Solubility curve and vocab

Define a solution in chemistry.

A solution is a homogeneous mixture composed of two or more substances, where one substance (the solute) is dissolved in another (the solvent).

Explain the Tyndall effect.

The Tyndall effect is the scattering of light by particles in a colloid or in very fine suspensions, which makes the path of the light beam visible.

Describe the difference between miscible and immiscible liquids.

Miscible liquids are those that can mix in any proportion without separating, while immiscible liquids do not mix and will separate into distinct layers.

What is a colloid?

A colloid is a mixture where very small particles of one substance are dispersed throughout another substance, and these particles do not settle out over time.

How does Brownian motion relate to particles in a suspension?

Brownian motion refers to the random movement of particles suspended in a fluid, resulting from collisions with the fast-moving molecules of the fluid.

Define electrolytes and non-electrolytes.

Electrolytes are substances that dissociate into ions in solution and conduct electricity, while non-electrolytes do not dissociate into ions and do not conduct electricity.

Describe the process of making a saturated solution.

A saturated solution is made by adding solute to a solvent until no more solute can dissolve at a given temperature, resulting in excess solute that remains undissolved.

Explain how temperature affects the solubility of solids in water.

Generally, the solubility of most solid solutes increases with an increase in temperature, allowing more solute to dissolve in the solvent.

What happens to a saturated solution when cooled?

When a saturated solution is cooled, the solubility of the solute typically decreases, leading to the precipitation of excess solute.

Describe the significance of solubility curves in chemistry.

Solubility curves graphically represent the relationship between solubility and temperature, helping to predict how much solute can dissolve in a solvent at various temperatures.

What is the expected outcome when adding a crystal to a saturated solution at a lower temperature?

Adding a crystal to a saturated solution at a lower temperature may result in the precipitation of some solute, as the solubility limit decreases with temperature.