Chemistry Reference
In-Depth Information
From the information found there, we can finish the subscripts in the
equation, as shown here:
Na
3
PO
4(aq)
+ FeCl
3(aq)
3NaCl
(aq)
+ FePO
4(s)
C.
We turn our balanced chemical equation into an ionic equation, by
showing the aqueous compounds as free ions, as they would really exist
in solution. This gives us the ionic equation:
3Na
+
(aq)
+ PO
4
3-
(aq)
+ Fe
3+
(aq)
+ 3Cl
-
(aq)
3Na
+
(aq)
+ 3Cl
-
(aq)
+ FePO
4(s)
D. We turn our ionic equation into a net ionic equation by eliminating the
spectator ions, which, as you know, are the ions that don't enter the
reaction. Cross out the spectator ions:
3Na
+
(aq)
+ PO
4
3-
(aq)
+ Fe
3+
(aq)
+ 3Cl
-
(aq)
3Na
+
(aq)
+ 3Cl
-
(aq)
+ FePO
4(s)
We get the net ionic equation:
Fe
3+
(aq)
+ PO
4
3-
(aq)
FePO
4(s)
E.
As far as identifying the precipitate, it is the iron (III) phosphate, which
is insoluble in water.
All of our results are summarized here:
A. Write a word equation.
sodium phosphate + iron (III) chloride
sodium chloride + iron (III) phosphate
B.
Write a balanced chemical reaction, with subscripts indicating state or
phase.
Na
3
PO
4(aq)
+ FeCl
3(aq)
3NaCl
(aq)
+ FePO
4(s)
C.
Write an ionic equation.
3Na
+
(aq)
+ PO
4
3-
(aq)
+ Fe
3+
(aq)
+ 3Cl
-
(aq)
3Na
+
(aq)
+ 3Cl
-
(aq)
+ FePO
4(s)
D. Write a net ionic equation.
Fe
3+
(aq)
+ PO
4
3-
(aq)
FePO
4(s)
E.
Identify the precipitate.
iron (III) phosphate
Lesson 6-3 Review
For each of the following compounds, state whether they are soluble,
slightly soluble, or insoluble in water at 25
o
C and 101.3 kPa of pressure.
1. aluminum acetate
2. magnesium bromide
3. zinc carbonate
4. potassium chloride
5. silver iodide
6. barium hydroxide
