CONCENTRATIONS & SOLUTIONS Flashcards
c = kP
P is the
pressure of the gas over the solution
Each ion is surrounded by solvent molecules. If the solvent is water, the ions are []
hydrated
Low [] = Low []
Low P = Low C
What are the Intermolecular forces?
Dispersion Forces, H-Bonding, Dipole dipole
contains less solute than the solvent has the capacity to dissolve at a specific temperature.
unsaturated
c = kP
c is the
concentration (M) of the dissolved gas
c = kP
k is a
constant (mol/L*atm) that depends only on temperature
Two substances with similar [] are likely to be soluble in each other.
intermolecular forces
is electrostatically attracted to an O, N, or F atom in another molecule
h-bonding
Factors affecting Solubility
Nature of Solvent, Temperature, pressure
Enthalpy (∆H) changes with each interaction [].
broken or formed
contains the maximum amount of a solute that will dissolve in a given solvent at a specific temperature.
saturated
C2H5OH in H2O
polar molecules are soluble with polar solvents
The solubility of a gas in a liquid is proportional to the pressure of
the gas over the solution
Henry’s law
Nonpolar substances tend to dissolve in []
non polar solvent
are attractive forces between permanent dipoles of two polar molecules
Dipole dipole
occurs when hydrogen atom is bonded to O, N, or F
h-bonding
Type of Force: Relative Strength: Exhibited by
London Dispersion
London Dispersion: Weak: All molecules
present in polar molecules.
Dipole dipole
contains more solute than is present in a saturated solution at a specific temperature.
supersaturated
are very weak interactions due to the momentary changes in electron
density in a molecules.
Dispersion Force
Type of Force: Relative Strength: Exhibited by
Hydrogen Bonding
H-Bonding: Strong: Molecules with O-H, N-H, H-F
ionic compounds are more [] in polar solvents
soluble
High [] = High []
High P = High C
larger dipole moment, larger the forces.
dipole dipole
Solvent molecules [] to surface ions. The ions are [] (surrounded by solvent).
attracted - solvated
Henry’s Law Formula
c = kP
Types of solutions
Saturated, Unsaturated, Supersaturated
Type of Force: Relative Strength: Exhibited by
Dipole dipole
Dipole Dipole: Moderate: Molecules with net dipole
are homogeneous mixtures of two or more pure substances.
Solutions
a substance that is dissolved
in a solvent to produce a
solution.
Solute
Polar substances tend to dissolve in []
polar solvent
Present in covalent molecules.
Dispersion
Factors Affecting Solubility
If the solution process [], then the solubility will be [] with [] temperature
Temperature
releases energy - decreased - increased
Chemists use the axiom “”
like dissolves like
the fraction of a solution in
which the other components
are dissolved.
Solvent
NaCl in H2O or NH3(l)
ionic compounds are more soluble in polar solvents
also known as Van der Waals forces and London dispersion
Dispersion forces
Factors Affecting Solubility
If the solution process [], then the solubility will be [] as the temperature is []
Temperature
absorbs energy - increased - increased
CCl4 in C6H6
non polar molecules are soluble with non polar solvents
