Non-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsHenry'sLawSgas =K xPgasMolarityMol/LPart bymass(Masssolute/masssolution) xmultiplicationfactorDissolvesanothersubstanceSolventLatticeenergyAttractiveforcesbetweenionsVan'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedSolutionformsWhen solvent-solute > or =solvent-solvent andsolute-soluteColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleAmount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressureSolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  Heat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterallowssolvent, butnot solute, toflow throughit.SemipermeablemembraneDelta Hof MixExothermicLikedissolves_____Likepi=mrtOsmoticpressureequationVaries withtemperatureandpressureThe solubilityof onesubstance inanotherDissolvesin asubstanceSoluteMolefractionAmountsolute(mol)/masssolvent (kg)LessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.Alwayssoluble inoneanotherGassesFreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. Idealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. moles ofparticles insolution/molesof formula unitsdissolvedi=Delta HofsoluteEndothermicMolalityMol/KgMolepercentAmountsolute(mol)/totalamount(mol) x 100Raoult'sLawPsolution =molfraction(solv.)x P puresolventNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsHenry'sLawSgas =K xPgasMolarityMol/LPart bymass(Masssolute/masssolution) xmultiplicationfactorDissolvesanothersubstanceSolventLatticeenergyAttractiveforcesbetweenionsVan'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedSolutionformsWhen solvent-solute > or =solvent-solvent andsolute-soluteColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleAmount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressureSolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  Heat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterallowssolvent, butnot solute, toflow throughit.SemipermeablemembraneDelta Hof MixExothermicLikedissolves_____Likepi=mrtOsmoticpressureequationVaries withtemperatureandpressureThe solubilityof onesubstance inanotherDissolvesin asubstanceSoluteMolefractionAmountsolute(mol)/masssolvent (kg)LessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.Alwayssoluble inoneanotherGassesFreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. Idealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. moles ofparticles insolution/molesof formula unitsdissolvedi=Delta HofsoluteEndothermicMolalityMol/KgMolepercentAmountsolute(mol)/totalamount(mol) x 100Raoult'sLawPsolution =molfraction(solv.)x P puresolvent

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