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solutions
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- 1a mixture of two or more substances in a single phase is called asolution
- 2how many substances must be mixed in order to create a solution?two
- 3the substance in larger amountSOLVENT
- 4the substance in the smallest amount and the one that dissolves or disperses is called theSOLUTE
- 5under which circumstances will a solute dissolve in a solvent?if the solute-solvent forces of attraction are great enough to overcome solute-solvent and solvent-solvent forces of attraction
- 6under which circumstances will a solute NOT dissolve in a solvent?if the solute-solvent forces are weaker than the individual solute and solvent IMF attractions
- 7two liquids that completely dissolve in each other aremiscible
- 8two liquids that are not miscible in each other areimmiscible
- 9what does the physical state of a solvent determinethe physical state of a solution (usually gas or liquid)
- 10if the solute:solvent forces are stronger than the solute:solute then the solution isexothermic
- 11if the solute:solvent forces are weaker than the solute:solute then the solution isweaker
- 12if the solute:solvent forces are much weaker than the solute:solute then the solutionwill not dissolve e
- 13when water is the solvent for a solution created by dissolving an ionic compound or ions, the process is calledhydration
- 14the amount of energy released when 1 mole of an ion is dissolved in a large volume of water to form a very dilute solutionthe heat of hydration
- 15how do ionic compounds dissolveIMF of solvent to solute (ion-dipole) replace the IMF of solute to solute and solvent to solvent
- 16ΔHhydration is alwaysexothermic
- 17If ΔHlattice = ΔHhydration thenthe formation of the solution does NOT have a noticeable change in energy
- 18if ΔHlattice is < ΔHhydration thenthe formation of the solution is exothermic
- 19if ΔHlattice is > ΔHhydration thenthe formation of the solution is endothermic
- 20a measure of randomness or disorder in a systementropy
- 21all gases are _____ soluble in one anotherinsoluble
- 22solid solutions are heterogenous meaningthey do not mix evenly
- 23the maximum amount of a solute that dissolves in a fixed quantity of solvent at a given tempsolubility
- 24when a dynamic equilibrium exists between the solute and solutionsaturated solution
- 25less solute is dissolved than could be dissolved at equilibriumunsaturated solution
- 26a solution that has more particles dissolved than the equilibrium value would allowsupersaturated solution
- 27- very unstable - the slightest disturbance causes recrystallization - usually achieved by heating a solution to allow more solute to dissolve and then cooling the solution quicklysuper saturated solution
- 28how does changing temperature affect the equilibriumshifts the equilibrium
- 29most solids need heat to dissolve this isendothermic
- 30most gases give heat to dissolve this isexothermic
- 31solubility of gases in water decreases astemperature increases
- 32how does pressure affect the solubility of solidsit does NOT because solids are incompressible
- 33solubility of a gas in water increases aspressure increases
- 34Gas = kH * PgasHenry's law
- 35mol solute / volume of solution (L)molarity
- 36mol solute / volume of solventmolality
- 37mass of solute /mass of solutionparts by mass
- 38volume of solute / volume of solutionparts by volume
- 39amount of solute / amount of solute + amount of solventmole fraction
- 40is molarity affected by changes of temperature?yes, because volume changes with temperature
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- Fichas sobre solutions, creado por May Du el 12/12/2021.
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- May Du
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