Study guide - Chapter 16

I.  Define or identify

  1.  solute -


  2.  solvent -


  3.  tincture -


  4.  saline solution -


  5.  saturated solution -


  6.  supersaturated solution -


  7.  amalgam -


  8.  lattice energy -


  9.  hydration energy -


 10.  % concentration versus proof -


 11.  solution -


 12.  exothermic reaction -

II.  Describe how one would prepare a supersaturated solution.



III.  Explain completely how an ice pack becomes cold when the inner liquid bag 
       within the ice pack is broken.
IV.  Calculate the following. 

1.  What is the % by weight of a solution consisting of 80g of salt dissolved 400g of   
        solution?



2.  How many grams of sugar are needed to dissolve in 840g of solution in order to 
     prepare a 60% concentration?



3.  What is the % by weight of a solution that is prepared by dissolving 24g of NaOH 
      in 260g of water?



4.  How many grams of sugar are dissolved in water to make 350 ml of solution with a
     concentration of 25% by weight?  The density of the resulting solution is 1.1g/ml.




5.  What is the concentration in parts per million ( ppm ) of a 2500g solution of 
      chlorinated water which is found to contain .0052g of chlorine?



6.  What is the morality ( M ) of  a solution which contains 8.0g of NaOH dissolved
      in 3 liters of solution?   ( atomic weights - Na = 23, O = 16, H = 1 )



7.  How many grams of NaCl are needed to dissolve in water in order to produce
     450ml of solution with a concentration of .5M.  ( atomic weights - Na = 23, Cl = 35.5)
 



8.  When a salt solution with a concentration of 2.5M is evaporated, 10g of NaCl are 
      produced.  How much salt solution was evaporated in order to retrieve that amount
      of salt?   ( atomic weights -  Na = 23,  Cl = 35.5 )