Lecture 18 Flashcards
Majority component of solution
solvent
Minority component in a solution
solute
Factors affecting solubility
- Temperature
- Pressure (gases)
- Nature of compound
Higher the temperature (solubility)
higher solubility of solid in liquid
Lower temperature (solubility)
Higher solubility of gas in liquid
Pressure and solubility (Gases)
Higher pressure=Higher solubility
Henrys law
Solubility of a gas is directly proportional to its partial pressure. Sg=k * Pg. Solubility of solid not affected by pressure. Solubility of a gas in a liquid increases as they pressure increases.
Classifying solvents water (polar or non polar)
Water (polar) O-H structure
Classifying solvents ethyl alcohol, c2H5OH
polar o-h
classifying solvents, acetone
c3h6o polar c=o
Classifying solvents, Toluene
non polar c-c and c-h c7h8
Classifying solvents, Hexane
C6h14 non polar c-c and c-h
Classifying solvents Diethyl ether
c4h10O, non polar c-c c-h and c-o
Ions are attracted to what solvents?
Polar solvents (polar molecules also attracted to polar solvents). Have either multiple OH groups or a little CH
Solvation definition
When materials dissolve, the solvent molecules surround the solvent particles due to the solvents attractions for the solute. (isolated from each other)
Saturated solutions definition
Maximum amt of solute that will dissolve in that solvent at that temp
Unsaturated definition
Solutions can dissolve more solute
Supersaturated definition
Solutions are holding more solute than they should be able to at that temperature. (unstable)
Solution concentrations -Mass Percent
Parts of solute in every 100 parts solution. Mass percent = Mass of solute, g over Mass of solution, G x 100%
Solution concentrations Molarity
Solution concentrations Molality
Dilute vs concentrated solutions definition (solute)
Dilute= low amounts of solute per amt. of solution and concentrated = high amounts of solute per amount of solution
concentrations example (units)
12% mass by sugar means 12g of sugar in a 100g solution
Electrolytes
substances whose aqueous solution is a conductor of electricity
Strong electrolytes:
All electrolyte molecules are dissociated into ions. Sodium Hydroxide, sodium chloride, hydrochloric acid
Nonelectrolytes:
non of the molecules are dissociated into ions. Sugar, Alcohol, and oil
Weak electrolytes:
Small percentage are dissociated into ions. Water, acetic acid, ammonia.