Chapter 16 Solutions: vocab and key ideas
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
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| What factors affect how fast a substance dissolves? | agitation, temperature and particle size.
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| Agitation affects what? | only the rate at which a substance dissolves.
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| Temperature influences the ___ at which the substance dissolves. | rate
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| What does a saturated solution contain? | the maximum amount of solute for a given quantity of solvent.
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| What is the solubitity of a substance? | the amount of solute that dissolves in a given quantity of solvent at a specified temperature and pressue to produce a saturated solution.
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| How do two liquids become miscible? | if they dissolve completely in each other in all proportions.
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| liquids that are insoluble in one another are called what? | immiscrible
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| What does a super saturated solution contain? | more solute than it can theoretically hold at a given temperature.
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| What does Henry's law state? | at a given temperature, the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid.
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| What is molarity? | yhe number of moles of solute dissolved in one liter of solution.
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| The concentration of a solution is the measure of what? | the amount of solute that is dissolved in a given quantity of solvent.
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| A solution that contains a realatively small amount of solute is known as what? | dilute solution.
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| A concentrated solution contains what? | a large amount of solute.
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| How do you calculate the molarity of a solution? | divide the number of moles by the volume of the solution in liters.
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| What is a colligative property? | a property of solutions that depends only upon the number of solute particles, not upon their identity.
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| What are the three important properties of solutions? | vapor-pressure lowering, freezing-point depression and boiling-point elevation.
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| What is the freezing-point depression? | the difference in temperature between the freezing point of a solution and the freezing point of the pure solvent.
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| Define boiling-point elevation. | the difference in temperature between the boiling point of a solution and the boiling point of the pure solvent.
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