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Chapter 5: Problem 106

What is the net ionic equation for the reaction that occurs when an aqueous solution of \(\mathrm{KI}\) is added to an aqueous solution of \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2} ?\)

Short Answer

Expert verified
The net ionic equation for the reaction that occurs when an aqueous solution of \(\mathrm{KI}\) is added to an aqueous solution of \(\mathrm{Pb(NO}_3)_2\) is \[2 \, \mathrm{I^-} + Pb^{2+} = \mathrm{PbI}_2(s)\]

Step by step solution

01

Write down the molecular equation

First, write down the molecular equation. Potassium iodide reacts with lead nitrate to produce lead iodide(which is a precipitate) and potassium nitrate. This translates to the following equation: \[2 \, \mathrm{KI} + \, \mathrm{Pb(NO}_3)_2 \, \rightarrow \, \mathrm{PbI}_2 + 2 \, \mathrm{KNO}_3\] This equation indicates that for each molecule of lead nitrate in solution, two molecules of potassium iodide are needed to produce one molecule of lead iodide and two molecules of potassium nitrate.
02

Write down the total ionic equation

The next step is to write down the ionic equation, which includes all of the ions present in the reaction: \[2 \, \mathrm{K^+} + 2 \, \mathrm{I^-} + Pb^{2+} + 2 \, \mathrm{NO}_3^- \, \rightarrow \, Pb \, \mathrm{I}_2(s) + 2 \, \mathrm{K^+} + 2 \, \mathrm{NO}_3^-\] The (s) next to \(PbI_2\) indicates that it is a solid (precipitate), while the other ions are all in aqueous solution.
03

Write down the net ionic equation

The net ionic equation is obtained by cancelling out the spectator ions that don’t participate in the reaction. In this case, the potassium ions \( \mathrm{K^+} \) and nitrate ions \( \mathrm{NO}_3^- \) are spectator ions. Removing these gives the net ionic equation: \[2 \, \mathrm{I^-} + Pb^{2+} \, \rightarrow \, \mathrm{PbI}_2(s)\] This equation indicates that in the reaction, lead ions combined with iodide ions to form the precipitate, lead iodide.

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Most popular questions from this chapter

Which of the following reactions are oxidationreduction reactions? (a) \(\mathrm{H}_{2} \mathrm{CO}_{3}(\mathrm{aq}) \longrightarrow \mathrm{H}_{2} \mathrm{O}(1)+\mathrm{CO}_{2}(\mathrm{g})\) (b) \(2 \mathrm{Li}(\mathrm{s})+2 \mathrm{H}_{2} \mathrm{O}(1) \longrightarrow 2 \mathrm{LiOH}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{g})\) (c) \(4 \mathrm{Ag}(\mathrm{s})+\mathrm{PtCl}_{4}(\mathrm{aq}) \longrightarrow 4 \mathrm{AgCl}(\mathrm{s})+\mathrm{Pt}(\mathrm{s})\) (d) \(2 \mathrm{HClO}_{4}(\mathrm{aq})+\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{aq}) \longrightarrow\) \(2 \mathrm{H}_{2} \mathrm{O}(1)+\mathrm{Ca}\left(\mathrm{ClO}_{4}\right)_{2}(\mathrm{aq})\)

What volume of \(0.0962 \mathrm{M} \mathrm{NaOH}\) is required to exactly neutralize \(10.00 \mathrm{mL}\) of \(0.128 \mathrm{M} \mathrm{HCl} ?\)

Which solution has the greatest \(\left[\mathrm{SO}_{4}^{2-}\right]:\) (a) \(0.075 \mathrm{M}\) \(\mathrm{H}_{2} \mathrm{SO}_{4} ; \quad\) (b) \(\quad 0.22 \mathrm{M} \mathrm{MgSO}_{4} ; \quad\) (c) \(\quad 0.15 \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{4}\) (d) \(0.080 \mathrm{M} \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} ;\) (e) \(0.20 \mathrm{M} \mathrm{CuSO}_{4} ?\)

Explain why these reactions cannot occur as written. (a) \(\mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{MnO}_{4}^{-}(\mathrm{aq})+\mathrm{H}^{+}(\mathrm{aq}) \longrightarrow\) \(\mathrm{Mn}^{2+}(\mathrm{aq})+\mathrm{Fe}^{2+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(1)\) (b) \(\mathrm{H}_{2} \mathrm{O}_{2}(\mathrm{aq})+\mathrm{Cl}_{2}(\mathrm{aq}) \longrightarrow\) \(\mathrm{ClO}^{-}(\mathrm{aq})+\mathrm{O}_{2}(\mathrm{g})+\mathrm{H}^{+}(\mathrm{aq})\)

Following are some laboratory methods occasionally used for the preparation of small quantities of chemicals. Write a balanced equation for each. (a) preparation of \(\mathrm{H}_{2} \mathrm{S}(\mathrm{g}): \mathrm{HCl}(\mathrm{aq})\) is heated with \(\mathrm{FeS}(\mathrm{s})\) (b) preparation of \(\mathrm{Cl}_{2}(\mathrm{g}): \mathrm{HCl}(\mathrm{aq})\) is heated with \(\mathrm{MnO}_{2}(\mathrm{s}) ; \mathrm{MnCl}_{2}(\mathrm{aq})\) and \(\mathrm{H}_{2} \mathrm{O}(1)\) are other products (c) preparation of \(\mathrm{N}_{2}: \mathrm{Br}_{2}\) and \(\mathrm{NH}_{3}\) react in aqueous solution; \(\mathrm{NH}_{4} \mathrm{Br}\) is another product (d) preparation of chlorous acid: an aqueous suspension of solid barium chlorite is treated with dilute \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})\)
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