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SOLUTION CHEMISTRY EXAM NEWEST VERSION -2025/2026-
100+ QUESTIONS AND VERIFIED ANSWERS 100% CORRECT
GUARANTEED SUCCESS
Crystallization
Process of forming solid crystals from the cooling of a SUPERSATURATED solution
at HIGH temperatures to room temp.
--> Seed req. to form nucleation site for the crystal.
Solid Dissolved in Liquid Example
salt water
Solid Dissolved in Gas Example
Vapour from a mothball
Solubility
(g/mL): MAXIMUM amount of solute that will dissolve in a given quantity of
solvent at a specific TEMPERATURE.
--> Ex. saturated solution of salt in water is 36g per 100mL of water.
3 Levels of Solubility
1. Insoluble: less than 0.10g of solute will dissolve in 100 mL of solvent.
2. Slightly Soluble: 0.10-1g of solute will dissolve in 100 mL of solvent
3. Soluble: more than 1g will dissolve in 100 mL of solvent
3 Types of Saturation Solutions
1. Unsaturated: More solute dissolves
2. Saturated: no more solute dissolves
3. Supersaturated: Crystals may grow
, 2
Determining Polarity
To be polar:
1. polar covalent bonds (change of EN)
--> ionic: EN >= 1.7
--> polar covalent: 0.5<= EN < 1.7
--> non-polar covalent: 0 <= EN < 0.5
2. net dipole moment (not symmetrical)
"like dissolves like"
-Polar solutes and ionic solutes dissolve in polar solvents (due to dipole-dipole
forces/ion-dipole being formed)
-Nonpolar solutes dissolve in nonpolar solvents due to the lack of dipoles.
--> Applies to gases as well, ex. CO2 is nonpolar (relatively insoluble in water, but
soluble in HCL since it's polar).
-Molecules that contain BOTH nonpolar and polar components (ex., soaps) can
dissolve in BOTH.
--> Soaps dissolve in both grease and water
Hydration
Ions attracted to dipole of water = dissolves by hydration (water molecule
surround the ions of a solute, separating and dispersing them thruout the water).
--> Not all ionic compounds will dissolve in water.
--> Although ions attracted to each other, attraction btwn ions to the dipole of
water is GREATER = ion dipole force (causes ions to pull away from the lattice =
dissolves).
Factors of Ionic Compound Solubility in Water
, 3
1. Larger ionic radius = increases solubility (when larger radii, attraction btwn ions
in ionic compound is weaker due to charges being more farther apart)
2. Greater charge = lower solubility (since more bonds = harder to take apart ions)
Molecular (covalent) Compounds
Dipole-dipole forces hold together the molecules in a polar compound.
--> this force is WEAKER than h-bonds btwn the solute and water = substance
dissolves
-Nonpolar molecular substances = do NOT dissolve in WATER
-Increasing size of non-polar portion of molecule = decreased solubility.
--> Ex. ethanol (larger molecule) vs methanol (smaller)
Dissolving
The BREAKING of INTERmolecular forces of solute particles and becoming
incorporated into solvent particles
--> Ex. Sugar dissolves well in tea
--> rate of dissolving = how quickly solute dissolves in solvent
Intermolecular forces
Van-Der-Wall forces:
1. London dispersion forces (LDF) (all molecular compounds: polar covalent, non-
polar covalent), weakest.
--> only force present in NONPOLAR molecules
2. Dipole-dipole forces (DD) (polar molecules w/ net dipole)
--> Hydrogen bonding (H-Bond) (type of DD force) (btwn H atom and F, O, or N).
Ion-Ion force: strongest intermolecular force only in ionic compounds (opp.
charged ions in ionic compound)
SOLUTION CHEMISTRY EXAM NEWEST VERSION -2025/2026-
100+ QUESTIONS AND VERIFIED ANSWERS 100% CORRECT
GUARANTEED SUCCESS
Crystallization
Process of forming solid crystals from the cooling of a SUPERSATURATED solution
at HIGH temperatures to room temp.
--> Seed req. to form nucleation site for the crystal.
Solid Dissolved in Liquid Example
salt water
Solid Dissolved in Gas Example
Vapour from a mothball
Solubility
(g/mL): MAXIMUM amount of solute that will dissolve in a given quantity of
solvent at a specific TEMPERATURE.
--> Ex. saturated solution of salt in water is 36g per 100mL of water.
3 Levels of Solubility
1. Insoluble: less than 0.10g of solute will dissolve in 100 mL of solvent.
2. Slightly Soluble: 0.10-1g of solute will dissolve in 100 mL of solvent
3. Soluble: more than 1g will dissolve in 100 mL of solvent
3 Types of Saturation Solutions
1. Unsaturated: More solute dissolves
2. Saturated: no more solute dissolves
3. Supersaturated: Crystals may grow
, 2
Determining Polarity
To be polar:
1. polar covalent bonds (change of EN)
--> ionic: EN >= 1.7
--> polar covalent: 0.5<= EN < 1.7
--> non-polar covalent: 0 <= EN < 0.5
2. net dipole moment (not symmetrical)
"like dissolves like"
-Polar solutes and ionic solutes dissolve in polar solvents (due to dipole-dipole
forces/ion-dipole being formed)
-Nonpolar solutes dissolve in nonpolar solvents due to the lack of dipoles.
--> Applies to gases as well, ex. CO2 is nonpolar (relatively insoluble in water, but
soluble in HCL since it's polar).
-Molecules that contain BOTH nonpolar and polar components (ex., soaps) can
dissolve in BOTH.
--> Soaps dissolve in both grease and water
Hydration
Ions attracted to dipole of water = dissolves by hydration (water molecule
surround the ions of a solute, separating and dispersing them thruout the water).
--> Not all ionic compounds will dissolve in water.
--> Although ions attracted to each other, attraction btwn ions to the dipole of
water is GREATER = ion dipole force (causes ions to pull away from the lattice =
dissolves).
Factors of Ionic Compound Solubility in Water
, 3
1. Larger ionic radius = increases solubility (when larger radii, attraction btwn ions
in ionic compound is weaker due to charges being more farther apart)
2. Greater charge = lower solubility (since more bonds = harder to take apart ions)
Molecular (covalent) Compounds
Dipole-dipole forces hold together the molecules in a polar compound.
--> this force is WEAKER than h-bonds btwn the solute and water = substance
dissolves
-Nonpolar molecular substances = do NOT dissolve in WATER
-Increasing size of non-polar portion of molecule = decreased solubility.
--> Ex. ethanol (larger molecule) vs methanol (smaller)
Dissolving
The BREAKING of INTERmolecular forces of solute particles and becoming
incorporated into solvent particles
--> Ex. Sugar dissolves well in tea
--> rate of dissolving = how quickly solute dissolves in solvent
Intermolecular forces
Van-Der-Wall forces:
1. London dispersion forces (LDF) (all molecular compounds: polar covalent, non-
polar covalent), weakest.
--> only force present in NONPOLAR molecules
2. Dipole-dipole forces (DD) (polar molecules w/ net dipole)
--> Hydrogen bonding (H-Bond) (type of DD force) (btwn H atom and F, O, or N).
Ion-Ion force: strongest intermolecular force only in ionic compounds (opp.
charged ions in ionic compound)
