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| Homogeneous mixture of two or more compounds in a single phase. |
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| Compound which there is more of in a solution |
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| Compound which there is less of in a solution. |
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| Solutions made of compounds with similar properties. |
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Solute molecules are completely separated by solvent molecules so that they no interaction with one another.
Mole fraction is about one. |
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| Violates properties of both ideal and ideally dilute solutions. |
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Solutions that form with different solvent/solute sizes.
Tyndall Effect: scattering of light through a colloid.
Seperation by coagulation of dialysis (semipermeable membrane). |
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| Ionic compounds are dissolved by... |
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| When ionic compounds are dissolved by polar substances and break apart into their respective cations and anions and they are surrounded by oppositely charged ends of the polar solvent. |
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| The process when several water molecules attach to one side of an ionic compound and are able to overcome the strong ionic bond to break the compound apart. |
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| Something that has been hydrated. |
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| Compounds that form ions in aqueous solutions. |
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| m=moles of solute/volume of solution |
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| m= moles solute/kg solvent |
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| X = moles of solute/total moles of all solutes and solvents |
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| mass solute/total mass solution x 100% |
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| ppm=(mass of solute/total mass solution) x 106 |
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Heat given off when bonds are formed.
Negative HoS gives off heat.
Solution formation has positive entropy. |
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The pressure created by molecules in an open space.
Increases with temperature. |
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| a solute with no vapor pressure. |
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Rault's Law
Vapor Pressure |
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| a solute with vapor pressure. |
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| Solutes tendancy to dissolve in a solvent. |
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| Solute falling out of solution. |
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| When the rate of dissolution and precipitation are equal. |
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The equilibrium constant of a solvation reaction.
Solids and pure liquids are left out.
Ex:
Ba(OH)2(s) ↔Ba2+(aq) + 2OH-(aq)
Ksp=[Ba2+][F-]2
Lowest Ksp is least soluble, first to precipitate. |
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| Disturbance in the equilibrium because of a common ion in the equilibrium expression. |
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