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Chapter 4: Problem 42

Because the oxide ion is basic, metal oxides react readily with acids. (a) Write the net ionic equation for the following reaction: $$ \mathrm{FeO}(s)+2 \mathrm{HClO}_{4}(a q) \longrightarrow \mathrm{Fe}\left(\mathrm{ClO}_{4}\right)_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) $$ (b) Based on the equation in part (a), write the net ionic equation for the reaction that occurs between \(\mathrm{NiO}(s)\) and an aqueous solution of nitric acid.

Short Answer

Expert verified
(a) The net ionic equation for the reaction between FeO and HClO4 is: \( FeO(s) + 2 H^+(aq) \longrightarrow Fe^{2+}(aq) + H_2O(l) \) (b) The net ionic equation for the reaction between NiO and nitric acid is: \( NiO(s) + 2 H^+(aq) \longrightarrow Ni^{2+}(aq) + H_2O(l) \)

Step by step solution

01

Identify the strong electrolytes

In the given reaction, we need to identify the strong electrolytes, which are HClO4. Strong electrolytes dissociate into their ions completely in an aqueous solution.
02

Dissociate the strong electrolytes into their ions

The strong electrolyte HClO4 can be dissociated as follows: \( 2 HClO_4 \longrightarrow 2 H^+ + 2 ClO_4^- \) For FeO, it should be noted that we cannot dissociate it into its ions because it is a solid metal oxide.
03

Write the complete ionic equation

Now, write the complete ionic equation by replacing the strong electrolytes with their dissociated ions: \( FeO (s) + 2 H^+ (aq) + 2 ClO_4^- (aq) \longrightarrow Fe^{2+} (aq) + 2 ClO_4^- (aq) + H_2O (l) \)
04

Identify and remove the spectator ions

Observe the complete ionic equation to identify the spectator ions. In this case, the spectator ion is ClO4-. Spectator ions are the ions that remain the same in the reactants and products. They can be removed to write the net ionic equation.
05

Write the net ionic equation

Remove the spectator ions and write the net ionic equation for the given reaction: \( FeO(s) + 2 H^+(aq) \longrightarrow Fe^{2+}(aq) + H_2O(l) \) Now, let's move on to part (b) of the exercise. (b):
06

Write the balanced reaction equation between NiO and nitric acid

The balanced reaction between NiO (s) and nitric acid (HNO3) can be written as: \( NiO(s) + 2 HNO_3(aq) \longrightarrow Ni(NO_3)_2(aq) + H_2O(l) \)
07

Identify the strong electrolytes and dissociate them

Nitric acid (HNO3) is a strong electrolyte. It dissociates into its ions completely in an aqueous solution: \( 2 HNO_3 \longrightarrow 2 H^+ + 2 NO_3^- \)
08

Write the complete ionic equation

Now, we can write the complete ionic equation: \( NiO(s) + 2 H^+(aq) + 2 NO_3^-(aq) \longrightarrow Ni^{2+}(aq) + 2 NO_3^-(aq) + H_2O(l) \)
09

Identify and remove the spectator ions

The spectator ion in this reaction is NO3-. By removing the spectator ions, we can write the net ionic equation.
10

Write the net ionic equation

Remove the spectator ions and write the net ionic equation for the reaction between NiO and nitric acid: \( NiO(s) + 2 H^+(aq) \longrightarrow Ni^{2+}(aq) + H_2O(l) \)

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Strong Electrolytes
Strong electrolytes are substances that completely dissociate into ions when dissolved in water. This complete dissociation means that they conduct electricity well in solution because there are many free ions to carry the charge. A good example from the exercise is perchloric acid,
often represented as HClO鈧�, and nitric acid,
HNO鈧�. Both are strong acids and thus, strong electrolytes. When they dissolve in water, they break down completely into their constituent ions:
- HClO鈧� dissociates into H鈦� and ClO鈧勨伝 ions. - HNO鈧� dissociates into H鈦� and NO鈧冣伝 ions. Knowing that a substance is a strong electrolyte helps in predicting the outcome of reactions, particularly when writing balanced and net ionic equations.
Spectator Ions
In chemical reactions, spectator ions are ions present in solution that do not participate in the reaction. They remain unchanged during the process. Identifying these ions is crucial while writing net ionic equations because they are eliminated from the equation, simplifying it to show only the reacting species.
Take the initial reaction for example: After dissociating HClO鈧�, the ClO鈧勨伝 ions do not engage in the chemical change and are therefore spectator ions. Similarly, in the reaction involving NiO and HNO鈧�, the NO鈧冣伝 ions are spectator ions because they do not take part in the central reaction between NiO and H鈦� ions.
Removing spectators, like ClO鈧勨伝 and NO鈧冣伝, helps us focus on the essential chemical changes, making it clearer to understand what actually happens in a reaction.
Metal Oxides
Metal oxides, such as FeO and NiO in the given problems, are solid compounds formed by metals bonded with oxygen. These oxides often exhibit basic characteristics, especially when interacting with acids.
In acidic reactions, these metal oxides typically undergo transformations where they react with hydrogen ions ( H鈦�) provided by the acidic solution, forming water and the soluble metal ions:
  • FeO reacts with H鈦� ions to produce Fe虏鈦� ions and water.
  • NiO reacts with H鈦� ions to yield Ni虏鈦� ions and water.
These reactions with metal oxides are key to forming the net ionic equations by showing only the necessary species. The metal ions in such reactions change their oxidation state, indicating a transfer of electrons, which is an essential part of understanding redox reactions and acid-base behavior of oxides.

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Most popular questions from this chapter

The commercial production of nitric acid involves the following chemical reactions: $$ \begin{aligned} 4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) & \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g) \\ 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) & \longrightarrow 2 \mathrm{NO}_{2}(g) \\ 3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) & \longrightarrow 2 \mathrm{HNO}_{3}(a q)+\mathrm{NO}(g) \end{aligned} $$ (a) Which of these reactions are redox reactions? (b) In each redox reaction identify the element undergoing oxidation and the element undergoing reduction. (c) How many grams of ammonia must you start with to make \(1000.0 \mathrm{~L}\) of a \(0.150 \mathrm{M}\) aqueous solution of nitric acid? Assume all the reactions give \(100 \%\) yield.

State whether each of the following statements is true or false. Justify your answer in each case. (a) When acetone, \(\mathrm{CH}_{3} \mathrm{COCH}_{3}\), is dissolved in water, a conducting solution results. (b) When ammonium nitrate, \(\mathrm{NH}_{4} \mathrm{NO}_{3}\), dissolves in water, the solution is weakly conducting and basic in nature.

Would you expect that an anion would be physically closer to the oxygen or to the hydrogens of water molecules that surround it in solution?

Label each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance existsin aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions. (a) HF, (b) acetonitrile, \(\mathrm{CH}_{3} \mathrm{CN},(\mathbf{c}) \mathrm{NaClO}_{4},\) (d) \(\mathrm{Ba}(\mathrm{OH})_{2} \cdot\)

(a) By titration, \(15.0 \mathrm{~mL}\) of \(0.1008 \mathrm{Msodium}\) hydroxide is needed to neutralizea \(0.2053-\mathrm{g}\) sample of a weak acid. What is the molar mass of the acid if it is monoprotic? (b) An elemental analysis of the acid indicates that it is composed of \(5.899 \mathrm{H}, 70.6 \% \mathrm{C},\) and \(23.5 \% \mathrm{O}\) by mass. What is its molecular formula?
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