Henry's Law

$p = K_H \cdot x$ K_H unit: atm or bar. K_H increases with temperature → solubility decreases.

Raoult's Law — Volatile Binary

$P_{total} = x_A \cdot P^\circ_A + x_B \cdot P^\circ_B$

Raoult's Law — Non-volatile Solute

$\frac{\Delta P}{P^\circ} = x_{solute} = \frac{n_2}{n_1 + n_2}$

Boiling Point Elevation

$\Delta T_b = i \cdot K_b \cdot m \qquad K_b(\text{water}) = 0.52 \text{ K·kg/mol}$

Freezing Point Depression

$\Delta T_f = i \cdot K_f \cdot m \qquad K_f(\text{water}) = 1.86 \text{ K·kg/mol}$

Osmotic Pressure

$\pi = i \cdot C \cdot R \cdot T \qquad R = 0.0821 \text{ L·atm/(mol·K)}, \quad T \text{ in Kelvin}$

Molar Mass — Boiling Point Method

$M_2 = \frac{K_b \times w_2 \times 1000}{\Delta T_b \times w_1}$

Molar Mass — Freezing Point Method

$M_2 = \frac{K_f \times w_2 \times 1000}{\Delta T_f \times w_1}$

Molar Mass — Osmometry

$M_2 = \frac{w_2 \cdot R \cdot T}{\pi \cdot V}$

Van't Hoff Factor — Dissociation

$i = 1 + (n-1)\alpha \qquad \alpha = \frac{i - 1}{n - 1}$

Van't Hoff Factor — Association (Dimerization, n = 2)

$i = 1 - \frac{\alpha}{2} \qquad \alpha = 2(1 - i)$

Mole Fraction of Vapour Phase

$y_A = \frac{x_A \cdot P^\circ_A}{x_A \cdot P^\circ_A + x_B \cdot P^\circ_B}$

Key Constant Values