MolepercentAmountsolute(mol)/totalamount(mol) x 100SolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  Henry'sLawSgas =K xPgasDelta HofsoluteEndothermicallowssolvent, butnot solute, toflow throughit.SemipermeablemembraneLatticeenergyAttractiveforcesbetweenionsDissolvesanothersubstanceSolventDelta Hof MixExothermicMolarityMol/LVan'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedRaoult'sLawPsolution =molfraction(solv.)x P puresolventPart bymass(Masssolute/masssolution) xmultiplicationfactorAlwayssoluble inoneanotherGassesSolutionformsWhen solvent-solute > or =solvent-solvent andsolute-solutepi=mrtOsmoticpressureequationAmount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressureHeat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterMolalityMol/KgColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleVaries withtemperatureandpressureThe solubilityof onesubstance inanothermoles ofparticles insolution/molesof formula unitsdissolvedi=MolefractionAmountsolute(mol)/masssolvent (kg)Idealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. LessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.FreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. Dissolvesin asubstanceSoluteNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsLikedissolves_____LikeMolepercentAmountsolute(mol)/totalamount(mol) x 100SolutionmayformSolvent–soluteinteractions <Solvent–solventand solute–soluteinteractions  Henry'sLawSgas =K xPgasDelta HofsoluteEndothermicallowssolvent, butnot solute, toflow throughit.SemipermeablemembraneLatticeenergyAttractiveforcesbetweenionsDissolvesanothersubstanceSolventDelta Hof MixExothermicMolarityMol/LVan'tHoffFactorthe ratio ofmoles of soluteparticles tomoles of formulaunits dissolvedRaoult'sLawPsolution =molfraction(solv.)x P puresolventPart bymass(Masssolute/masssolution) xmultiplicationfactorAlwayssoluble inoneanotherGassesSolutionformsWhen solvent-solute > or =solvent-solvent andsolute-solutepi=mrtOsmoticpressureequationAmount ofpressureneeded to keeposmotic flowfrom takingplaceOsmoticPressureHeat ofHydrationHeat releasedwhen 1 mol ofgas ions isdissolved intowaterMolalityMol/KgColligativepropertiesProperties who'svalues dependonly on thenumber of soluteparticles and noton the type ofparticleVaries withtemperatureandpressureThe solubilityof onesubstance inanothermoles ofparticles insolution/molesof formula unitsdissolvedi=MolefractionAmountsolute(mol)/masssolvent (kg)Idealformation of solute–solvent interactionsare equal to the sumof the broken solute–solute and solvent–solvent interactions. LessThe vapor pressureof the solvent insolution will alwaysbe _____ than thevapor pressure ofthe pure solvent.FreezingPointDepressionFreezing point ofa solution islower than thefreezing point ofthe pure solvent. Dissolvesin asubstanceSoluteNon-Idealsolute–solventinteractions arestronger orweaker than thebrokeninteractionsLikedissolves_____Like

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