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Definition
| A homogenous mixture of two or more substances in a single physical state. |
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| a mixture characterized by visibly different parts. |
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| a mixture that does not have visibly distinguishable parts. |
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| substance that does the dissolving. |
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| the substance that is dissolved. |
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| Capable of being dissolved. |
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| incapable of being dissolved. |
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| Solid solutions that contain two or more metals. Formed by melting the component metals together, mixing them together, and then allowing them to cool. |
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| all mixtures of gases, including the air we breathe. |
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Definition
| the solvent and solution are liquids. the solute may be a gas, liquid, or solid. |
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Definition
| Pairs of liquids that can mix in any amount. |
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| liquids that can not mix in any proportions. |
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| solutions with water as the solvent. |
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Definition
| A substance that dissolves in water to form a solution that conducts an electric current, like sodium chloride. |
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Definition
| A substance that dissolves in water to give a solution that does not conduct electricity, like sugar. |
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Term
| concentration of a solution |
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Definition
| the amount of solute in a given amount of solvent or solution. |
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Definition
| moles of solute/liters of solution |
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Definition
| moles of solute/kilograms of solvent |
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Term
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Definition
| moles of component/total moles of solution |
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Definition
| A solution is saturated if it contains as much solute as can possible be dissolved under the existing conditions of temperature and pressure. |
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Definition
| A solution that has less than the maximum amount of solute that can be dissolved. |
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| A solution that contains a greater amount of solute than that needed to form a saturated solution. |
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Definition
| The interaction between solute and solvent particles. |
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| Solvation when the solvent is water. |
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Definition
| The separation of solute particles from one another and of solvent particles from one another are energy absorbing processes. |
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Definition
| The formation of attractions between solute and solvent particles is an energy releasing process. |
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Definition
| the amount of solute that will dissolve in a specific solvent under given conditions. |
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Term
| polar solute w/ polar solvent |
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Definition
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Term
| polar solute w/ nonpolar solvent |
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Definition
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| nonpolar solute w/ polar solvent |
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Definition
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| nonpolar solute w/ nonpolar solvent |
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Definition
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| ionic solute with polar solvent |
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Definition
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| ionic solute with nonpolar solvent |
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Definition
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Definition
| Similar substances dissolve in each other. |
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Term
| As temperature increases, the __________ of a solute gas becomes __________. |
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Definition
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Term
| as temperature increases, the solubility of a gas in a liquid ________ |
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Definition
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Term
| as temperature increases, the solubility of a solid in a liquid ________ |
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Definition
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Term
| the solubility of a gas in any solvent is increases as the pressure of the gas over the solvent ______ |
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Definition
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Term
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Definition
| The solubility of a gas is proportional to the partial pressure of the gas above the liquid. |
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Term
| 3 factors that affect the rate at which a solid solute dissolves in a solution: |
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Definition
| surface area, stirring, temperature |
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Term
| if the surface area of a solid solute is _______, it dissolves faster. |
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Definition
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Term
| If a solid solute is stirred into the liquid solvent, the rate of dissolving _______. |
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Definition
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Term
| Raising the temperature of a solvent _______ the rate at which a solid solute dissolves. |
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Definition
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Definition
| Properties that are dependent upon the concentration of solute particles, but are independent of their nature. |
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Term
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Definition
| the pressure of a vapor over a solvent is reduced when a nonvolatile solute is dissolved in the solvent. directly related to the concentration of a solution. |
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Definition
| the amount by which the boiling temperature is raised by the addition of a nonvolatile solute. |
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Term
| freezing point depression |
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Definition
| the ability of a dissolved solute to lower the freezing point of its solution. |
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Definition
| A net flow of solvent molecules from the less concentrated solution to the more concentrated solution. |
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| the pressure required to prevent osmosis. |
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