; SCH3U – Solutions and Solubility Review
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SCH3U – Solutions and Solubility Review


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									SCH3U – Solutions and Solubility Review

1) Explain each of the following:

     a) Salt dissolves in water but not in non-polar trifluorotrichloroethane (TTE) whereas iodine
         does not dissolve in water but does dissolve in TTE.

     b) Hydrochloric acid is a good conductor of electricity but concentrated acetic acid is a poor

     c) When sufficient salt is added to water the solution becomes saturated and no more salt
         will dissolve.

2) How would you prepare a 0.50 M solution of sodium hydroxide?

3) What is the general word equation for any neutralization reaction?

4) Write a chemical equation representing the neutralization of iron (III) hydroxide and nitric

5) Write the balanced chemical equation for the reaction of H2SO4 and KOH.

     a) Write the total ionic equation and the net ionic equation for the above reaction.

     b) Circle the spectators.

6) Explain or discuss the dissociation that occurs when sodium chloride is placed in water.
     What is one physical property ionic solutions demonstrate that ionic solids do not?

7) Write the balanced ionic and net-ionic equations, and circle the spectator ions for each of the
     following reactions:

     a) Na3PO4(aq) + Ca(OH)2(aq)      
                                       NaOH(aq) + Ca3(PO4)2(s)
         i)    ionic:

         ii)   net-ionic:   
8)    Zn(s) + CuSO4(aq)     
                             ZnSO4(aq) + Cu(s)
         i)    ionic:

         ii)   

9) Give an example of a solution consisting of a solid in a solid.

10) A crystal of solute is added to an aqueous solution of the same solute. After some time it is
     noted that the crystal has not changed in mass. Is the solution unsaturated, saturated or
     supersaturated? How do you know?
11) A clear colourless liquid with density of 1.4 g/mL was boiled. The initial boiling point was
    101°C and successive boiling points noted were 103°C, 105°C and 107°C. After cooling, the
    density was found to be 2.0 g/mL. Was the original colourless liquid a pure substance or a
    solution? Explain.

12) If a relatively small amount of solute is dissolved in a relatively large amount of solvent, the
    solution is said to be _________________

13) A homogeneous mixture of two or more substances is known as a(n) ________________

14) A saturated solution of potassium nitrate may be made unsaturated by:

15) If much more solute can be dissolved in a solution without altering the temperature, the
    solution is said to be ____________________

16) Chlorate (HClO3) is dissolved in enough water to make 1.00 L of chloric acid. What is the
    molar concentration of this acid?

17) 13. 8.00 g of NaOH is dissolved in sufficient water to make 200.0 mL of solution. What is the
    molar concentration of the solution?
18) At 20 C, a saturated solution of CaCl2 has a concentration of 0.0250 mol/L. A student takes
    50 mL of this solution and evaporates it. What mass of the salt, in grams, is left in the dish?

19) What is the difference between a saturated, a supersaturated and an unsaturated solution?
    How would you differentiate between them experimentally or through observation?

20) Table 1 – Properties of some unknown substances:

    Unknown               Colour                  pH              Conductivity           Litmus
       1                 Colourless               13                 High                  Blue
       2                 Colourless                1                 High                  Red
       3                 Colourless                7                 Low                No change
       4                 Colourless                7                 High               No change
       5                   Blue                    7                 High               No change
The possible substances are HCl, NaOH, NaCl, CuBr2, CH3OH. Identify unknowns 1 – 5 and
briefly explain your reasoning.

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