moles ofparticles insolution/molesof formula unitsdissolvedi=pi=mrtOsmoticpressureequationNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsLessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.Amount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressurePart bymass(Masssolute/masssolution) xmultiplicationfactorVaries withtemperatureandpressureThe solubilityof onesubstance inanotherVan'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedHenry'sLawSgas =K xPgasFreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. MolalityMol/KgDelta HofsoluteEndothermicDelta Hof MixExothermicSolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  allowssolvent, butnot solute, toflow throughit.SemipermeablemembraneDissolvesin asubstanceSoluteRaoult'sLawPsolution =molfraction(solv.)x P puresolventLikedissolves_____LikeColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleAlwayssoluble inoneanotherGassesDissolvesanothersubstanceSolventMolepercentAmountsolute(mol)/totalamount(mol) x 100Idealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. SolutionformsWhen solvent-solute > or =solvent-solvent andsolute-soluteLatticeenergyAttractiveforcesbetweenionsHeat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterMolarityMol/LMolefractionAmountsolute(mol)/masssolvent (kg)moles ofparticles insolution/molesof formula unitsdissolvedi=pi=mrtOsmoticpressureequationNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsLessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.Amount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressurePart bymass(Masssolute/masssolution) xmultiplicationfactorVaries withtemperatureandpressureThe solubilityof onesubstance inanotherVan'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedHenry'sLawSgas =K xPgasFreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. MolalityMol/KgDelta HofsoluteEndothermicDelta Hof MixExothermicSolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  allowssolvent, butnot solute, toflow throughit.SemipermeablemembraneDissolvesin asubstanceSoluteRaoult'sLawPsolution =molfraction(solv.)x P puresolventLikedissolves_____LikeColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleAlwayssoluble inoneanotherGassesDissolvesanothersubstanceSolventMolepercentAmountsolute(mol)/totalamount(mol) x 100Idealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. SolutionformsWhen solvent-solute > or =solvent-solvent andsolute-soluteLatticeenergyAttractiveforcesbetweenionsHeat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterMolarityMol/LMolefractionAmountsolute(mol)/masssolvent (kg)

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