pi=mrtOsmoticpressureequationAlwayssoluble inoneanotherGassesLatticeenergyAttractiveforcesbetweenionsmoles ofparticles insolution/molesof formula unitsdissolvedi=Heat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterDelta Hof MixExothermicMolefractionAmountsolute(mol)/masssolvent (kg)DissolvesanothersubstanceSolventDelta HofsoluteEndothermicHenry'sLawSgas =K xPgasVaries withtemperatureandpressureThe solubilityof onesubstance inanotherMolalityMol/KgLikedissolves_____LikeFreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. Raoult'sLawPsolution =molfraction(solv.)x P puresolventMolarityMol/LDissolvesin asubstanceSoluteIdealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. ColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsLessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.Part bymass(Masssolute/masssolution) xmultiplicationfactorAmount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressureSolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  SolutionformsWhen solvent-solute > or =solvent-solvent andsolute-soluteMolepercentAmountsolute(mol)/totalamount(mol) x 100Van'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedallowssolvent, butnot solute, toflow throughit.Semipermeablemembranepi=mrtOsmoticpressureequationAlwayssoluble inoneanotherGassesLatticeenergyAttractiveforcesbetweenionsmoles ofparticles insolution/molesof formula unitsdissolvedi=Heat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterDelta Hof MixExothermicMolefractionAmountsolute(mol)/masssolvent (kg)DissolvesanothersubstanceSolventDelta HofsoluteEndothermicHenry'sLawSgas =K xPgasVaries withtemperatureandpressureThe solubilityof onesubstance inanotherMolalityMol/KgLikedissolves_____LikeFreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. Raoult'sLawPsolution =molfraction(solv.)x P puresolventMolarityMol/LDissolvesin asubstanceSoluteIdealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. ColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsLessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.Part bymass(Masssolute/masssolution) xmultiplicationfactorAmount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressureSolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  SolutionformsWhen solvent-solute > or =solvent-solvent andsolute-soluteMolepercentAmountsolute(mol)/totalamount(mol) x 100Van'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedallowssolvent, butnot solute, toflow throughit.Semipermeablemembrane

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