Chapter 10 Solutions
Example 10.11
Write net equations for the precipitation reactions in example 10.9.
a) Solutions of FeSO
and KOH 4
The precipitate is Fe(OH)
, so 2OH 2
1- ions are required for each Fe
2+ ion.
Fe
2+ + 2OH
1-^ →
Fe(OH)
(^2)
b) Solutions of Pb(ClO
) 42
and CuSO
(^4)
The precipitate is PbSO
. There is 1:1 ratio of ions, so the net equation is 4
Pb
2+ + SO
2- 4
→
PbSO
(^4)
c) Solutions of K
PO 3
and CoCl 4
(^2)
The precipitate is Co
(PO 3
) 42
, so 3Co
2+ and 2PO
3- 4
are required.
3Co
2+ + 2PO
3-^4
→
Co
(PO 3
) 42
Example 10.12 Write net equations for the reactions occurring when solutions of the following substances are mixed. Indicate ‘no reaction’ if no precipitate is expected to form. a) Potassium iodide + lead nitrate
1+K
- I
1- + Pb
2+ + NO
1-^3
1
2
- No reaction because KNO
is soluble by Rules 1 and 2. 3
- PbI
precipitates by Rule 3. 2
Net reaction: Pb
2+ + 2I
1-^ →
PbI
(s). 2
b) Sodium phosphate + silver nitrate
Na
1+ + PO
3- 4
+ Ag
1+ + NO
1- 3
1
2
- No reaction because NaNO
is soluble by Rules 1 and 2. 3
(^)
- Ag
PO 3
precipitates by Rule 5. 4
Net reaction: 3Ag
1+ + PO
3-^4
→
Ag
PO 3
(s). 4
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