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