Solutions and Mixtures Quiz

Grade 10 · Science · Quiz

Test your knowledge of solution chemistry, concentration calculations, solubility factors, and colligative properties.

Questions

  1. How many moles of solute are present in 500 mL of a 3.0 M solution?

    1. 0.50 mol
    2. 1.50 mol
    3. 6.0 mol
    4. 3.0 mol
    Show answer

    Answer: 1.50 mol

    moles = M × V = 3.0 mol/L × 0.500 L = 1.50 mol

  2. A 200 mL sample of 4.0 M HCl is diluted to 800 mL. What is the new molarity?

    1. 16.0 M
    2. 2.0 M
    3. 0.5 M
    4. 1.0 M
    Show answer

    Answer: 1.0 M

    M₁V₁ = M₂V₂: (4.0 M)(200 mL) = M₂(800 mL). M₂ = 800/800 = 1.0 M

  3. Which of the following substances would make the best electrolyte when dissolved in water?

    1. Sugar (C₁₂H₂₂O₁₁)
    2. Ethanol (C₂H₅OH)
    3. Sodium chloride (NaCl)
    4. Vegetable oil
    Show answer

    Answer: Sodium chloride (NaCl)

    NaCl dissociates into Na⁺ and Cl⁻ ions, allowing electrical conduction. Sugar and ethanol are nonelectrolytes; oil doesn't dissolve in water

  4. The freezing point depression constant (Kf) of water is 1.86°C/m. What is the freezing point of a solution of 0.5 mol NaCl (i=2) in 1 kg of water?

    1. −0.93°C
    2. −1.86°C
    3. −3.72°C
    4. −0.465°C
    Show answer

    Answer: −1.86°C

    ΔTf = Kf × m × i = 1.86 × 0.5 × 2 = 1.86°C. Freezing point = 0 - 1.86 = -1.86°C

  5. Which solution has the highest boiling point?

    1. Pure water
    2. 0.5 m glucose solution
    3. 0.5 m NaCl solution (i=2)
    4. 0.5 m MgCl₂ solution (i=3)
    Show answer

    Answer: 0.5 m MgCl₂ solution (i=3)

    ΔTb = Kb × m × i. MgCl₂ (i=3) gives highest particle count: 0.5×3=1.5 effective molality vs. NaCl 0.5×2=1.0 and glucose 0.5×1=0.5

  6. A solute dissolves exothermically in water. What happens to its solubility when temperature increases?

    1. Solubility increases
    2. Solubility decreases
    3. Solubility stays the same
    4. Solubility increases then decreases
    Show answer

    Answer: Solubility decreases

    For exothermic dissolution, higher temperature shifts equilibrium (Le Chatelier's principle) toward the dissolution being reversed, so solubility decreases

  7. Osmotic pressure is a colligative property that can be used to determine the molar mass of large molecules like proteins.

    Show answer

    Answer: True

    Osmotic pressure π = iMRT is measurable even for dilute solutions of large molecules, allowing molar mass determination: M = π/(iRT)

  8. The formula M₁V₁ = M₂V₂ is used when ________ a concentrated solution to a lower concentration.

    Show answer

    Answer: diluting

    The dilution formula M₁V₁ = M₂V₂ conserves moles of solute; used to calculate the new concentration or volume after adding solvent

Get a personalized course on Solutions and Mixtures built around your child.