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Chapter 8: Problem 12

Aqueous solutions of lead nitrate and sodium sulfate combine to produce a precipitate. (a) What are the spectator ions? (b) Write the net ionic equation for this precipitation reaction.

Short Answer

Expert verified
(a) The spectator ions are sodium (Na⁺) and nitrate (NO₃⁻). (b) The net ionic equation is: \(Pb^{2+}(aq) + SO_4^{2-}(aq) \rightarrow PbSO_4(s)\).

Step by step solution

01

Write the balanced chemical equation

Write the balanced chemical equation for the reaction between aqueous lead nitrate and sodium sulfate. The reactants are lead nitrate (Pb(NO₃)₂) and sodium sulfate (Na₂SO₄), and their products are lead sulfate (PbSO₄, the precipitate) and sodium nitrate (NaNO₃). The balanced chemical equation is: Pb(NO₃)₂(aq) + Na₂SO₄(aq) → PbSO₄(s) + 2NaNO₃(aq)
02

Identify the spectator ions

The spectator ions are the ions that remain unchanged during the chemical reaction (i.e., the ones that do not participate in forming the product). In this reaction, sodium (Na⁺) and nitrate (NO₃⁻) ions are the spectator ions, as they remain in the solution and do not form the precipitate of lead sulfate.
03

Write the complete ionic equation

Rewrite the chemical equation by listing all the ions present in the reaction (excluding the solid precipitate). The equation becomes: Pb²⁺(aq) + 2NO₃⁻(aq) + 2Na⁺(aq) + SO₄²⁻(aq) → PbSO₄(s) + 2Na⁺(aq) + 2NO₃⁻(aq)
04

Write the net ionic equation

To write the net ionic equation, remove the spectator ions (Na⁺ and NO₃⁻) from both sides of the complete ionic equation. The net ionic equation is: Pb²⁺(aq) + SO₄²⁻(aq) → PbSO₄(s) This net ionic equation shows the formation of the precipitate (PbSO₄) from aqueous lead ions (Pb²⁺) and sulfate ions (SO₄²⁻).

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Most popular questions from this chapter

You need calcium sulfate, but there is none in the lab. However, there are lots of other ionic compounds on the shelves. (a) Propose a synthesis for calcium sulfate. (b) Write a complete ionic equation for the synthesis. (c) Write a net ionic equation for the synthesis. (d) Write the equation you wrote for (b) as an English sentence.

Balance each equation: (a) \(\mathrm{Zn}+\mathrm{HCl} \rightarrow \mathrm{ZnCl}_{2}+\mathrm{H}_{2}\) (b) \(\mathrm{Na}_{2} \mathrm{O}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{NaOH}\) (c) \(\mathrm{CH}_{4}+\mathrm{H}_{2} \mathrm{~S} \rightarrow \mathrm{CS}_{2}+\mathrm{H}_{2}\) (d) \(\mathrm{CO}+\mathrm{H}_{2} \rightarrow \mathrm{CH}_{3} \mathrm{O} \mathrm{H}\)

Balance this chemical equation by inspection: \(\mathrm{C}_{2} \mathrm{H}_{4}+\mathrm{O}_{2} \rightarrow \mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}\)

Write the complete ionic equation and net ionic equation for the neutralization reaction between aqueous hydrobromic acid and barium hydroxide.

Nitrous oxide, \(\mathrm{N}_{2} \mathrm{O}\), is produced when ammonium nitrate, \(\mathrm{NH}_{4} \mathrm{NO}_{3}\), is heated gently. Water is also produced in the reaction. Write the balanced equation for the reaction.
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