Colloidal solutions and true solutions:

Definition:
- Colloidal solutions are a type of heterogeneous mixture in which the solute particles are larger than the particles in a true solution but smaller than those in a suspension.
- True solutions, on the other hand, are homogeneous mixtures in which the solute particles are uniformly dispersed at a molecular level and cannot be seen with the naked eye.

Particle size:
- The particle size in colloidal solutions ranges from 1 to 1000 nanometers, whereas in true solutions, the particle size is less than 1 nanometer.
- The larger particle size in colloidal solutions allows them to scatter light and exhibit the Tyndall effect.

Tyndall effect:
- The Tyndall effect is the phenomenon in which light is scattered by particles in a medium, making the path of the light visible.
- When a beam of light passes through a colloidal solution, the suspended particles scatter the light in all directions, making the path of the light visible.
- This scattering of light is not observed in true solutions because the particles in true solutions are too small to scatter visible light.

Example:
- An example of a colloidal solution is milk. When a beam of light is passed through a glass of milk, the path of the light becomes visible due to the scattering of light by the suspended fat and protein particles.
- On the other hand, a true solution such as saltwater does not exhibit the Tyndall effect because the dissolved salt particles are much smaller and cannot scatter visible light.

Conclusion:
- In summary, colloidal solutions show the Tyndall effect because of the larger particle size, which allows them to scatter light.
- True solutions do not exhibit the Tyndall effect because the particle size is much smaller and cannot scatter visible light.
- The Tyndall effect is a useful phenomenon in distinguishing between colloidal solutions and true solutions.

Because true solution are (salt,sugar)