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					Lv One 2010-2011
Naming and Writing Formulas of Compounds (Ch. 6)
                 Names and Formulas of Ionic Compounds

In this lab activity, you will combine a number of different
chemicals, and will determine which combinations result in a chemical
reaction. For each reaction that occurs, you will write out the
chemical name and formula of each of the products formed. You will
then use a solubility chart to determine the state of matter of each

Required materials: Read the procedure and create a list of materials
needed to complete the lab.

Safety & Disposal
You must wear goggles and an apron for this lab. At the end of the
lab, the chemicals should be soaked up with paper towels, and disposed
of in the waste container in the hood. Transparencies should be
washed with soap and water and dried off.
Look up the MSDS for solutions of NaOH, AgNO3, Pb(NO3)2, and Na2CO3 and
record their hazards in your lab notebook. Na3PO4 and CaCl2 are not
considered hazardous, so you do not need to write entries for these.
You will need to figure out the names for each of these compounds
before looking up the MSDS. This is pre-lab question one.

Add two drops of each aqueous solution on the reaction grid
(transparency sheet) provided. Record your observations of each
reaction (or non-reaction). The solutions you will be using are:
0.1 M Na3PO4                                0.5 M NaOH
0.05 M AgNO3                                0.2 M Pb(NO3)2
0.5 M CaCl2                           1.0 M Na2CO3

Pre-lab Questions:
1. Write the names of all the chemicals used in this lab.
2. List four indicators of a chemical reaction.

Data Table: No data table is needed for this lab.
Observations Table: Create your table to record procedure step # and
observations.   You will need detailed observations of the solutions
before you begin combining them, as well as detailed observations of
the results of each combination.

Calculations – There are no calculation for this lab.
Error Analysis – No error analysis is necessary for this lab.
1. All of the chemical reactions that you just observed are called
double replacement reactions. Double replacement reactions are
characterized by the mixing of two aqueous reactants to form one
aqueous product and one solid product. The solid product exists
because the compound is insoluble in water.
For each reaction,
         1. Write the formulas for the cation and anion that make up
            each reactant.
         2. Complete the chemical equation by writing the formulas of
            each product formed.
            3. Name both reactants and products to complete the word
            4. Write the state of matter for each product. Use your
               solubility chart to determine if each product is soluble.
               Write (s) beside the solid (insoluble) product and (aq)
               beside the aqueous (soluble) product.

Record this information in your notebook in the order shown on the
back of this page. The first reaction is done for you. Follow this
format for all of the other reactions.   If there was no chemical
reaction observed, write ‘no reaction’ beside the reactants. Do not
complete anything else for this/these reaction(s).

 Rxn 1:      AgNO3 and Na2CO3

Ions in reactants: Ag+1           NO3-1     Na+1   CO3-2

Chemical Equation:              AgNO3(aq) + Na2CO3(aq)        Ag2CO3(s) + NaNO3(aq)

Word Equation:      silver nitrate + sodium carbonate  silver carbonate +
sodium nitrate

Rxn   2:   AgNO3 and Na3PO4
Rxn   3:   AgNO3 and NaOH
Rxn   4:   Pb(NO3)2 and Na2CO3
Rxn   5:   Pb(NO3)2 and Na3PO4
Rxn   6:   Pb(NO3)2 and NaOH
Rxn   7:   CaCl2 and Na2CO3
Rxn   8:   CaCl2 and Na3PO4
Rxn   9:   CaCl2 and NaOH

Conclusion – Write a summary of your results, and identify how this
lab relates to content we are studying in class.

General Solubility Rules (needed to complete analysis)

  1. Most compounds containing an alkali metal or ammonium ion are
  2. Most nitrates and acetates are soluble.
  3. Most halides (compound containing halogens) are soluble, except
     those containing Ag, Pb, Hg.
  4. Most sulfates are soluble except Ba, Sr, Ca, Hg, Ag, Pb.
  5. Except when paired with an alkali metal or ammonium, most
     carbonates, hydroxides, oxides, and phosphates are insoluble.

For this lab we will be focusing on observations and analysis

                                Complete    Incomplete Missing
                                without     or
                                errors      complete
     Title/Date           1            0.5          0
     Purpose              1            0.5          0
     Required             1            0.5          0
     Safety and           2            1.0          0
     Pre-lab              2            1.0          0
                          Proficient   Developing   Beginning Missing
     Observations         5            4-3          2-1       0
     Analysis             12-10        9-6          5-0       0
                          Complete     Incomplete   Missing
                          without      or
                          errors       complete
     Conclusion           1            .5           0

                                  Score:     _________ /25

Reaction Grid

                  AgNO3            Pb(NO3)2                     CaCl2

                  A               B                     C


                  D               E                     F


                  G               H                     I


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