1.  List the solute and solvent in a glass of lemonade

2.  If 35 grams of a certain salt will dissolve in 100 grams of water at a 25°C.  If you dissolve 30 grams in 100 grams of water at that temp, describe this solution using the words saturated/unsaturated/supersaturated and concentrated/dilute.

3.  a.  Will oxygen gas be more soluble in water at 10°C or 50°C?
     b.  Will ethyl alcohol (drinking alcohol) be more soluble in water at 10°C or 50°C?
     c.  Will sugar be more soluble in water at 10°C or 50°C?

4. Which of the following will dissolve in liquid CCl₄?  Why?

      a.  NH₃                       b.  CS₂                               c.  H₂O                        d.  CF₄

5. When a salt dissolves in water, water molecules surround it.  Which end of the water is attracted to the cation and which to the anion?  What do we call this?

6.  Complete these concentration problems:

      a.  What is the Molarity (M) if .0030 moles of KCl is dissolved in water to make 250
            ml of solution?
      b.  What is the Molarity (M)  if 8.5 grams of NaNO₃ is dissolved in water to make 500
           ml of solution?
      c.  How many grams of CaSO₄ would you need to make 2 liters of 1.0 M solution?

7.  Compare a solution of 1 M NaCl to pure water in terms of

     a.  boiling point  
     b. freezing point   
     c. vapor pressure
     d.  osmotic pressure

 8.  Which of these solutions will have the greatest effect on the boiling point?

     a.  1 M CaCl₂        b.  1 M NaNO₃           c.  1 M C₆H₁₂O₆         d.  1M AlCl₃

9.  What type of equation is each of the following?

     a.  Cu + AgNO3 ®  CuNO3 + Ag
     b.  Cu + S ®  CuS
     c.   2C₂H₂ + 5O₂ ® 4CO₂  + 2H₂O
     d.  2NaI + ZnCl₂  ®  ZnI₂  + 2NaCl
     e.  2NaClO₃ ®  2NaCl + 3O₂

10.  List oxidation numbers for each element in the following:

       a.  H₂      
       b.  CuCl₂
       c.  KMnO₄
       d.  HBrO₃

  11.  Using the equations in questions #9, list what is oxidized and reduced.

  12.  For each equation, explain if it is exo or endo-thermic.

            a.  2KClO₃ + E ®  2KCl + 3O₂
            b.  C + O₂  ®  CO₂ + E

            Then sketch a graph showing how the energy changes over the time of the
             reaction.

13.  Explain the term Activation Energy.

14.   If you want to speed up the decomposition of hydrogen peroxide into water and oxygen, list two things you could do to the solution.

15.  You have an aquarium divided into two parts with a barrier in between and you put and put 10 goldfish on one side.  Then you remove the barrier.  At what point will equilibrium be reached?  Explain how this is like a chemical reaction.

16.  Set up the K_eq expression for these equations:

            a.  2C₂H₂ (g) + 5O₂ (g) =  4CO₂ (g)  + 2H₂O (g)
            b. 4 P(s)+ 5O₂ (g₎ = 2P₂O₅  (g)

17.  Given the equation  3O₂ (g)  = 2O₃ (g)

            If at a particular temperature at equilibrium the O₂ concentration is .40 M and the
            O₃ is  .0030 M, what is the value of K?

18.   Given the equation in 16a, which way will the equilibrium shift if you

            a.  Add more oxygen
            b.  Increase the temperature (assume it is exothermic)
            c.  Cool the temperature
            d.  Increase the pressure
            e.  Add more carbon dioxide

19.   According to Arrhenius, label the following as an acid, base or salt

            a.  CaSO₄
            b.  HNO₂
            b.  NH₄OH

20.   a.  A liquid tastes sour and turns litmus paper red.  What is it an acid or base?
         b.  A liquid tastes bitter and feels slippery.  What is it an acid or base?

 21.  Complete the following ionization equations.  Label the acid and base on either side of the equation

            a.  HF + H₂O ®
            b.  SO₄^-2 + H₂O ®

22.  Fill in the table: 

23.  What do we call things like HCO₃^-1  that can act like either acids or bases?

24.  Which of the following is a diprotic acid?

            HNO₃              HC₂H₃O₂                    H₂CO₃

25.  Given the K_a for these two weak acids

            Nitrous acid   HNO₂   is 4.5 x 10 ^–4
            Boric acid H₃BO₃ is 5.8 x 10 ^–10

            a.  Which is a stronger acid?
            b.  Which is a stronger base NO₂^-1 or H₃BO₃^-1  ?
            c.  What could you mix if you wanted a buffer approximately equal to 4?
            d.  What would the buffer do?

26.  Write the ionization equation for HNO₂ and its K_a expression.

27.  Name an acid that will ionize completely.

28.  a.  Which is more acidic a solution with pH 3 or 6?
       b.  Which is more basic, a solution with pH 10 or 13?      
       c.  If you have a solution with pH of 3 and you start adding water, what will happen
            to the pH? 
       d.  If you have a solution of pH 9 and you add water, what is the lowest pH number
            you will reach? 

29.  What is the pH of each of the following:

            a.  .001 M HCl
            b.  .000001 M HCl
            c.  .1 M NaOH
            d.  .0001 M NaOH

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