DissolvesanothersubstanceSolventMolarityMol/LColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleMolefractionAmountsolute(mol)/masssolvent (kg)Dissolvesin asubstanceSoluteNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsVan'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedHenry'sLawSgas =K xPgasRaoult'sLawPsolution =molfraction(solv.)x P puresolventallowssolvent, butnot solute, toflow throughit.SemipermeablemembraneDelta HofsoluteEndothermicVaries withtemperatureandpressureThe solubilityof onesubstance inanotherAlwayssoluble inoneanotherGassesSolutionformsWhen solvent-solute > or =solvent-solvent andsolute-soluteHeat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterIdealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. MolepercentAmountsolute(mol)/totalamount(mol) x 100Delta Hof MixExothermicPart bymass(Masssolute/masssolution) xmultiplicationfactormoles ofparticles insolution/molesof formula unitsdissolvedi=FreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. LatticeenergyAttractiveforcesbetweenionspi=mrtOsmoticpressureequationSolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  Amount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressureLikedissolves_____LikeLessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.MolalityMol/KgDissolvesanothersubstanceSolventMolarityMol/LColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleMolefractionAmountsolute(mol)/masssolvent (kg)Dissolvesin asubstanceSoluteNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsVan'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedHenry'sLawSgas =K xPgasRaoult'sLawPsolution =molfraction(solv.)x P puresolventallowssolvent, butnot solute, toflow throughit.SemipermeablemembraneDelta HofsoluteEndothermicVaries withtemperatureandpressureThe solubilityof onesubstance inanotherAlwayssoluble inoneanotherGassesSolutionformsWhen solvent-solute > or =solvent-solvent andsolute-soluteHeat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterIdealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. MolepercentAmountsolute(mol)/totalamount(mol) x 100Delta Hof MixExothermicPart bymass(Masssolute/masssolution) xmultiplicationfactormoles ofparticles insolution/molesof formula unitsdissolvedi=FreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. LatticeenergyAttractiveforcesbetweenionspi=mrtOsmoticpressureequationSolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  Amount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressureLikedissolves_____LikeLessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.MolalityMol/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. Solvent
    Dissolves another substance
  2. Mol/L
    Molarity
  3. Properties who's values depend only on the number of solute particles and not on the type of particle
    Colligative properties
  4. Amount solute (mol)/mass solvent (kg)
    Mole fraction
  5. Solute
    Dissolves in a substance
  6. solute–solvent interactions are stronger or weaker than the broken interactions
    Non-Ideal
  7. the ratio of moles of solute particles to moles of formula units dissolved
    Van't Hoff Factor
  8. Sgas = K x Pgas
    Henry's Law
  9. Psolution = mol fraction(solv.) x P pure solvent
    Raoult's Law
  10. Semipermeable membrane
    allows solvent, but not solute, to flow through it.
  11. Endothermic
    Delta H of solute
  12. The solubility of one substance in another
    Varies with temperature and pressure
  13. Gasses
    Always soluble in one another
  14. When solvent-solute > or = solvent-solvent and solute-solute
    Solution forms
  15. Heat released when 1 mol of gas ions is dissolved into water
    Heat of Hydration
  16. formation of solute–solvent interactions are equal to the sum of the broken solute–solute and solvent–solvent interactions.
    Ideal
  17. Amount solute (mol)/total amount (mol) x 100
    Mole percent
  18. Exothermic
    Delta H of Mix
  19. (Mass solute/mass solution) x multiplication factor
    Part by mass
  20. i=
    moles of particles in solution/moles of formula units dissolved
  21. Freezing point of a solution is lower than the freezing point of the pure solvent.
    Freezing Point Depression
  22. Attractive forces between ions
    Lattice energy
  23. Osmotic pressure equation
    pi=mrt
  24. Solvent–solute interactions < Solvent–solvent and solute–solute interactions
    Solution may form
  25. Osmotic Pressure
    Amount of pressure needed to keep osmotic flow from taking place
  26. Like
    Like dissolves _____
  27. The vapor pressure of the solvent in solution will always be _____ than the vapor pressure of the pure solvent.
    Less
  28. Mol/Kg
    Molality