CHEM 162 LAB #6 SYNTHESIS OF ASPIRIN
COMPLETE SOLUTION ACTUAL EXAM
PAPER 2026 QUESTIONS WITH ANSWERS
GRADED A+
⩥ Matter. Answer: Anything that has mass + takes up space
Phases: solid, liquid, gas
Condensed phases = solids + liquids
⩥ Intermolecular Forces (IMF). Answer: = Interactions between
molecules/atoms/ions
⩥ Solution. Answer: = Homogenous mixtures of 2+ pure substances
In a solution, the solute is dispersed uniformly throughout the solvent
- Solute = compound(s) in lesser amount
- Solvent = compound in greater amount
E.g. air
,⩥ Ability of substances to form solutions depends on ... ?. Answer: 1)
Natural tendency toward mixing (always favorable):
- Entropy = measure of energy randomization/energy dispersal in a
system
- All things in nature want to be as spread out/disordered as possible
(AKA increase their entropy)
- Solution formed = entropy of system is increased!
2) Intermolecular Forces (depends on solute-solvent interactions):
- Strength of IMF: attractive intermolecular forces are another one of the
big driving forces contributing to solution formation between
solute/solvent molecules.
⩥ Covalent VS Ionic Compounds. Answer: Covalent = generally more
soluble in nonpolar solvents, b/w 2 nonmetallic atoms
Ionic = generally more soluble in polar solvents, b/w 2 atoms with
opposite charge
⩥ Solute-Solvent interactions. Answer: Soluble compound = can mix
homogeneously in all proportions with another compounds
,Insoluble compound = cannot mix homogeneously in all proportions
with another compound
Miscible liquids = mix in all proportions with another liquid
Immiscible liquids = do not mix in one another
Range of solubility for all compounds: stronger the solute-solvent
interaction, greater solubility of a solute in that solvent
*** In order for a solute-solvent interaction to be favorable (soluble with
each other), both must have SIMILAR POLARITY! "LIKE
DISSOLVES LIKE"
⩥ Solute-Solvent Combinations. Answer: Soluble:
- Polar + polar: water, sugar
- Ionic + polar: "Hydration Shells" = solvent interface of any compound
that consists of the solute.
- Non-polar + non-polar: octane
Insoluble:
Non-polar + polar
Ionic + non-polar
, ⩥ Non-Polar Gases in Water. Answer: London dispersion force =
weakest IMF, temporary attractive force when electrons in 2 adjacent
atoms occupy positions that make the atoms form temporary dipoles.
E.g. N2, O2, Ar, Kr in water
*** Larger gas = more soluble it will be in water
Solubility of non-polar gases is VERY low, but solubility will increase
with increasing London dispersion forces!
⩥ Solute-solute interactions (Forming a Solution). Answer: Must be
OVERCOME to DISPERSE PARTICLES when making a solution
These "interactions" could be IMF in covalent compounds, Coulombic
attractions in ionic compounds, metallic bonding in metals, etc.
⩥ Solvent-solvent interactions. Answer: Must be OVERCOME to
MAKE ROOM for the solute (same types of interactions as above)
⩥ Solvent-solute interactions. Answer: Must be LARGE ENOUGH to
COMPENSATE FOR THE ENERGY that must be put into breaking
solute-solute + solvent-solvent interactions (same types of interactions
as above)
COMPLETE SOLUTION ACTUAL EXAM
PAPER 2026 QUESTIONS WITH ANSWERS
GRADED A+
⩥ Matter. Answer: Anything that has mass + takes up space
Phases: solid, liquid, gas
Condensed phases = solids + liquids
⩥ Intermolecular Forces (IMF). Answer: = Interactions between
molecules/atoms/ions
⩥ Solution. Answer: = Homogenous mixtures of 2+ pure substances
In a solution, the solute is dispersed uniformly throughout the solvent
- Solute = compound(s) in lesser amount
- Solvent = compound in greater amount
E.g. air
,⩥ Ability of substances to form solutions depends on ... ?. Answer: 1)
Natural tendency toward mixing (always favorable):
- Entropy = measure of energy randomization/energy dispersal in a
system
- All things in nature want to be as spread out/disordered as possible
(AKA increase their entropy)
- Solution formed = entropy of system is increased!
2) Intermolecular Forces (depends on solute-solvent interactions):
- Strength of IMF: attractive intermolecular forces are another one of the
big driving forces contributing to solution formation between
solute/solvent molecules.
⩥ Covalent VS Ionic Compounds. Answer: Covalent = generally more
soluble in nonpolar solvents, b/w 2 nonmetallic atoms
Ionic = generally more soluble in polar solvents, b/w 2 atoms with
opposite charge
⩥ Solute-Solvent interactions. Answer: Soluble compound = can mix
homogeneously in all proportions with another compounds
,Insoluble compound = cannot mix homogeneously in all proportions
with another compound
Miscible liquids = mix in all proportions with another liquid
Immiscible liquids = do not mix in one another
Range of solubility for all compounds: stronger the solute-solvent
interaction, greater solubility of a solute in that solvent
*** In order for a solute-solvent interaction to be favorable (soluble with
each other), both must have SIMILAR POLARITY! "LIKE
DISSOLVES LIKE"
⩥ Solute-Solvent Combinations. Answer: Soluble:
- Polar + polar: water, sugar
- Ionic + polar: "Hydration Shells" = solvent interface of any compound
that consists of the solute.
- Non-polar + non-polar: octane
Insoluble:
Non-polar + polar
Ionic + non-polar
, ⩥ Non-Polar Gases in Water. Answer: London dispersion force =
weakest IMF, temporary attractive force when electrons in 2 adjacent
atoms occupy positions that make the atoms form temporary dipoles.
E.g. N2, O2, Ar, Kr in water
*** Larger gas = more soluble it will be in water
Solubility of non-polar gases is VERY low, but solubility will increase
with increasing London dispersion forces!
⩥ Solute-solute interactions (Forming a Solution). Answer: Must be
OVERCOME to DISPERSE PARTICLES when making a solution
These "interactions" could be IMF in covalent compounds, Coulombic
attractions in ionic compounds, metallic bonding in metals, etc.
⩥ Solvent-solvent interactions. Answer: Must be OVERCOME to
MAKE ROOM for the solute (same types of interactions as above)
⩥ Solvent-solute interactions. Answer: Must be LARGE ENOUGH to
COMPENSATE FOR THE ENERGY that must be put into breaking
solute-solute + solvent-solvent interactions (same types of interactions
as above)
