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Aqueous Ion Lab

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					Aqueous Ion Lab
Postlab
Set 1
  For the boxes that made precipitates:
 • Number half the X’s (one half is the mirror image
   of the other

      Set 1

              Ba2+ Cl-       K+ CrO42-   Na+ CrO42-   Ba2+ NO3-

 Ba2+ Cl-



 K+ CrO42-               1



Na+ CrO42-           2

Ba2+ NO3-                            3           4
                        A. Ions Present
• For the numbered boxes, write the ions present.
• Ex. 1: Ba2+, Cl-, K+, CrO42-


             Ba2+ Cl-         K+ CrO42-   Na+ CrO42-   Ba2+ NO3-

 Ba2+ Cl-



 K+ CrO42-              1



Na+ CrO42-          2

Ba2+ NO3-                             3          4
                 B. Compounds
• The solutions preformed double replacement (the
  anions switched places)
• Write the possible compounds formed with each
  number
• Ex. 1: Ba2+, Cl-, K+, CrO42-
• BaCrO4 and KCl
• Only once actual compound precipitated
• Discover which compound actually was formed
  – Check your solubility rules on page 920 to find which
    compounds are soluble and insoluble
  – If there is an S between the 2 ions, then no compound was
    formed
  – If there is an I between the 2 ions, then that compound is
    your precipitate. Circle this compound
     C. Equation for the precipitate
• For each precipitate, write the equation of
  formation
• Ex. 1: Ba2+ + Cl- + K+ + CrO42-  BaCrO4 (s) + Cl- + K+
• Eliminate any ion that does not react (called
  spectator ions)

• Ex. 1: Ba2+ + CrO42-  BaCrO4 (s)
Set 2
   For the boxes that made precipitates:
 • Number half the X’s (one half is the mirror image
   of the other

      Set II

               Sr+2 NO3-   Ba2+ NO3-   Al+3 SO42-   Na+ SO42-   Ba2+ Cl-

 Sr+2 NO3-

 Ba2+ NO3-



Al+3 SO42-             1          3

Na+ SO42-              2           4

 Ba2+ Cl-                                      5           6
                    A. Ions Present
• For the numbered boxes, write the ions present.
• Ex. 1: Sr2+, NO3-, Al+3, SO42-


             Sr+2 NO3-   Ba2+ NO3-   Al+3 SO42-   Na+ SO42-   Ba2+ Cl-

 Sr+2 NO3-

 Ba2+ NO3-




Al+3 SO42-           1          3

Na+ SO42-            2           4

 Ba2+ Cl-                                    5           6
                 B. Compounds
• The solutions preformed double replacement (the
  anions switched places)
• Write the possible compounds formed with each
  number
• Ex. 1: Sr2+, NO3-, Al+3, SO42-
• SrSO4 and Al(NO3)3
• Only once actual compound precipitated
• Discover which compound actually was formed
  – Check your solubility rules on page 920 to find which
    compounds are soluble and insoluble
  – If there is an S between the 2 ions, then no compound was
    formed
  – If there is an I between the 2 ions, then that compound is
    your precipitate. Circle this compound
                   C. Equation
• For each precipitate, write the equation of
  formation
• Ex. 1: Sr2+ + NO3- + Al+3 + SO42-  SrSO4 (s) + NO3- +
  Al+3
• Eliminate any ion that does not react (called
  spectator ions)

• Ex. 1: Sr2+ + SO42-  SrSO4 (s)
Set 3
For the boxes that made precipitates:
• Number half the X’s (one half is the mirror image
  of the other



             K+ OH-       Na+ OH-       Fe3+ NO3-   Co2+ NO3- Co+2 Cl-

 K+ OH-

Na+ OH-

 Fe3+ NO3-            1         4

Co2+ NO2-             2             5

 Co+2 Cl-             3             6
                     A. Ions Present
• For the numbered boxes, write the ions present.
• Ex. 1: Sr2+, NO3-, Al+3, SO42-


            K+ OH-       Na+ OH-       Fe3+ NO3-   Co2+ NO3- Co+2 Cl-

 K+ OH-

Na+ OH-

Fe3+ NO3-            1             4

Co2+ NO2-            2             5

Co+2 Cl-             3         6
                 B. Compounds
• The solutions preformed double replacement (the
  anions switched places)
• Write the possible compounds formed with each
  number
• Ex. 1: Fe+3, NO3-, K+, OH-
• Fe(OH)3 and KNO3
• Only once actual compound precipitated
• Discover which compound actually was formed
  – Check your solubility rules on page 920 to find which
    compounds are soluble and insoluble
  – If there is an S between the 2 ions, then no compound was
    formed
  – If there is an I between the 2 ions, then that compound is
    your precipitate. Circle this compound
                   C. Equation
• For each precipitate, write the equation of
  formation
• Ex. 1: Fe+3 + NO3- + K+ + OH-  Fe(OH)3 (s) + K+ +
  NO3-
• Eliminate any ion that does not react (called
  spectator ions)

• Ex. 1: Fe+3 + OH-  Fe(OH)3(s)

				
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posted:4/28/2011
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