LatticeenergyAttractiveforcesbetweenionsVan'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedMolepercentAmountsolute(mol)/totalamount(mol) x 100allowssolvent, butnot solute, toflow throughit.SemipermeablemembraneColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleRaoult'sLawPsolution =molfraction(solv.)x P puresolventAmount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressureDissolvesin asubstanceSoluteSolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  Part bymass(Masssolute/masssolution) xmultiplicationfactorFreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. Heat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterLessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.Varies withtemperatureandpressureThe solubilityof onesubstance inanotherDelta Hof MixExothermicMolalityMol/KgAlwayssoluble inoneanotherGassesNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsDelta HofsoluteEndothermicMolefractionAmountsolute(mol)/masssolvent (kg)Idealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. MolarityMol/LDissolvesanothersubstanceSolventHenry'sLawSgas =K xPgasLikedissolves_____Likepi=mrtOsmoticpressureequationSolutionformsWhen solvent-solute > or =solvent-solvent andsolute-solutemoles ofparticles insolution/molesof formula unitsdissolvedi=LatticeenergyAttractiveforcesbetweenionsVan'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedMolepercentAmountsolute(mol)/totalamount(mol) x 100allowssolvent, butnot solute, toflow throughit.SemipermeablemembraneColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleRaoult'sLawPsolution =molfraction(solv.)x P puresolventAmount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressureDissolvesin asubstanceSoluteSolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  Part bymass(Masssolute/masssolution) xmultiplicationfactorFreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. Heat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterLessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.Varies withtemperatureandpressureThe solubilityof onesubstance inanotherDelta Hof MixExothermicMolalityMol/KgAlwayssoluble inoneanotherGassesNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsDelta HofsoluteEndothermicMolefractionAmountsolute(mol)/masssolvent (kg)Idealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. MolarityMol/LDissolvesanothersubstanceSolventHenry'sLawSgas =K xPgasLikedissolves_____Likepi=mrtOsmoticpressureequationSolutionformsWhen solvent-solute > or =solvent-solvent andsolute-solutemoles ofparticles insolution/molesof formula unitsdissolvedi=

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