Question

Write the complete ionic equation for the reaction between lead perchlorate and sodium sulfide.

A. Pb(ClO4)2 + 2Na2S → PbS + 4NaClO4
B. Pb2+(aq) + 2ClO4-(aq) + 2Na+(aq) + S2-(aq) → PbS(s) + 2Na+(aq) + 2ClO4-(aq)
C. Pb(ClO4)2 + Na2S → PbS + 2NaClO4
D. Pb2+(aq) + 2ClO4-(aq) + 2Na+(aq) + S2-(aq) → PbS(s) + Na2S(aq)

Answer 1

The complete ionic equation for the reaction of lead perchlorate with sodium sulfide is shown in option B, which includes the ions and the solid precipitate formed.

Step-by-step explanation:

The complete ionic equation for the reaction between lead perchlorate and sodium sulfide requires breaking down all soluble ionic compounds into their constituent ions. The given options include both complete ionic equations and net ionic equations. To find the correct complete ionic equation, remember that solid precipitates and weak electrolytes are not broken down into ions.

The reaction between lead perchlorate (Pb(ClO4)2) and sodium sulfide (Na2S) forms lead sulfide (PbS), a solid precipitate, and sodium perchlorate (NaClO4), which remains in solution. Thus, the complete ionic equation should show the lead, perchlorate, and sodium ions, and the sulfide ion before the reaction, and the solid lead sulfide after the reaction. Sodium and perchlorate ions remain unchanged and are spectator ions. Therefore, option B is the correct complete ionic equation:

Pb2+(aq) + 2ClO4-(aq) + 2Na+(aq) + S2-(aq) → PbS(s) + 2Na+(aq) + 2ClO4-(aq).

Answer 2

The complete ionic equation for the reaction between lead perchlorate and sodium sulfide is:

Pb²⁺(aq) + 2ClO₄⁻(aq) + 2Na⁺(aq) + S²⁻(aq) → PbS(s) + 2Na⁺(aq) + 2ClO₄⁻(aq) Option B is answer.

Step-by-step explanation:

Identify the reactants and products:

Reactants: Lead perchlorate (Pb(ClO₄)₂), sodium sulfide (Na₂S)

Products: Lead sulfide (PbS), sodium perchlorate (NaClO₄)

Write the balanced molecular equation:

Pb(ClO₄)₂ + Na₂S → PbS + 2NaClO₄

Separate the electrolytes into their ions:

Pb(ClO₄)₂ → Pb²⁺ + 2ClO₄⁻

Na₂S → 2Na⁺ + S²⁻

Identify spectator ions:

Both sodium and perchlorate ions appear on both sides of the equation, indicating they are not involved in the reaction itself and are considered spectator ions.

Write the complete ionic equation:

Combine the ionic equations for the reactants and exclude spectator ions:

Pb²⁺(aq) + 2ClO₄⁻(aq) + 2Na⁺(aq) + S²⁻(aq) → PbS(s) + 2Na⁺(aq) + 2ClO₄⁻(aq)

Therefore, the complete ionic equation shows the actual participating ions and accurately represents the reaction between lead perchlorate and sodium sulfide.

Option B is answer.