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Chapter 17: Problem 9

Write balanced net ionic equations for the following reactions in acid solution. (a) Liquid hydrazine reacts with an aqueous solution of sodium bromate. Nitrogen gas and bromide ions are formed. (b) Solid phosphorus \(\left(\mathrm{P}_{4}\right)\) reacts with an aqueous solution of nitrate to form nitrogen oxide gas and dihydrogen phosphate \(\left(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\right)\) ions. (c) Aqueous solutions of potassium sulfite and potassium permanganate react. Sulfate and manganese(II) ions are formed.

Short Answer

Expert verified
Question: Write the balanced net ionic equations for the following acid solution reactions: (a) Liquid hydrazine (\(N_2H_4\)) reacts with sodium bromate (\(NaBrO_3\)) to form nitrogen gas (\(N_2\)) and bromide ions (\(Br^-\)). (b) Solid phosphorus (\(P_4\)) reacts with nitrate (\(NO_3^-\)) to form nitrogen oxide gas (\(NO\)) and dihydrogen phosphate ions (\(H_2PO_4^-\)). (c) Potassium sulfite (\(K_2SO_3\)) reacts with potassium permanganate (\(KMnO_4\)) in an acidic solution to form sulfate (\(SO_4^{2-}\)) and manganese(II) ions (\(Mn^{2+}\)). Answers: (a) The balanced net ionic equation for the reaction between liquid hydrazine and sodium bromate in an acidic solution is: $$N_2H_4 + 2BrO_3^- + 8H^+ \to 2N_2 + 2Br^- + 8H_2O$$ (b) The balanced net ionic equation for the reaction between solid phosphorus and nitrate is: $$P_4 + 20NO_3^- + 20H^+ \to 20NO + 4H_2PO_4^-$$ (c) The balanced net ionic equation for the reaction between potassium sulfite and potassium permanganate in an acidic solution is: $$3SO_3^{2-} + 2MnO_4^- + 6H^+ \to 3SO_4^{2-} + 2Mn^{2+} + 8H_2O$$

Step by step solution

01

(a) Balanced Molecular Equation

First, let's write the balanced molecular equation for the reaction between liquid hydrazine \((N_2H_4)\) and sodium bromate \((NaBrO_3)\) in an acidic solution. We are given that nitrogen gas \((N_2)\) and bromide ions \((Br^-)\) are formed. The balanced molecular equation is: $$N_2H_4 + 2NaBrO_3 + 8H^+ \to 2N_2 + 2NaBr + 8H_2O$$
02

(a) Total Ionic Equation

Now, let's write the total ionic equation by breaking all species into their respective ions: $$N_2H_4 + 2Na^+ + 2BrO_3^- + 8H^+ \to 2N_2 + 2Na^+ + 2Br^- + 8H_2O$$
03

(a) Net Ionic Equation

Eliminate the spectator ions from the total ionic equation to find the net ionic equation. Spectator ions: \(2Na^+\) Net ionic equation: $$N_2H_4 + 2BrO_3^- + 8H^+ \to 2N_2 + 2Br^- + 8H_2O$$
04

(b) Balanced Molecular Equation

Now, let's write the balanced molecular equation for the reaction between solid phosphorus \((P_4)\) and nitrate \((NO_3^-)\). We are given that nitrogen oxide gas \((NO)\) and dihydrogen phosphate ions \((H_2PO_4^-)\) are formed. The balanced molecular equation is: $$P_4 + 20NO_3^- + 20H^+ \to 20NO + 4H_2PO_4^-$$
05

(b) Total Ionic Equation

Since solid phosphorus and nitrogen oxide gas do not dissociate into ions, we do not need to break them up. The total ionic equation is: $$P_4 + 20NO_3^- + 20H^+ \to 20NO + 4H_2PO_4^-$$
06

(b) Net Ionic Equation

As there are no spectator ions in this reaction, the net ionic equation is the same as the total ionic equation: $$P_4 + 20NO_3^- + 20H^+ \to 20NO + 4H_2PO_4^-$$
07

(c) Balanced Molecular Equation

Let's write the balanced molecular equation for the reaction between potassium sulfite \((K_2SO_3)\) and potassium permanganate \((KMnO_4)\) in an acidic solution. We are given that sulfate \((SO_4^{2-})\) and manganese(II) ions \((Mn^{2+})\) are formed. The balanced molecular equation is: $$3K_2SO_3 + 2KMnO_4 + 6H^+ \to 3K_2SO_4 + 2Mn^{2+} + 8H_2O$$
08

(c) Total Ionic Equation

Now, let's write the total ionic equation by breaking all species into their respective ions: $$6K^+ + 3SO_3^{2-} + 2K^+ + 2MnO_4^- + 6H^+ \to 6K^+ + 3SO_4^{2-} + 2Mn^{2+} + 8H_2O$$
09

(c) Net Ionic Equation

Eliminate the spectator ions from the total ionic equation to find the net ionic equation. Spectator ions: \(6K^+\) Net ionic equation: $$3SO_3^{2-} + 2MnO_4^- + 6H^+ \to 3SO_4^{2-} + 2Mn^{2+} + 8H_2O$$

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Most popular questions from this chapter

Which of the changes below will increase the voltage of the following cell? \(\mathrm{Co}\left|\mathrm{Co}^{2+}(0.010 \mathrm{M}) \| \mathrm{H}^{+}(0.010 \mathrm{M})\right| \mathrm{H}_{2}(0.500 \mathrm{~atm}) \mid \mathrm{Pt}\) (a) Increase the volume of \(\mathrm{CoCl}_{2}\) solution from \(100 \mathrm{~mL}\) to \(300 \mathrm{~mL}\). (b) Increase \(\left[\mathrm{H}^{+}\right]\) from \(0.010 \mathrm{M}\) to \(0.500 \mathrm{M}\). (c) Increase the pressure of \(\mathrm{H}_{2}\) from 0.500 atm to \(1 \mathrm{~atm}\). (d) Increase the mass of the Co electrode from \(15 \mathrm{~g}\) to \(25 \mathrm{~g}\). (e) Increase \(\left[\mathrm{Co}^{2+}\right]\) from \(0.010 \mathrm{M}\) to \(0.500 \mathrm{M}\).

Write balanced equations for the following reactions in acid solution. (a) \(\mathrm{Ni}^{2+}(a q)+\mathrm{IO}_{4}^{-}(a q) \longrightarrow \mathrm{Ni}^{3+}(a q)+\mathrm{I}^{-}(a q)\) (b) \(\mathrm{O}_{2}(g)+\mathrm{Br}^{-}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}+\mathrm{Br}_{2}(l)\) (c) \(\mathrm{Ca}(s)+\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q) \longrightarrow \mathrm{Ca}^{2+}(a q)+\mathrm{Cr}^{3+}(a q)\) (d) \(\mathrm{IO}_{3}^{-}(a q)+\mathrm{Mn}^{2+}(a q) \longrightarrow \mathrm{I}^{-}(a q)+\mathrm{MnO}_{2}(s)\)

Consider the reaction for the formation of the complex ion \(\mathrm{CuCl}_{2}^{-}\). $$ \mathrm{Cu}^{+}(s)+2 \mathrm{Cl}^{-}(a q) \rightarrow \mathrm{CuCl}_{2}^{-}(a q) $$ The formation constant \(K_{\mathrm{f}}\) for this reaction is \(3.0 \times 10^{5} .\) (a) Write the two half-reactions that give rise to the formation of the complex ion. (b) Find the standard reduction potential at \(25^{\circ} \mathrm{C}\) for the reaction.

Follow the directions in Question 17 for a salt bridge cell in which the anode is a platinum rod immersed in an aqueous solution of sodium iodide containing solid iodine crystals. The cathode is another platinum rod immersed in an aqueous solution of sodium bromide with bromine liquid.

Write balanced net ionic equations for the following reactions in basic medium. (a) \(\mathrm{Ca}(s)+\mathrm{VO}_{4}^{3-}(a q) \longrightarrow \mathrm{Ca}^{2+}(a q)+\mathrm{V}^{2+}(a q)\) (b) \(\mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{BiO}_{3}^{-}(a q) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{Bi}^{3+}(a q)\) (c) \(\mathrm{PbO}_{2}(s)+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{O}_{2}(g)+\mathrm{Pb}^{2+}\) (b) \(\mathrm{IO}_{3}^{-}(a q)+\mathrm{Cl}^{-}(a q) \longrightarrow \mathrm{Cl}_{2}(g)+\mathrm{I}_{3}^{-}(a q)\)
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