Properties of Solutions key terms
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| molarity (M) | moles of solute per kilogram of solvent in a solution.
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| mass percent | the percent by mass of a component of a mixture, or of a given element in a compound.
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| mole fraction | the ratio of the number of moles of a given component in a mixture to the total number of moles in the mixture.
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| molality (m) | the number of moles of solute per kilogram of solvent in a solution.
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| normality | the number of equivalents of a substance dissolved in a liter of solution.
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| enthalpy (heat) of solution | the enthalpy change associated with dissolving a solute in a solvent; the sum of the energies needed to expand both solvent and solute in a solution and the energy released from the solvent-solute reactions.
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| enthalpy (heat) of hydration | the enthalpy change associated with placing gaseous molecules or ions in water; the sum of the energy needed to expand the solvent and the energy released from the solvent-solute interactions.
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| Henry's law | the amount of gas dissolved in a solution is directly proportional to the pressure of the gas above the solution.
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| thermal pollution | the oxygen-depleting effect on lakes and rivers of using water for industrial cooling and returning it to its natural source at a higher temperature.
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| Raoult's law | the vapor pressure of a solution is directly proportional to the mole fraction of solvent present.
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| ideal solution | a solution whose vapor pressure is directly proportional to the mole fraction of solvent present.
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| colligative properties | properties of a solution that depend only on the number, and not on the identity, of the solute particles (concentration).
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| molal boiling-point elevation constant | a constant characteristic of a particular solvent that gives the change in boiling point as a function of solution molality; used in molecular weight determinations.
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| molal freezing-point depression constant | a constant characteristic of a particular solvent that gives the change in freezing point as a function of the solution molality; used in molecular weight determinations.
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| semipermeable membrane | a membrane that allows solvent but not solute molecules to pass through.
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| osmosis | the flow of solvent into a solution through a semipermeable membrane.
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| osmotic pressure (pi) | the pressure that must be applied to stop osmosis.
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| dialysis | a phenomenon in which a semipermeable membrane allows transfer of both solvent molecules and small solute molecules and ions.
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| isotonic solutions | solutions having identical osmotic pressures.
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| reverse osmosis | the process occurring when the external pressure on a solution causes a net flow of solvent through a semipermeable membrane from the solution of to the solvent.
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| desalination | the removal of dissolved salts from an aqueous solutions.
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| van't Hoff factor | the ratio of moles of particles in solution to moles of solute dissolved.
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| ion pairing | a phenomenon occurring in solution when oppositely charged ions aggregate and behave as a single particle.
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| Tyndall effect | the scattering of light by particles in a suspension.
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| colloid (colloidal dispersion) | a suspension of particles in a dispersing medium.
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| coagulation | the deduction of a colloid by causing particles to aggregate and settle out.
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