Solutions

Definition and Components

Solutions represent homogeneous mixtures made of two or more components that form a uniform composition throughout. Understanding the nature of solutions is fundamental in chemistry, as many chemical reactions occur in solution.

• Solute: The smaller portion of the solution that is dissolved within the solvent.

• Solvent: The part of a solution that is present in the larger amount, which can dissolve other substances.

• Concentration: A measurement of the amount of solute in a given amount of solvent.

Example: If 10 g NaCl is dissolved in 500.0 mL of water, NaCl is the solute and water is the solvent.

Equation for Concentration:

Solution Formation

When a solute is added to a solvent, the solute particles disperse uniformly throughout the solvent, forming a homogeneous mixture. For example, salt (NaCl) dissolves in water to form a saltwater solution.

• Solute particles are evenly distributed in the solvent.

• The resulting mixture is homogeneous and appears as a single phase.

Suspensions vs. Colloids

Types of Mixtures

Mixtures can be classified based on the size of their particles and their ability to remain uniformly distributed.

Additional info: Colloids scatter light (Tyndall effect), while solutions do not.

Examples and Identification

Given images of three containers:

• A: Solution (clear, homogeneous)

• B: Suspension (particles visible, settle over time)

• C: Colloid (cloudy, does not settle)

Example: Milk is a colloid, muddy water is a suspension, and saltwater is a solution.

Summary Table: Mixture Types