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:

• AgNO3(aq) + NaCl(aq) = AgCl(s) + NaNO3(aq)
• HCl(aq) + NaOH(aq) = NaCl(aq) + H2O(l)
• BaCl2(aq) + Na2SO4(aq) = BaSO4(s) + NaCl(aq)
• Pb(NO3)2(aq) + KI(aq) = PbI2(s) + KNO3(aq)
• CaCl2(aq) + Na2CO3(aq) = CaCO3(s) + NaCl(aq)
• HNO3(aq) + KOH(aq) = KNO3(aq) + H2O(l)
• FeCl3(aq) + NaOH(aq) = Fe(OH)3(s) + NaCl(aq)
• H2SO4(aq) + Ba(OH)2(aq) = BaSO4(s) + H2O(l)

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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