Varies withtemperatureandpressureThe solubilityof onesubstance inanothermoles ofparticles insolution/molesof formula unitsdissolvedi=Dissolvesin asubstanceSolutepi=mrtOsmoticpressureequationDelta Hof MixExothermicNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsMolarityMol/LRaoult'sLawPsolution =molfraction(solv.)x P puresolventLatticeenergyAttractiveforcesbetweenionsAmount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressureLessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.MolefractionAmountsolute(mol)/masssolvent (kg)Delta HofsoluteEndothermicHeat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterVan'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedAlwayssoluble inoneanotherGassesSolutionformsWhen solvent-solute > or =solvent-solvent andsolute-solutePart bymass(Masssolute/masssolution) xmultiplicationfactorMolepercentAmountsolute(mol)/totalamount(mol) x 100SolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  FreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. Henry'sLawSgas =K xPgasLikedissolves_____LikeIdealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. allowssolvent, butnot solute, toflow throughit.SemipermeablemembraneMolalityMol/KgDissolvesanothersubstanceSolventColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleVaries withtemperatureandpressureThe solubilityof onesubstance inanothermoles ofparticles insolution/molesof formula unitsdissolvedi=Dissolvesin asubstanceSolutepi=mrtOsmoticpressureequationDelta Hof MixExothermicNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsMolarityMol/LRaoult'sLawPsolution =molfraction(solv.)x P puresolventLatticeenergyAttractiveforcesbetweenionsAmount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressureLessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.MolefractionAmountsolute(mol)/masssolvent (kg)Delta HofsoluteEndothermicHeat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterVan'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedAlwayssoluble inoneanotherGassesSolutionformsWhen solvent-solute > or =solvent-solvent andsolute-solutePart bymass(Masssolute/masssolution) xmultiplicationfactorMolepercentAmountsolute(mol)/totalamount(mol) x 100SolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  FreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. Henry'sLawSgas =K xPgasLikedissolves_____LikeIdealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. allowssolvent, butnot solute, toflow throughit.SemipermeablemembraneMolalityMol/KgDissolvesanothersubstanceSolventColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticle

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