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In chemistry, colligative properties are the properties of dilute solutions of non-volatile solutes whose values depend only on the concentration of solute particles, not on the type of particles present.
Sifat koligatif larutan adalah sifat larutan yang tidak tergantung pada macamnya zat terlarut tetapi semata-mata hanya ditentukan oleh banyaknya zat terlarut (konsentrasi zat terlarut).

The four colligative properties are:

Vapor pressure depression: The change in vapor pressure where the solute is less volatile than the solvent is regulated by Raoult’s law, which states that the pressure is equal to the mole fraction of the solvent times the vapor pressure of pure solvent: P = Xsolvent*P°. This holds truest for ideal solutions.

Freezing-point depression: The presence of a solute decreases the freezing point as compared to a pure solvent. The exact change (?T) can be calculated as van ‘t Hoff factor (i) of the solute multiplied by its molality (m) multiplied by the freezing point depression constant of the solvent (Kf): ?T = i(?Kf)m. Alternatively, it can be calculated as the total molality of all solutes in solution times the depression constant: ?T = Kf ? m.

Boiling-point elevation: Because of the lowered vapor pressure, the boiling point of a solution is elevated as compared to the pure solvent. The change in boiling point (?T) can be calculated in the same way as the change in freezing point, except a different constant is used: the van ‘t Hoff factor (i) of the solute multiplied by its molality multiplied by the boiling point elevation constant of the solvent (Kb): ?T = iKbm. ?T can also be calculated using the sum of all molalities: ?T = Kb ? m.

Osmotic pressure: The presence of solute can cause pressure to be exerted across a permeable membrane according to an equation quite similar to the ideal gas law: ? is the osmotic pressure, n is the number of moles of solute, R is the ideal gas constant, T is the absolute temperature in kelvins, and V is the volume: ? = (nRTi)/V.

Sifat koligatif meliputi:

1. Penurunan tekanan uap jenuh
2. Kenaikan titik didih
3. Penurunan titik beku
4. Tekanan osmotik

Banyaknya partikel dalam larutan ditentukan oleh konsentrasi larutan dan sifat Larutan itu sendiri. Jumlah partikel dalam larutan non elektrolit tidak sama dengan jumlah partikel dalam larutan elektrolit, walaupun konsentrasi keduanya sama. Hal ini dikarenakan larutan elektrolit terurai menjadi ion-ionnya, sedangkan larutan non elektrolit tidak terurai menjadi ion-ion. Dengan demikian sifat koligatif larutan dibedakan atas sifat koligatif larutan non elektrolit dan sifat koligatif larutan elektrolit.

berikut adalah soal latihan kimia, latihan soal berikut di tekankan pada penguasaan larutan terutama sifat koligatif larutan.
Soal Kimia Larutan

Soal tersebut dalam bahasa indonesia dengan format pdf, berbentuk pilihan ganda di sesuaikan dengan format soal UAN dan SPMB