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Representations of Solutions

Solutions are homogeneous mixtures of two or more substances, consisting of a solute dissolved in a solvent. Representing solutions correctly is essential for quantitative chemistry calculations and understanding chemical reactions in solution.

Concentration Units​

  1. Molarity (M)

    • Moles of solute per liter of solution.
    • M = n(solute)/V(solution)

  2. Molality (m)

    • Moles of solute per kilogram of solvent.
    • m = n(solute)/mass(solvent in kg)

  3. Percent Composition

    • Mass Percent: (mass of solute/mass of solution) × 100%
    • Volume Percent: (volume of solute/volume of solution) × 100%
    • Mass/Volume Percent: (mass of solute/volume of solution) × 100%

  4. Mole Fraction (χ)

    • Ratio of moles of one component to total moles in solution.
    • χ = n(component)/n(total)

Dilution​

  • Definition: Reducing the concentration of a solution by adding more solvent.
  • Equation: C₁V₁ = C₂V₂
    • C₁ = initial concentration
    • V₁ = initial volume
    • C₂ = final concentration
    • V₂ = final volume

Importance​

  • Accurate solution representation is critical in stoichiometry, titrations, and chemical analysis.
  • Helps predict colligative properties like boiling point elevation and freezing point depression.
  • Essential in laboratory preparation and chemical reactions.

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