H Chemistry: Unit 7 Flashcards
solution
homogeneous mixture made of a solute and a solvent
solute
substance being dissolved
solvent
substance dissolving the solute
universal solvent
water
solutions can be
solids, liquids, and gases
solutions made with water are referred to as
aqueous
soluble
solutes ability to dissolve in a solvent
insoluble
inability for a solute to dissolve
miscible
the ability of two liquids to mix together
immiscible
the inability of two liquids to mix together
solvation
process of dissolving; opposite of crystallization
factors that increase solvation
- agitation
- increase the temperature
- increase the surface area of the solute
solvation>crystallization
unsaturated solution
solvation=crystallization
saturated solution
solvation<crystallization
precipitation(solid in solution)
supersaturated solution
solution that contains more solute than a saturated solution; unstable and crystallizes rapidly
how to make a supersaturated solution
- add solute slowly and heat a saturated soln
- stir slowly
- let it cool to room temperature
delta H of solution
change in energy when a solution is formed
solubility
maximum amount of solute that can be dissolved in 100 grams of solvent at STP
factors that affect solubility
- temperature
- pressure
concentration
expression of the ratio of solute to solvent
diluted solution
very little solute to solvent
concentrated solution
a lot of solute compared to solvent(saturated solution)
molarity
M; concentration of miles of solute per liter of solution
stock solution
solution that is concentrated from which diluted solutions can be made
M1V1=
M2V2
solubility rules 1
salts made with Group 1A elements and ammonium are soluble
solubility rules 2
acetates, bicarbonates, chlorates, & nitrates are soluble
solubility rules 3
salts made with Br, Cl, I are soluble except when bound to silver, mercury, or lead
solubility rules 4
sulfates are soluble except when bound to silver, mercury, lead, calcium, strontium, or barium
solubility rules 5
carbonates, chromates, hydroxides, oxides, and phosphates are insoluble except for rule #1
assumptions of ideal gases(5)
- gas particles are in constant random motion
- gas particles do not attract or repel each other
- gas particles are much smaller than the space between them
- gas particles do not lose kinetic energy when they collide with themselves or their container
- gas particles have the same kinetic energy at a given temperature
4 properties if gases
- volume
- pressure
- temperature(K)
- amount(mol)
Charles law
a volume of a specific amount of gas is directly proportional to its kelvin temperature at constant pressure
charles law formula
V1/T1 = V2/T2
Boyles Law
the pressure of a specific amount of gas is inversely related to volume at constant temperature
boyles law formula
P1V1 = P2V2
how many psi in 1 atm
14.7
how many bar in 1 atm
1.01
how many mmHg(torr) in 1 atm
760
how many kPa in 1 atm
101.3
Gay-Lussacs law
the pressure of a specific amount of gas is directly proportional to its Kelvin temperature at constant volume
gay-lussacs law formula
P1/T1 = P2/T2
combined gas law formula
P1V1/T1 = P2V2/T2
combined gas law is used when
only miles are constant and 5 pieces of information are given and you must solve for the 6th; temp must be in K
ideal gas law
used to solve for a property of a gas at a given moment
ideal gas law formula
PV = nRT
ideal gas constant
0.0821(Lxatm)/(molxK)
vapor
gaseous substance that is a liquid or solid at room temperature
vapor pressure
pressure exerted by a vapor; every liquid has vapor pressure; determined by molecular structure and mass
boiling point
temperature at which the vapor pressure is equal to the atmospheric pressure
partial pressure
pressure exerted by a single gas in a mixture
Dalton’s law of partial pressure
the total pressure of a mixture is equal to the sun of the partial pressure of the gases that make up a mixture
diffusion
movement of a gas from high concentration to low concentration
effusion
movement of a gas through a small opening of hole
KE=
1/2 mv^2
the smaller the gas particle
the higher the velocity
grahams law
the rate(velocity) of a gas particle is inversely related to the square root of its molar mass
grahams law formula
Rate a/Rate b = (molar mass a/ molar mass b)^1/2
Avagadros law
the volume at constant pressure is directly proportional to the number of gas particles at a given temperature
avagadros law formula
V1/N1 = V2/N2
standard volume of gas
one mole of gaseous particles at STP occupies 22.4 L of space regardless of identity