LessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.Van'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedpi=mrtOsmoticpressureequationMolefractionAmountsolute(mol)/masssolvent (kg)Delta HofsoluteEndothermicDissolvesin asubstanceSoluteLatticeenergyAttractiveforcesbetweenionsmoles ofparticles insolution/molesof formula unitsdissolvedi=Idealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. Raoult'sLawPsolution =molfraction(solv.)x P puresolventMolepercentAmountsolute(mol)/totalamount(mol) x 100MolalityMol/KgLikedissolves_____LikeDissolvesanothersubstanceSolventDelta Hof MixExothermicallowssolvent, butnot solute, toflow throughit.SemipermeablemembraneNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsAlwayssoluble inoneanotherGassesColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleSolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  FreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. MolarityMol/LHenry'sLawSgas =K xPgasVaries withtemperatureandpressureThe solubilityof onesubstance inanotherHeat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterPart bymass(Masssolute/masssolution) xmultiplicationfactorSolutionformsWhen solvent-solute > or =solvent-solvent andsolute-soluteAmount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressureLessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.Van'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedpi=mrtOsmoticpressureequationMolefractionAmountsolute(mol)/masssolvent (kg)Delta HofsoluteEndothermicDissolvesin asubstanceSoluteLatticeenergyAttractiveforcesbetweenionsmoles ofparticles insolution/molesof formula unitsdissolvedi=Idealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. Raoult'sLawPsolution =molfraction(solv.)x P puresolventMolepercentAmountsolute(mol)/totalamount(mol) x 100MolalityMol/KgLikedissolves_____LikeDissolvesanothersubstanceSolventDelta Hof MixExothermicallowssolvent, butnot solute, toflow throughit.SemipermeablemembraneNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsAlwayssoluble inoneanotherGassesColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleSolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  FreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. MolarityMol/LHenry'sLawSgas =K xPgasVaries withtemperatureandpressureThe solubilityof onesubstance inanotherHeat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterPart bymass(Masssolute/masssolution) xmultiplicationfactorSolutionformsWhen solvent-solute > or =solvent-solvent andsolute-soluteAmount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressure

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