Tf = T f – DTf What is the freezing point of a solution containing 478 g of ethylene glycol (antifreeze) in 3202 g of water? The molar mass of ethylene glycol is 62.01 g. DTf = Kfm Kf water = 1.86 0C/m = 2.41 m DTf = Kfm = 1.86 0C/m x 2.41 m = 4.48 0C = 0.00 0C – 4.48 0C = -4.48 0C 12.6

  9. actual number of particles in soln after dissociation van’t Hoff factor (i) = number of formula units initially dissolved in soln Colligative Properties of Electrolyte Solutions 0.1 m NaCl solution 0.1 m Na+ ions & 0.1 m Cl- ions Colligative properties are properties that depend only on the number of solute particles in solution and not on the nature of the solute particles. 0.1 m NaCl solution 0.2 m ions in solution i should be 1 nonelectrolytes 2 NaCl CaCl2 3 12.7

  10. Change in Freezing Point • Which chemical below would be besttode-ice a frozen street and why? • sand, SiO2 • Rock salt, NaCl • Ice Melt, CaCl2

  11. Freezing Point Depression At what temperature will a 5.4 molal solution of NaCl freeze? Solution ∆TFP = Kf • m • i ∆TFP = (1.86 oC/molal) • 5.4 m • 2 ∆TFP = 20.oC FP = 0 – 20. = -20.oC

  12. Triple point diagram solid liquid gas

  13. Phase diagram

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