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30 Cards in this Set
- Front
- Back
hydroscopic
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salts taht absorb water from the air
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efflorescence
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to lose water of hydration
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deliquescent
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describes a substance that removes sufficient water from the air to form a solution
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example of something deliquescent
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CaCl2
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water of hydration
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water molecules that are an integral part of a crystal struction
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example of water of hydration structure
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CuSO4 . 5H20
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desicant
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a hydroscopic substance used as a drying agent
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anhydrous
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a salt that has lost its water of hydration
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serial dilutions
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1 M, .1M, .01M, .001M,
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solutions
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homogenous
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suspension
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heterogenous mixture from which the particles settle out upon standing; the particle size is usualy greater than 100 nanometers
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colloid
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heterogenous mixture where the particles are smaller than a suspension but bigger than a solution
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example of colloids
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milk, mayonaise, fog, jelly, paint, helatain,
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5 types of solutions
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1. weak
2. strong 3. saturated 4. unsaturated 5. supersaturated |
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weak solution
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dilute- not much solute
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strong solution
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concentrated
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saturated solution
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holding all the solute that the solvent can
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unsaturated
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holding less solute than the solvent can
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supersaturated
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holding more solute than is normally possible
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two supersaturated solutions
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1. NA acetate
2. NA thiosulfate |
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temp of a fas and solubility
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as the temp of a GAs increase, the solubility decreases
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factors affecting solubility
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nature of the solvent/solute
temp polarity pressure |
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factors affecting the rate of solubility
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agitation/stirring
temp (higher=faster) pressure |
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temp and vapor pressure
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higher temp=higher vapor pressure
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formula for molaRity
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molarity= number of moles
---------------- L of solution |
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formula for molaLity
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molality= number of moles
--------------- i kG solvent |
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difference between molaRity and molaLity
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molarity= affected by temp and press
molality= not affected by temp and press |
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one molal
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one molal= 1 mole
------- 1000 kg solvent |
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colligative properties
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properties of a solution that depend on the number of solute particles, not the type of particles
-the more particles in the solution, the more change in the properties |
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examples of colligative properties
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freezing point, boiling point, vapor pressure
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