Dilute solutions contain a relatively small amount of solute compared to the solvent, while concentrated solutions have a higher proportion of solute.
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Homogeneity in a solution is achieved when the particles of the solute are evenly distributed throughout the solvent, resulting in uniform properties throughout the mixture.
Examples include lemonade, soda water, alloys (solid solutions), and air (gaseous solution).
A solution is a homogeneous mixture composed of two or more substances, where the components are evenly distributed at the particle level.
The concentration of a solution refers to the amount (mass or volume) of solute present in a given amount (mass or volume) of solution, expressed as a ratio or percentage.
The three common methods for expressing concentration are mass/volume percent (%), molarity (M), and molality (m). These methods provide different perspectives on the amount of solute relative to the solvent in a solution.
Different substances in a given solvent can have different solubilities at the same temperature due to variations in their molecular structures and interactions with the solvent molecules.
When a saturated solution is slowly cooled, its solubility typically decreases, leading to the precipitation of excess solute as solid crystals.
An unsaturated solution is one in which the amount of solute dissolved in the solvent is less than the saturation level, allowing for further solute to dissolve.
Understanding solubility allows for the preparation of solutions with desired concentrations by determining the maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature, ensuring the solution is not oversaturated or undersaturated.