CHM 1046                           TEST  1          Name _______________________
May 22, 1996                                    (please print)                  
                                                   Soc.Sec.Num. ________________

      This exam consists of four pages.  Make sure you
have one of each.  Print your name at the top of each
page now.  A fifth page contains a periodic chart and
other information you may need.  You may tear this
sheet off and use it for scratch paper.  Show your
work on calculations, be sure to include units in the
calculations, and give answers to the correct number
of significant figures.  You may use atomic weight
values rounded to the nearest 0.1 amu.

      If anything confuses you or is not clear, raise
your hand and ask!

Points

1.    For the potential reactants below:
      1)   provide the correct formulas in molecular form for the
           potential reactants;
      2)   provide correct formulas for the potential metathesis products
           in the molecular form;
      3)   write a balanced, net ionic equation, or indicate "no net
           ionic equation" if there is none;
      4)   if there is a net reaction, state your conclusion as to
           whether it goes forward, backward, or is indeterminate.


(6)A. iron(III) chloride  +  silver nitrate











(6)B. magnesium iodide  +  sodium hydroxide











(6)2. Circle the strong bases in the following list:

      NaOH      NH4OH      Ca(OH)2    Be(OH)2   Fe(OH)3    MgBr2



(12)3.Balance the following redox reaction under basic conditions.  Show
      your work by writing and balancing the half-reactions.  Reduce the
      balanced equation by canceling species on both sides and by
      reducing the coefficients to the lowest whole numbers.  Identify
      the reacting species called for immediately below the equation.

      NO2-   +     Alo    ---->     NH3     +     AlO2-

      Oxidizing agent ________        Reducing agent ______














(6)4. Although FeCO3 is insoluble in water, it still reacts with an
      aqueous solution of HCl.  What provides the driving force for this
      reaction?  Write the net ionic reaction.







(4)5. Copper does not react with HCl(aq).  Why not?  Yet it does react
      with nitric acid (HNO3(aq)).  Explain.







(5)6. You have an aqueous solution labeled 13.2% AgNO3.  One hundred
      grams of this solution would contain how many moles of AgNO3?










(6)7. A commercial reagent bottle of concentrated aqueous ammonia
      contains 28% NH3 and has a density of 0.90 g/mL.  What is the
      molarity (M) of this solution?










8.    Eighty proof alcohol contains 40% ethanol (C2H6O) in water.  

(6)   (a)  What is the mole fraction (X) of ethanol in this solution?









(6)   (b)  What is the molality (m) of alcohol in this solution?










(3)9. Analysis of your water supply showed it to contain 19 ppb cadmium. 
      How many grams of cadmium would you consume by drinking 325 mL of
      the water?





(6)10.Water has a vapor pressure of 525.8 torr at 90 oC.  What would be
      the vapor pressure at this temperature of a solution of 15 g of
      urea (molecular weight = 60 g/mol, non-dissociating in solution) in
      150 g of water?
      
      
      
      
      
      
      
      
      
      
      
(12)11.The boiling point of chloroform is 61.2 oC, and the boiling point
      elevation constant (Kb) for chloroform is 3.63 oC/m.  A solution of
      3.53 g of an unknown substance dissolved in 115 g of chloroform
      boils at 63.1 oC.  What is the molecular weight of the unknown,
      assuming it does not dissociate in solution?
















(6)12.In the following list, place an h next to the solution with the
      highest boiling point, and an l next to the one with the lowest
      boiling point.

      ____ 0.25 m ammonia

      ____ 0.12 m sugar

      ____ 0.05 m magnesium chloride


(10)13.The osmotic pressure of blood plasma is about 7.0 atmospheres.  You
      want to prepare a solution of a similar osmotic pressure for
      storing blood cells by dissolving sucrose (MW = 342 g/mol) in
      water.  How many grams of sucrose will be needed per 100 mL of
      solution?  (R = 0.08205 L-atm/mol-K; assume T = 25 oC).