NH4Cl and Na2CO3

Balanced Equation

Total Ionic Equation

Net Ionic Equation

2NH4Cl (aq) + Na2CO3 (aq) → 2NaCl (aq) + (NH₄) ₂CO₃ (s)

2NH4 + (aq) + 2Cl - (aq) + 2Na + (aq) + CO3^2 - (aq) → 2Na + (aq) + 2Cl - (aq) + (NH₄) ₂CO₃ (s)

2NH4 + (aq) + CO3^2 - (aq) → (NH₄) ₂CO₃ (s)

Explanation:

Step 1: Data given

The reactant are NH4Cl and Na2CO3

Step 2: The unbalanced equation

NH4Cl (aq) + Na2CO3 (aq) → NaCl (aq) + (NH₄) ₂CO₃ (s)

Step 3: Balancing the equation

NH4Cl (aq) + Na2CO3 (aq) → NaCl (aq) + (NH₄) ₂CO₃ (s)

On the left side we have 2x Na (in Na2CO3) on the right side we have 1x Na. To balance the amount of Na on both sides we have to multiply Nacl by 2

NH4Cl (aq) + Na2CO3 (aq) → 2NaCl (aq) + (NH₄) ₂CO₃ (s)

On the right side we have 2x N (in (NH4) 2CO3), on the left side we have 1x N (in NH4Cl). To balance the amount of N on both side, we have to multiply NH4Cl by 2.

2NH4Cl (aq) + Na2CO3 (aq) → 2NaCl (aq) + (NH₄) ₂CO₃ (s)

The total ionic equation

The complete ionic equation is used to describe the chemical reaction while also clearly indicating which of the reactants and/or products exist primarily as ions in aqueous solution.

2NH4 + (aq) + 2Cl - (aq) + 2Na + (aq) + CO3^2 - (aq) → 2Na + (aq) + 2Cl - (aq) + (NH₄) ₂CO₃ (s)

The net ionic equation

In a net ionic equation, all spectator ions are completely removed.

2NH4 + (aq) + CO3^2 - (aq) → (NH₄) ₂CO₃ (s)

a) Balanced Equation

2NaCl (aq) + (NH₄) ₂CO₃ (aq) → Na₂CO₃ (aq) + 2NH₄Cl (aq)

b) Total Ionic Equation

2Na⁺ (aq) + 2Cl⁻ (aq) + 2NH₄⁺ (aq) + CO₃ ²⁻ (aq) → 2Na⁺ (aq) + CO₃²⁻ (aq) + 2NH₄⁺ (aq) + 2Cl⁻ (aq)

c) Net Ionic Equation

All are spectator ions, so no net ionic equation.