Solubility 2

exam 1, chem 116, WVU spring '26

Solutions with __ boiling points have lower freezing points

higher

Henry’s Law: formula

C(gas) = Kₕ × P(gas)

C(gas)

solubility of gas (usually in mol / L)

Kₕ

Henry’s law constant; different for each gas

P(gas)

pressure of gas above the solution

When given percentages, assume a total of __

100g

Vapor pressure: definition

the pressure due to gas particles above the surface of an open container

Vapor pressure is affected by __

temperature and IMF strength

When temperature increases, __

vapor pressure increases

When IMFs increase,

vapor pressure decreases

Non-volatile

insignificant VP, usually a solid

Vapor pressure of a solution (nonvolatile solute) is __ than that of a pure solvent

lower

Raoult’s Law: formula

P(soln) = x(solv) × P⁰(solv)

P(soln)

vapor pressure above solution

X(soln)

mole fraction of solvent

P⁰(solv)

VP of pure solvent at a specific temp

Vapor pressure with a volatile solute and solvent: effect

Partial pressure of each lowers

Vapor pressure with a volatile solute and solvent: formula

P(soln) = (Xa × P⁰a) + (Xb × P⁰b)

Gas phase is __ in more volatile component

enriched

Mixing two types of gas ___ change the partial pressure of each

does not

Partial pressure

basically a measure of how much of each gas is present

Higher vapor pressure =

faster evaporation