Chp 13 & 14 Flashcards

Solution components

Homogeneous mixture of solute present in smallest amount) & solve (present in largest amount)

What determines whether a solution forms

Strengths of IMFs between & among solute and solvent particles.

How do solutions forms

When the magnitudes of the attractive forces between solute and solvent particles are comparable or greater than those that exist between solute particles themselves or between solve particle themselves.

Dissolve

solute + solvent → solution

Crystallization

solution → solute + solvent

Saturation

crystallization and dissolution are in equilibrium

Solubility

amount of solute reuqire dot form a saturated solution

supersaturated

a state where a solution contains more dissolved solute than it would under normal circumstances, typically achieved by increasing temperature or pressure.

Interactions

— Polar solvent will dissolve polar solutres

miscible liquids

mix in any proportions

immiscible liquids

don’t mix

Factors Affecting Solubility

more oh within a molecule → increases solubility in water

“Like dissolves like”

More polar bonds in the molecule, the better it dissolves in a polar solvent

Less polar a molecule → less soluble in water

Non polar increases, less solauble in water.

Why don’t network solides dissolve?

Forces in the solids are too strong. They are bonded rto each other in a covalent bond in every direction.

Henry’s Law

Higher the pressure, the more molecules of gas are close to the solceneet and the greater the chance of a gas molecule striking the surface and entering the solution.

• Higer pressure → greater solubility

• Lower pressure → fewer molecules of gas are close to the solvent & lower the solubility

Henry’s Law Formula

S_g = kP_g

Sg = solubility of gas

K = constant

Pg = Partial gas

Temperature

Solubility of salts increase with temp increase, 95% of the time.

Gases & Temps

Increases in temp → Less soluable gas