$word_{count}$: 200

Molarity to molality: m = 1000$\frac{M}{1000d - M*M_s}$, where d = density $\frac{g}{mL}$, $M_s$ = solute molar mass. Molarity from density and mass%: M = 10dw%/$M_s$. Molarity to mole fraction: $x_{solute}$ = M*$\frac{M_solvent}{1000d}$ approximately for dilute solutions. Normality = M x n-factor. Dilution: M1V1 = M2V2 (moles conserved). Mixing solutions of same solute: $M_f$ = $\frac{M1V1 + M2V2}{(V1+V2)}$. Mixing acid and base: find meq of each, subtract, divide by total volume. If meq(acid) > meq(base): solution is acidic, [H+] = excess meq / total V(mL) x 10^-3. Weight/volume %: g solute per 100 mL solution. Volume/volume %: mL solute per 100 mL solution. ppm: mg/L for aqueous (since density ≈ 1). ppb: micrograms/L. Molarity is temperature-dependent (volume changes). Molality, mole fraction, mass%, ppm are temperature-independent.