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Test 3 Review Questions.

Quiz by Jeremy Mitchell-Koch

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30 questions
Show answers
  • Q1
    Which substance is present in the smallest proportion in a solution?
    liquid
    solute
    solvent
    solid
    30s
  • Q2
    Determine the molarity of a solution made by dissolving 11.7 g of NaNO3 in water where the final volume is 250.0 mL.
    0.0311 M
    0.551 M
    0.214 M
    0.138 M
    300s
  • Q3
    Determine the volume of a 0.0351 M Li3PO4 solution that contains 0.0164 moles of Li3PO4
    576 mL
    467 mL
    174 mL
    214 mL
    300s
  • Q4
    Determine the molality of a solution formed by dissolving 0.187 moles of NaCl in 456 grams of water. The density of the solution is 1.44 g/mL.
    0.351 m
    0.244 m
    0.410 m
    0.285 m
    300s
  • Q5
    What mass of LiOH is required to prepare 0.250 L of a 3.55 M solution?
    0.0371 g
    250 g
    0.888 g
    21.3 g
    300s
  • Q6
    What mass of water is required to dissolve 27.8 g of ammonium nitrate NH4NO3 in order to prepare a 0.452 m solution?
    1.30 kg
    0.100 kg
    0.177 kg
    0.768 kg
    300s
  • Q7
    The distinguishing characteristic of all electrolyte solutions is that they
    conduct electricity
    contain molecules
    conduct heat
    react with other solutions
    30s
  • Q8
    Which process defines how an ionic compounds break apart into its constituent ions upon dissolution?
    dissociation
    ionization
    decomposition
    electrolysis
    30s
  • Q9
    What volume of concentrated (14.7 M) phosphoric acid is needed to prepare 25.0 L of 3.0 M H3PO4?
    0.57 L
    5.1 L
    3.6 L
    1.8 L
    300s
  • Q10
    What is the molarity of a solution prepared by diluting 1.85 L of 6.5 M KOH to 11.0 L?
    0.91 M
    1.1 M
    0.28 M
    3.1 M
    300s
  • Q11
    From the following list of aqueous solutions and water, select the one with the highest boiling point.
    pure water
    0.75 M NaCl
    0.75 M CuCl2
    1.0 M KNO3
    60s
  • Q12
    Determine the freezing point of a solution formed by dissolving 0.187 moles of glucose in 456 grams of water. (For water, Kf = 1.86°C/m)
    -3.48 C
    -0.410 C
    -0.351 C
    -0.528 C
    300s
  • Q13
    What is defined as the selective passage of solvent molecules through a porous membrane from a more dilute solution to a more concentrated solution?
    Semipermeability
    Permeability
    Osmosis
    Osmotic Pressure
    30s
  • Q14
    Based on the solubility rules, which of these processes will occur when solutions of ZnSO4(aq) and MgCl2(aq) are mixed?
    ZnCl2 will precipitate; Mg2+ and SO42− are spectator ions.
    No precipitate will form.
    ZnSO4 will precipitate; Mg2+ and Cl− are spectator ions.
    MgSO4 will precipitate; Zn2+ and Cl− are spectator ions.
    120s
  • Q15
    If aqueous solutions of Pb(NO3)2 and NaCl are mixed, which ions, if any, are spectator ions? Pb(NO3)2(aq) + 2NaCl(aq) → PbCl2(s) + 2NaNO3(aq)
    Pb2+(aq), Cl−(aq)
    Na+(aq), NO3− (aq)
    Na+(aq), Cl−(aq)
    Pb2+(aq), NO3−(aq)
    120s

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