Calculator Form
Enter reactants and products as comma-separated species. Add states like (aq), (s), (l), or (g).
Example Data Table
| Case | Unbalanced Molecular Entry | Balanced Net Ionic Result | Reaction Pattern |
|---|---|---|---|
| Silver chloride precipitation | AgNO3(aq), KCl(aq) → AgCl(s), KNO3(aq) | Ag+(aq) + Cl−(aq) → AgCl(s) | Precipitation |
| Acid and base neutralization | HCl(aq), LiOH(aq) → H2O(l), LiCl(aq) | H+(aq) + OH−(aq) → H2O(l) | Neutralization |
| Carbonate with acid | HCl(aq), K2CO3(aq) → H2O(l), CO2(g), KCl(aq) | 2 H+(aq) + CO32−(aq) → H2O(l) + CO2(g) | Gas evolution |
| Barium sulfate formation | BaCl2(aq), H2SO4(aq) → BaSO4(s), HCl(aq) | Ba2+(aq) + SO42−(aq) → BaSO4(s) | Precipitation |
Formula Used
1. Element balance matrix: each element becomes a row, and each species becomes a column. The calculator solves A · x = 0 for the smallest whole-number coefficient vector.
2. Complete ionic expansion: strong aqueous electrolytes are dissociated into ions. Solids, liquids, gases, and listed weak species remain intact.
3. Net ionic reduction: identical ions on both sides are canceled. The remaining species form the balanced net ionic equation.
How to Use This Calculator
- Enter reactants as comma-separated formulas, then include phases when known.
- Enter products in the same format, keeping solids, liquids, gases, and aqueous species clearly marked.
- List weak acids or weak bases you want left undissociated.
- Submit the form to view the balanced molecular, complete ionic, and net ionic equations.
- Use the graph for coefficient comparison, then download the result as CSV or PDF.
Requested Practice Answers
Write balanced complete ionic equation for the reaction AgNO3(aq) + KCl(aq) → AgCl(s) + KNO3(aq).
Ag+(aq) + NO3−(aq) + K+(aq) + Cl−(aq) → AgCl(s) + K+(aq) + NO3−(aq)
Complete the balanced overall ionic equation for lead(II) nitrate dissolving in water.
Pb(NO3)2(s) → Pb2+(aq) + 2 NO3−(aq)
Write balanced complete ionic equation for HCl(aq) + LiOH(aq) → H2O(l) + LiCl(aq).
H+(aq) + Cl−(aq) + Li+(aq) + OH−(aq) → H2O(l) + Li+(aq) + Cl−(aq)
Enter the balanced net ionic equation, including phases, for this reaction.
For a standard strong acid and strong base neutralization, the balanced net ionic equation is H+(aq) + OH−(aq) → H2O(l).
Complete the balanced overall ionic equation for sodium iodide dissolving in water.
NaI(s) → Na+(aq) + I−(aq)
Enter the balanced complete ionic equation for HCl(aq) + K2CO3(aq) → H2O(l) + CO2(g) + KCl(aq).
2 H+(aq) + 2 Cl−(aq) + 2 K+(aq) + CO32−(aq) → H2O(l) + CO2(g) + 2 K+(aq) + 2 Cl−(aq)
Write a balanced net ionic equation for the following reaction BaCl2(aq) + H2SO4(aq).
Ba2+(aq) + SO42−(aq) → BaSO4(s)
Write balanced complete ionic equation for Na3PO4(aq) + NiCl2(aq) → Ni3(PO4)2(s) + NaCl(aq).
6 Na+(aq) + 2 PO43−(aq) + 3 Ni2+(aq) + 6 Cl−(aq) → Ni3(PO4)2(s) + 6 Na+(aq) + 6 Cl−(aq)
Write a balanced complete ionic equation for HCHO2(aq) + NaOH(aq) →
HCHO2(aq) + Na+(aq) + OH−(aq) → H2O(l) + Na+(aq) + CHO2−(aq)
Enter the balanced complete ionic equation for K2SO4(aq) + CaI2(aq) → CaSO4(s) + KI(aq).
2 K+(aq) + SO42−(aq) + Ca2+(aq) + 2 I−(aq) → CaSO4(s) + 2 K+(aq) + 2 I−(aq)
FAQs
What is the difference between a complete ionic equation and a net ionic equation?
A complete ionic equation shows all strong aqueous electrolytes as free ions. A net ionic equation removes spectator ions and keeps only the species that actually change during the reaction.
Why are phase labels important?
Phase labels tell the calculator which substances stay intact. Solids, liquids, and gases are not split into ions, while many aqueous species can dissociate and later cancel as spectators.
Should every aqueous compound be dissociated?
No. Strong acids, strong bases, and soluble salts usually dissociate. Weak acids, weak bases, water, gases, and precipitates should remain intact in the ionic form.
What is a spectator ion?
A spectator ion appears unchanged on both sides of the complete ionic equation. It does not participate in bond formation, precipitation, neutralization, or gas evolution, so it is canceled.
Why might a reaction fail to balance here?
The most common reasons are missing products, incorrect formulas, wrong states, or unsupported ion decomposition. Recheck spelling, subscripts, and whether the reaction is chemically valid.
Does water dissociate in the final answer?
Water is usually left as H2O(l) in complete and net ionic equations. Even though water self-ionizes slightly, it is not written as free ions in standard classroom balancing.
Can weak acids stay molecular in ionic equations?
Yes. Weak acids such as HCHO2 or HC2H3O2 are commonly written undissociated in the complete ionic equation, then converted only where reaction chemistry demands a net change.
Why are solids never split into ions?
A solid precipitate is written as a single compound because its ions are locked in the crystal lattice. The precipitate forms the visible product and stays intact in ionic notation.