Amount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressureLessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.Delta HofsoluteEndothermicHenry'sLawSgas =K xPgasallowssolvent, butnot solute, toflow throughit.SemipermeablemembraneSolutionformsWhen solvent-solute > or =solvent-solvent andsolute-soluteAlwayssoluble inoneanotherGassesPart bymass(Masssolute/masssolution) xmultiplicationfactorMolarityMol/LSolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  moles ofparticles insolution/molesof formula unitsdissolvedi=MolepercentAmountsolute(mol)/totalamount(mol) x 100Likedissolves_____LikeLatticeenergyAttractiveforcesbetweenionspi=mrtOsmoticpressureequationVaries withtemperatureandpressureThe solubilityof onesubstance inanotherRaoult'sLawPsolution =molfraction(solv.)x P puresolventColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsHeat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterIdealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. Dissolvesin asubstanceSoluteDelta Hof MixExothermicMolefractionAmountsolute(mol)/masssolvent (kg)MolalityMol/KgVan'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedDissolvesanothersubstanceSolventFreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. Amount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressureLessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.Delta HofsoluteEndothermicHenry'sLawSgas =K xPgasallowssolvent, butnot solute, toflow throughit.SemipermeablemembraneSolutionformsWhen solvent-solute > or =solvent-solvent andsolute-soluteAlwayssoluble inoneanotherGassesPart bymass(Masssolute/masssolution) xmultiplicationfactorMolarityMol/LSolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  moles ofparticles insolution/molesof formula unitsdissolvedi=MolepercentAmountsolute(mol)/totalamount(mol) x 100Likedissolves_____LikeLatticeenergyAttractiveforcesbetweenionspi=mrtOsmoticpressureequationVaries withtemperatureandpressureThe solubilityof onesubstance inanotherRaoult'sLawPsolution =molfraction(solv.)x P puresolventColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsHeat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterIdealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. Dissolvesin asubstanceSoluteDelta Hof MixExothermicMolefractionAmountsolute(mol)/masssolvent (kg)MolalityMol/KgVan'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedDissolvesanothersubstanceSolventFreezingPointDepressionFreezing 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. Osmotic Pressure
    Amount of pressure needed to keep osmotic flow from taking place
  2. The vapor pressure of the solvent in solution will always be _____ than the vapor pressure of the pure solvent.
    Less
  3. Endothermic
    Delta H of solute
  4. Sgas = K x Pgas
    Henry's Law
  5. Semipermeable membrane
    allows solvent, but not solute, to flow through it.
  6. When solvent-solute > or = solvent-solvent and solute-solute
    Solution forms
  7. Gasses
    Always soluble in one another
  8. (Mass solute/mass solution) x multiplication factor
    Part by mass
  9. Mol/L
    Molarity
  10. Solvent–solute interactions < Solvent–solvent and solute–solute interactions
    Solution may form
  11. i=
    moles of particles in solution/moles of formula units dissolved
  12. Amount solute (mol)/total amount (mol) x 100
    Mole percent
  13. Like
    Like dissolves _____
  14. Attractive forces between ions
    Lattice energy
  15. Osmotic pressure equation
    pi=mrt
  16. The solubility of one substance in another
    Varies with temperature and pressure
  17. Psolution = mol fraction(solv.) x P pure solvent
    Raoult's Law
  18. Properties who's values depend only on the number of solute particles and not on the type of particle
    Colligative properties
  19. solute–solvent interactions are stronger or weaker than the broken interactions
    Non-Ideal
  20. Heat released when 1 mol of gas ions is dissolved into water
    Heat of Hydration
  21. formation of solute–solvent interactions are equal to the sum of the broken solute–solute and solvent–solvent interactions.
    Ideal
  22. Solute
    Dissolves in a substance
  23. Exothermic
    Delta H of Mix
  24. Amount solute (mol)/mass solvent (kg)
    Mole fraction
  25. Mol/Kg
    Molality
  26. the ratio of moles of solute particles to moles of formula units dissolved
    Van't Hoff Factor
  27. Solvent
    Dissolves another substance
  28. Freezing point of a solution is lower than the freezing point of the pure solvent.
    Freezing Point Depression