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Chapter 4: Problem 41

Write balanced molecular and net ionic equations for the following reactions, and identify the gas formed in each: (a) solid cadmium sulfide reacts with an aqueous solution of sulfuric acid; (b) solid magnesium carbonate reacts with an aqueous solution of perchloric acid.

Short Answer

Expert verified
The balanced net ionic equations for the given reactions are: (a) \(CdS_{(s)} + 2H^+_{(aq)} \rightarrow Cd^{2+}_{(aq)} + H_2S_{(g)}\) with hydrogen sulfide (H2S) gas formed. (b) \(MgCO_3_{(s)} + 2H^+_{(aq)} \rightarrow Mg^{2+}_{(aq)} + CO_2_{(g)}\) with carbon dioxide (CO2) gas formed.

Step by step solution

01

Write the unbalanced molecular equation

The given reaction can be represented as: \(CdS_{(s)} + H_2SO_4_{(aq)} \rightarrow\) products
02

Identify the products

Cadmium sulfide reacts with sulfuric acid to form cadmium sulfate and hydrogen sulfide gas: \(CdS_{(s)} + H_2SO_4_{(aq)} \rightarrow CdSO_4_{(aq)} + H_2S_{(g)}\)
03

Balance the molecular equation

The equation is already balanced: \(CdS_{(s)} + H_2SO_4_{(aq)} \rightarrow CdSO_4_{(aq)} + H_2S_{(g)}\)
04

Write the complete ionic equation

As the reaction occurs in aqueous solution, dissociate the strong electrolytes: \(CdS_{(s)} + 2H^+_{(aq)} + SO_4^{2-}_{(aq)} \rightarrow Cd^{2+}_{(aq)} + SO_4^{2-}_{(aq)} + H_2S_{(g)}\)
05

Write the net ionic equation

Remove spectator ions, which are the same on both sides of the equation: \(CdS_{(s)} + 2H^+_{(aq)} \rightarrow Cd^{2+}_{(aq)} + H_2S_{(g)}\) The balanced net ionic equation is: \(CdS_{(s)} + 2H^+_{(aq)} \rightarrow Cd^{2+}_{(aq)} + H_2S_{(g)}\) The gas formed is hydrogen sulfide (H2S). (b) Solid magnesium carbonate reacts with an aqueous solution of perchloric acid:
06

Write the unbalanced molecular equation

The given reaction can be represented as: \(MgCO_3_{(s)} + HClO_4_{(aq)} \rightarrow\) products
07

Identify the products

Magnesium carbonate reacts with perchloric acid to form magnesium perchlorate and carbon dioxide gas: \(MgCO_3_{(s)} + HClO_4_{(aq)} \rightarrow Mg(ClO_4)_2_{(aq)} + CO_2_{(g)}\)
08

Balance the molecular equation

Balance the equation by adding coefficients: \(MgCO_3_{(s)} + 2HClO_4_{(aq)} \rightarrow Mg(ClO_4)_2_{(aq)} + CO_2_{(g)}\)
09

Write the complete ionic equation

As the reaction occurs in aqueous solution, dissociate the strong electrolytes: \(MgCO_3_{(s)} + 2H^+_{(aq)} + 2ClO_4^-_{(aq)} \rightarrow Mg^{2+}_{(aq)} + 2ClO_4^-_{(aq)} + CO_2_{(g)}\)
10

Write the net ionic equation

Remove spectator ions, which are the same on both sides of the equation: \(MgCO_3_{(s)} + 2H^+_{(aq)} \rightarrow Mg^{2+}_{(aq)} + CO_2_{(g)}\) The balanced net ionic equation is: \(MgCO_3_{(s)} + 2H^+_{(aq)} \rightarrow Mg^{2+}_{(aq)} + CO_2_{(g)}\) The gas formed is carbon dioxide (CO2).

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Most popular questions from this chapter

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 \(0.0105 \mathrm{M} \mathrm{HCl}\). The \(\mathrm{NH}_{3}\) reacts with \(\mathrm{HCl}\) 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?

A 3.455-g sample of a mixture was analyzed for barium ion by adding a small excess of sulfuric acid to an aqueous solution of the sample. The resultant reaction produced a precipitate of barium sulfate, which was collected by filtration, washed, dried, and weighed. If \(0.2815 \mathrm{~g}\) of barium sulfate was obtained, what was the mass percentage of barium in the sample?

A solid sample of \(\mathrm{Zn}(\mathrm{OH})_{2}\) is added to \(0.350 \mathrm{~L}\) of \(0.500 M\) aqueous HBr. The solution that remains is still acidic. It is then titrated with \(0.500 \mathrm{M} \mathrm{NaOH}\) solution, and it takes \(88.5 \mathrm{~mL}\) of the \(\mathrm{NaOH}\) solution to reach the equivalence point. What mass of \(\mathrm{Zn}(\mathrm{OH})_{2}\) was added to the \(\mathrm{HBr}\) solution?

Suppose you have \(5.00 \mathrm{~g}\) of powdered magnesium metal, \(1.00 \mathrm{~L}\) of \(2.00 \mathrm{M}\) potassium nitrate solution, and \(1.00 \mathrm{~L}\) of \(2.00 \mathrm{M}\) silver nitrate solution. (a) Which one of the solutions will react with the magnesium powder? (b) What is the net ionic equation that describes this reaction? (c) What volume of solution is needed to completely react with the magnesium? (d) What is the molarity of the \(\mathrm{Mg}^{2+}\) ions in the resulting solution?

(a) How many grams of solid silver nitrate would you need to prepare \(200.0 \mathrm{~mL}\) of a \(0.150 \mathrm{M} \mathrm{AgNO}_{3}\) solution? (b) An experiment calls for you to use \(100 \mathrm{~mL}\) of \(0.50 \mathrm{MHNO}_{3}\) solution. All you have available is a bottle of \(3.6 \mathrm{M} \mathrm{HNO}_{3}\). How many milliliters of the \(3.6 \mathrm{M} \mathrm{HNO}_{3}\) solution and of water do you need to prepare the desired solution?
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