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Net Ionic Equation Calculator


Net Ionic Equation Analysis

Molecular Equation
FeCl3(aq) + 3 NaOH(aq) = Fe(OH)3(s) + 3 NaCl(aq)

Full Ionic Equation
Fe{+3} + 6 Cl{-} + 6 Na{+} + 3 OH{-} = Fe(OH)3(s)

Net Ionic Equation
Fe{+3} + 3 OH{-} = Fe(OH)3(s)

Spectator Ions
3 Cl{-} 3 Na{+}
These ions appear unchanged on both sides of the equation and do not participate in the reaction.

Physical States and Products
Precipitates (↓): Fe(OH)3

Step-by-Step Analysis
Step 1: Write the balanced molecular equation

Step 2: Break down aqueous ionic compounds into their constituent ions

FeCl3(aq) dissociates into Fe{+3} + 3Cl{-}

NaOH(aq) dissociates into 3Na{+} + 3OH{-}

NaCl(aq) dissociates into 3Na{+} + 3Cl{-}

Step 3: Write the full ionic equation showing all ions

Step 4: Identify and cancel spectator ions (ions that appear unchanged on both sides)

Cl{-} appears on both sides with the same coefficient (3) - it is a spectator ion

Na{+} appears on both sides with the same coefficient (3) - it is a spectator ion

Step 5: Write the net ionic equation by removing spectator ions

Step 6: The net ionic equation shows only the species that actually participate in the reaction


Instructions for net ionic equation analysis:

  • Enter a balanced chemical equation with aqueous reactants and products
  • Use correct chemical formulas (e.g., AgNO3, not AgNo3)
  • Include state symbols: (aq) for aqueous, (s) for solid, (l) for liquid, (g) for gas
  • Separate reactants and products with = or →
  • Use + to separate multiple compounds on each side
  • Example format: AgNO3(aq) + NaCl(aq) = AgCl(s) + NaNO3(aq)
  • The calculator will identify spectator ions and show the net ionic equation

Examples of equations for net ionic analysis:

Understanding Net Ionic Equations

Net ionic equations show only the chemical species that actually participate in a chemical reaction by removing spectator ions that appear unchanged on both sides of the equation.

Types of Chemical Equations

  • Molecular Equation: Shows complete chemical formulas of all reactants and products
  • Full Ionic Equation: Shows all aqueous ionic compounds as dissociated ions
  • Net Ionic Equation: Shows only ions and compounds that actually change during the reaction

Key Concepts

  • Spectator Ions: Ions that appear unchanged on both sides of the equation and can be cancelled out
  • Precipitate: An insoluble solid that forms from aqueous solutions, marked with (s) or ↓
  • Gas: A gaseous product that escapes from solution, marked with (g) or ↑
  • Aqueous: Dissolved in water, marked with (aq)

Example Analysis

Molecular equation: AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq)

Full ionic equation: Ag⁺(aq) + NO₃⁻(aq) + Na⁺(aq) + Cl⁻(aq) → AgCl(s) + Na⁺(aq) + NO₃⁻(aq)

Net ionic equation: Ag⁺(aq) + Cl⁻(aq) → AgCl(s)

Spectator ions: Na⁺ and NO₃⁻ (appear unchanged on both sides)

Precipitate: AgCl(s) - silver chloride forms as an insoluble solid

Lesson on Net Ionic Equations

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