Chemistry 30

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Solutions

Assignment 5: Net Ionic Equations and Precipitation Reactions

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1. Use a Table of Solubilities to predict whether or not the following compounds are soluble in water.
 

Compound

Soluble (yes or no)

CaI2

 

MgSO4

 

AlPO4

 

Pb(NO3)2

 

Ag2SO4

 

Ca(OH)2

 

 

2. Write formulas for the following compounds, and using a Table of Solubilities predict whether or not the compound is soluble in water.
 

 

 

Formula

 

Soluble (y/n)

a.

potassium phosphate

 

 

 

b.

calcium carbonate

 

 

 

c.

copper(II) bromide

 

 

 

d.

aluminum sulfide

 

 

 

3. What are spectator ions?
4.

For each of the following reactions, predict the products of the reaction. Be sure to write balanced equations.

Then determine if any of the products forms a precipitate.

  • If no precipitate forms, write NR (for “No Reaction”).
  • If a precipitate forms, write the net ionic equation for the reaction.
  a. Mg(NO3)2 (aq) + 2 NaOH(aq)
  b. CuSO4 (aq) + FeCl3 (aq)
  c. K2CO3 (aq) + Sr(OH)2(aq)
5. An aqueous solution contains a mixture of Ba2+, Pb2+ and Ca2+. Select the ONE negative ion listed below which could be used to separate Ba 2+ from the other two positive ions in the mixture.
  a.

Cl-

  b. S2-
  c. OH-
  d.

PO43-

  e. SO42-
6.

An aqueous solution containing the following cations:

Ca2+    Ag+    Cu2+    K+

In order to separate them, the following solutions are available:

Na2S    Na2CO3    NaBr

If we wish to separate the cations by causing only one cation to precipitate out of solution as a time:

  • in what order should the solutions Na2S, Na2CO3, and NaBr be added?
  • identify the three precipitates that form after the addition of those solutions.
  • which one cation will remain in solution?

 

Credits | Central iSchool | Sask Learning | Saskatchewan Evergreen Curriculum | Updated: 22-May-2006