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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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Most popular questions from this chapter

We have learned in this chapter that many ionic solids dissolve in water as strong electrolytes; that is, as separated ions in solution. Which statement is most correct about this process? (a) Water is a strong acid and therefore is good at dissolving ionic solids. (b) Water is good at solvating ions because the hydrogen and oxygen atoms in water molecules bear partial charges. (c) The hydrogen and oxygen bonds of water are easily broken by ionic solids.

Determine the oxidation number of sulfur in each of the following substances: (a) barium sulfate, \(\mathrm{BaSO}_{4},\) (b) sulfurous acid, $\mathrm{H}_{2} \mathrm{SO}_{3},(\mathbf{c})\( strontium sulfide, \)\mathrm{Sr} S,(\mathbf{d})$ hydrogen sulfide, \(\mathrm{H}_{2} \mathrm{~S}\). (e) Locate sulfur in the periodic table in Exercise 4.47 what region is it in? (f) Which region(s) of the periodic table contains elements that can adopt both positive and negative oxidation numbers?

You know that an unlabeled bottle contains an aqueous solution of one of the following: \(\mathrm{AgNO}_{3}, \mathrm{CaCl}_{2},\) or \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} . \mathrm{A}\) friend suggests that you test a portion of the solution with \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}\) and then with NaCl solutions. According to your friend's logic, which of these chemical reactions could occur, thus helping you identify the solution in the bottle? (a) Barium sulfate could precipitate. (b) Silver chloride could precipitate. (c) Silver sulfate could precipitate. (d) More than one, but not all, of the reactions described in answers a-c could occur. (e) All three reactions described in answers a-c could occur.

A fertilizer railroad car carrying \(129,840 \mathrm{~L}\) of commercial aqueous ammonia (30\% ammonia by mass) tips over and spills. The density of the aqueous ammonia solution is \(0.88 \mathrm{~g} / \mathrm{cm}^{3}\) What mass of citric acid, $\mathrm{C}(\mathrm{OH})(\mathrm{COOH})\left(\mathrm{CH}_{2} \mathrm{COOH}\right)_{2}$ (which contains three acidic protons) is required to neutralize the spill?

Federal regulations set an upper limit of 50 parts per million (ppm) of \(\mathrm{NH}_{3}\) in the air in a work environment [that is, 50 molecules of \(\mathrm{NH}_{3}(g)\) for every million molecules in the air]. Air from a manufacturing operation was drawn through a solution containing $1.00 \times 10^{2} \mathrm{~mL}\( of \)0.0105 \mathrm{MHCl} .\( The \)\mathrm{NH}_{3}$ reacts with HCl according to: $$ \mathrm{NH}_{3}(a q)+\mathrm{HCl}(a q) \longrightarrow \mathrm{NH}_{4} \mathrm{Cl}(a q) $$ After drawing air through the acid solution for \(10.0 \mathrm{~min}\) at a rate of \(10.0 \mathrm{~L} / \mathrm{min},\) the acid was titrated. The remaining acid needed \(13.1 \mathrm{~mL}\) of \(0.0588 \mathrm{M} \mathrm{NaOH}\) to reach the equivalence point. (a) How many grams of \(\mathrm{NH}_{3}\) were drawn into the acid solution? (b) How many ppm of \(\mathrm{NH}_{3}\) were in the air? (Air has a density of \(1.20 \mathrm{~g} / \mathrm{L}\) and an average molar mass of \(29.0 \mathrm{~g} / \mathrm{mol}\) under the conditions of the experiment.) (c) Is this manufacturer in compliance with regulations?
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