Explanation:
Raoult's law is stated as:
The relative lowering in vapor pressure of an ideal solution containing the non-volatile solute is equal to the mole fraction of the solute at a given temperature.
i,e, Relative lowering of v.p = mole fraction of solute
Mathematically, it is given by:
\(\frac{{P_1^0 - {P_1}}}{{P_1^0}} = {x_2} = \frac{{{n_2}}}{{{n_1} + {n_2}}}\)
Where n1and n2= no. of moles of solvent and solute respectively, x2= mole fraction of solute, P1o- P1= reduction in vapor pressure of the solvent.
Key Points
- \(Mole\;fraction\;X:\;moles\;of\;a\;component\;/\;Total\;moles\;of\;solution\)
- Mass %: Mass of solute (in g) present in 100g of solution.
- Mass/Vol: Mass of solute (in g) present in 100 mL of solution.
- v/v: Volume of solute/volume of solution {only for liq-liq solutions.}
- g/L: Wt. of solute (g) in 1 L of solutions.
- \(Molality\;\left( m \right) = \frac{{mass\;of\;solute}}{{mass\;of\;solvent\;\left( {kg} \right)}}\)
- \(Molarity\;\left( M \right) = \frac{{moles\;of\;solute}}{{volume\;of\;solution\left( L \right)}}\)
- \(ppm = \frac{{moles\;of\;solute}}{{mss\;of\;solution}} \times {10^6}\)