62. Figure 11.14 p. 536 The Development of Osmotic Pressure pp AP requires you to diagram the change when adding solute to a solvent The effect of adding a solute is to extend the range of a solvent.
63.
64. Figure 11.16 Osmotic Pressure. Net transfer of solvent molecules until hydrostatic pressure equalizes the solvent flow in both directions
SE 11.1 Z5e 514 Molarity = 0.215 M Mass % = 0.990% Mole fraction = 0.00389 Molality - 0.217 m
SE 11.1 Z5e 514 Molarity = 0.101 L Mass % = 0.990% Mole fraction = 0.00389 Molality - 0.217 m
Section 11.2 The Energies of Solution Formation 5e 518
Fig. 11.1 Z5e 519
Rf. Fig. 11-2 Z5e 519
Rf. Z553 #35.
Rf. Z553 #35.
Rf. Z553 #35.
Section 11.3 Factors Affecting Solubility Z5e 522
Bottom diagram shows skeletal structure of soap with nonpolar and polar ends
Z5e 1133 Fig. 23.29.
Z5e 523.
Rf. Fig. 11.5 Z5e 523
Z5e 524 SE 11.4
Z5e 524 SE 11.4
Z5e 524 SE 11.4
Z5e 525.
Rf. Fig. 11.6 Z5e 525 Note: most become more soluble with higher temperature, but note cerium sulfate
Rf. Z5e 526 Warmer water on lakes blocks oxygen getting to older water below and the warmer water contains less oxygen.
Fig. 11.7 Z5e 527
Section 11.4 The Vapor Pressures of Solutions Z5e 538
Z5e 529
This is because the dissolved nonvolatile solute decreases the number of solvent molecules at the surface, and so proportionately lowers the escaping tendency of the solvent molecules. Rf. Z5e 528 and Fig. 11.9
Note: all substances are molecules (so no colligative property problem) Use mole fraction 77 b.
Note: all substances are molecules (so no colligative property problem) Use mole fraction 77 b.
Note: all substances are molecules (so no colligative property problem) Use mole fraction 77 b.
Z5e 532
Z5e 554 # 51. Use density to get number of moles. Then find of liquid pentane & hexane. Then use Raoult’s law to get P in torr of both partial and total pressure. b. Since partial pressure of gas is proportional to number of moles of gas present use mol pentane in vapor/total mol vapor to get See solutions guide p. 267
Z5e 554 # 51. Use density to get number of moles. Then find of liquid pentane & hexane. Then use Raoult’s law to get P in torr of both partial and total pressure. b. Since partial pressure of gas is proportional to number of moles of gas present use mol pentane in vapor/total mol vapor to get See solutions guide p. 267
Use density to get number of moles. Then find of liquid pentane & hexane. Then use Raoult’s law to get P in torr of both partial and total pressure. b. Since partial pressure of gas is proportional to number of moles of gas present use mol pentane in vapor/total mol vapor to get See solutions guide p. 267
Z5e 554 # 51. Use density to get number of moles. Then find of liquid pentane & hexane. Then use Raoult’s law to get P in torr of both partial and total pressure. b. Since partial pressure of gas is proportional to number of moles of gas present use mol pentane in vapor/total mol vapor to get See solutions guide p. 267
Use density to get number of moles. Then find of liquid pentane & hexane. Then use Raoult’s law to get P in torr of both partial and total pressure. b. Since partial pressure of gas is proportional to number of moles of gas present use mol pentane in vapor/total mol vapor to get See solutions guide p. 267
Z5e 532
Z5e 532
Z5e 532 SE 11.6
Z5e 532
Section 11.5 Bp elevation & Fp depression Stays liquid longer because intermolecular forces between solute/solvent help hold the liquid together.
Stays liquid longer (before freezing) because IMF of solute/solution prevents forming orderly crystal
Fig. 11.14 Z5e 536 AP question will require you to diagram the change of addition of a solute to a solvent. The effect of adding a solute is to extend the range of a solvent.
Section 11.6 Osmotic Pressure Z5e 540
Z5e 540 fig. 11.16
Z5e 540 Fig. 11.17
Z5e 546 Section 11.7 Colligative Properties of Electrolyte Solutions
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