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Simple Explanation:
What are Mixtures?
Mixtures are composed of two or more substances. There are three types of mixtures:
Homogeneous Mixtures
Colloids
Heterogeneous Mixtures
Homogeneous Mixtures:
Particle sizes are tiny, usually in the nanometer range.
Substances are distributed evenly throughout its volume.
Particles do not settle down.
Examples include brass, salt water, and the air.
Colloids:
Particle sizes are small but larger than ones in a homogeneous mixture.
Substances appear homogeneous but are actually heterogeneous at the microscopic level.
Particles are large enough to be somewhat visible yet small enough to not settle, giving the mixture the property to scatter light.
Examples include milk and fog.
Heterogeneous Mixtures:
Substances are not evenly distributed throughout its volume.
Particles may settle over time if left undisturbed.
Particles are suspended, meaning they don't dissolve into another substance.
Examples include salads, sand in water, and chocolate chip cookies.
Solutions in Chemistry
Solutions are homogeneous mixtures, and are composed of solutes and solvents.
Solvent: A substance that dissolves other substances.
Solute: A substance that gets dissolved into a solvent.
To dissolve a solute, solvents break up the attraction forces between solute particles. For example, water, the universal polar solvent, can dissolve most polar molecular compounds by disrupting their dipole-dipole interactions. It can also dissolve ionic compounds through dissociation, where the electrostatic forces between ions are broken. To get further into detail about the dissolution process, check out this tutorial.
Molarity Formula
M = n ÷ V
M - Molarity
n - Moles of Solute
V - Volume (liters) of Solvent
Molarity is a unit of measurement used to express the concentration of a solute in a solution. We use this formula to determine the concentration or to solve for moles of solute or liters of solvent by rearranging the formula.
Dilution Formula
M₁V₁ = M₂V₂
M - Molarity
V - Volume
This formula is used to calculate a missing measurement value between two versions of a solution before and after dilution. The idea is that molarity is inversely related to volume. It helps determine how to dilute a solution to reach a specific concentration.
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