Alwayssoluble inoneanotherGassesLessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.LatticeenergyAttractiveforcesbetweenionsallowssolvent, butnot solute, toflow throughit.SemipermeablemembraneHenry'sLawSgas =K xPgasLikedissolves_____LikePart bymass(Masssolute/masssolution) xmultiplicationfactorMolefractionAmountsolute(mol)/masssolvent (kg)Delta HofsoluteEndothermicMolepercentAmountsolute(mol)/totalamount(mol) x 100pi=mrtOsmoticpressureequationMolalityMol/KgVan'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedDissolvesanothersubstanceSolventmoles ofparticles insolution/molesof formula unitsdissolvedi=Varies withtemperatureandpressureThe solubilityof onesubstance inanotherNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsHeat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterAmount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressureMolarityMol/LIdealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. Delta Hof MixExothermicColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleDissolvesin asubstanceSoluteRaoult'sLawPsolution =molfraction(solv.)x P puresolventSolutionformsWhen solvent-solute > or =solvent-solvent andsolute-soluteSolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  FreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. Alwayssoluble inoneanotherGassesLessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.LatticeenergyAttractiveforcesbetweenionsallowssolvent, butnot solute, toflow throughit.SemipermeablemembraneHenry'sLawSgas =K xPgasLikedissolves_____LikePart bymass(Masssolute/masssolution) xmultiplicationfactorMolefractionAmountsolute(mol)/masssolvent (kg)Delta HofsoluteEndothermicMolepercentAmountsolute(mol)/totalamount(mol) x 100pi=mrtOsmoticpressureequationMolalityMol/KgVan'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedDissolvesanothersubstanceSolventmoles ofparticles insolution/molesof formula unitsdissolvedi=Varies withtemperatureandpressureThe solubilityof onesubstance inanotherNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsHeat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterAmount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressureMolarityMol/LIdealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. Delta Hof MixExothermicColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleDissolvesin asubstanceSoluteRaoult'sLawPsolution =molfraction(solv.)x P puresolventSolutionformsWhen solvent-solute > or =solvent-solvent andsolute-soluteSolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  FreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. 

Solubility Bingo - Call List

(Print) Use this randomly generated list as your call list when playing the game. There is no need to say the BINGO column name. Place some kind of mark (like an X, a checkmark, a dot, tally mark, etc) on each cell as you announce it, to keep track. You can also cut out each item, place them in a bag and pull words from the bag.


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  1. Gasses
    Always soluble in one another
  2. The vapor pressure of the solvent in solution will always be _____ than the vapor pressure of the pure solvent.
    Less
  3. Attractive forces between ions
    Lattice energy
  4. Semipermeable membrane
    allows solvent, but not solute, to flow through it.
  5. Sgas = K x Pgas
    Henry's Law
  6. Like
    Like dissolves _____
  7. (Mass solute/mass solution) x multiplication factor
    Part by mass
  8. Amount solute (mol)/mass solvent (kg)
    Mole fraction
  9. Endothermic
    Delta H of solute
  10. Amount solute (mol)/total amount (mol) x 100
    Mole percent
  11. Osmotic pressure equation
    pi=mrt
  12. Mol/Kg
    Molality
  13. the ratio of moles of solute particles to moles of formula units dissolved
    Van't Hoff Factor
  14. Solvent
    Dissolves another substance
  15. i=
    moles of particles in solution/moles of formula units dissolved
  16. The solubility of one substance in another
    Varies with temperature and pressure
  17. solute–solvent interactions are stronger or weaker than the broken interactions
    Non-Ideal
  18. Heat released when 1 mol of gas ions is dissolved into water
    Heat of Hydration
  19. Osmotic Pressure
    Amount of pressure needed to keep osmotic flow from taking place
  20. Mol/L
    Molarity
  21. formation of solute–solvent interactions are equal to the sum of the broken solute–solute and solvent–solvent interactions.
    Ideal
  22. Exothermic
    Delta H of Mix
  23. Properties who's values depend only on the number of solute particles and not on the type of particle
    Colligative properties
  24. Solute
    Dissolves in a substance
  25. Psolution = mol fraction(solv.) x P pure solvent
    Raoult's Law
  26. When solvent-solute > or = solvent-solvent and solute-solute
    Solution forms
  27. Solvent–solute interactions < Solvent–solvent and solute–solute interactions
    Solution may form
  28. Freezing point of a solution is lower than the freezing point of the pure solvent.
    Freezing Point Depression