Chemisode Simulations Precipitation Reactions All simulations

Precipitation reactions

Predict the product, animate the mixing, inspect the ions, then write the full and net ionic equations.

1. Choose and predict

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Prediction is optional. Enter a formula/name or NA, or mix immediately.
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Writing a full equation

1. Predict productsFor a possible double-displacement reaction, pair each cation with the anion from the other solution. At this stage, write the names only.silver nitrate + barium chloride → silver chloride + barium nitrate
2. Write formulasUse ion charges to write formulas for both reactants and both products. Ag⁺ and NO₃⁻ form AgNO₃; Ba²⁺ and Cl⁻ form BaCl₂; Ag⁺ and Cl⁻ form AgCl; Ba²⁺ and NO₃⁻ form Ba(NO₃)₂.AgNO₃ + BaCl₂ → AgCl + Ba(NO₃)₂
3. Balance equationChange coefficients only; never change subscripts. Two AgNO₃ units are needed to supply two Ag⁺ and two NO₃⁻ ions.2AgNO₃ + BaCl₂ → 2AgCl + Ba(NO₃)₂
4. Add statesStarting solutions are aqueous. The VCE table identifies AgCl as insoluble, while Ba(NO₃)₂ remains aqueous.2AgNO₃(aq) + BaCl₂(aq) → 2AgCl(s) + Ba(NO₃)₂(aq)
Net ionic equation
Remove Ba²⁺ and NO₃⁻ because they remain unchanged as spectator ions.
Ag⁺(aq) + Cl⁻(aq) → AgCl(s)

VCE qualitative solubility table

Relevant product cells are outlined in purple. Select any cell to inspect the salt and its classification.

s = solubless = sparingly solublei = insoluble— = no reliable data because the salt decomposes or reacts with water before dissolving
Select a cell.