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More lessons on Chemistry
In this lesson, we will look at some examples of
Balancing chemical equations containing polyatomic ions
Atoms can neither be destroyed nor created during a simple chemical reaction. Therefore, in a chemical reaction
The sum of atoms before reaction = the sum of atoms after reaction
The following figure gives some hints on how to balance chemical equations. Scroll down the page for more examples and solutions.

General Rules for balancing chemical equations – Polyatomic Ions
Balancing chemical equations may require some trial and error. There are some general rules that could be helpful, but they may not work all the time.
Rule 1 Balancing chemical equations using the one’s and two’s technique
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Rule 2 Balancing chemical equations using the two’s and three’s technique
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Rule 3 Balancing chemical equations using the CHO technique
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Rule 4 Balancing chemical equations using the even technique
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Rule 5 Balancing chemical equations containing polyatomic ions
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Case 1: If the polyatomic ion remains the same before and after the reaction, then treat it as “a single element” for ease of calculation. Try to start with the most complicated-looking group.
Example:
Balance the equation
Ca + HNO3 → H2 + Ca(NO3)2
Solution:
- Check to make sure that all coefficients are in the lowest-possible ratio
How to balance chemical equations containing polyatomic ions?
Example:
Balance the following equation:
Ca(NO
3)
2 + Na
2S → CaS + NaNO
3
Example:
Balance the following chemical equation:
Fe(NO
3)
3 + (NH
4)
2CO
3 → Fe
2(CO
3)
3 + NH
4NO
3
Example:
Balance the following chemical equation:
AgNO
3 + K
2CrO
4 → Ag
2CrO
4 + KNO
3
How to balance chemical equations containing polyatomic ions?
Example:
Balance the following chemical equation:
Pb(NO
3)
2 + NA
2CO
3 → PbCO
3 + NaNO
3
Case 2: If the polyatomic ion is changed after the reaction then it would be necessary to consider each atom individually.
Example:
Balance the chemical equation
Ba(OH)2 + H3PO4 → BaHPO4 + H2O
Solution:
- Check to make sure that all coefficients are in the lowest-possible ratio.
How to balance chemical equations with polyatomic ions by rewriting H2O as H(OH)?
Examples:
Balance the following chemical equations:
Al
4C
3 + H
2O → Al(OH)
3 + CH
4
C
3H
8 + O
2 → CO
2 + H
2O
C
6H
6 + O
2 → CO
2 + H
2O
Three helpful tips and tricks that make Balancing Chemical Equations easier
Tip #1: Put a star(*) next to any element appearing more than once on either the product or the reactant side; balance those elements last.
Tip #2: Recognize polyatomic groups that appear on both sides of the equation, and tea them as single items (e.g. don't break SO
4 into one sulfur and four oxygens)
Tip #3: If you have H and OH on one side and H
2O on the other, it is helpful to rewrite H
2) as H(OH).
Examples:
Balance the following chemical equations:
1. C
3H
8 + O
2 → CO
2 + H
2O
2. Al
2(SO
4)
3 + Ca(OH)
2 → Al(OH)
3 + CaSO
4
3. H
3PO
4 + NaOH → Na
3PO
4 + H
2O
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