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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
In the reaction between solid cadmium sulfide (CdS) and an aqueous solution of sulfuric acid (H2SO4), the balanced molecular equation is: \(CdS (s) + H2SO4 (aq) \rightarrow CdSO4 (aq) + H2S (g)\). The net ionic equation is: \(CdS (s) + 2H^+ (aq) \rightarrow Cd^{2+} (aq) + H2S (g)\). The gas formed is hydrogen sulfide (H2S). In the reaction between solid magnesium carbonate (MgCO3) and an aqueous solution of perchloric acid (HClO4), the balanced molecular equation is: \(MgCO3 (s) + 2HClO4 (aq) \rightarrow Mg(ClO4)2 (aq) + CO2 (g) + H2O (l)\). The net ionic equation is: \(MgCO3 (s) + 2H^+ (aq) \rightarrow Mg^{2+} (aq) + CO2 (g) + H2O (l)\). The gas formed is carbon dioxide (CO2).

Step by step solution

01

(Reaction a: Cadmium sulfide with sulfuric acid)

The reaction between solid cadmium sulfide (CdS) and an aqueous solution of sulfuric acid (H2SO4) can be represented as follows: CdS (s) + H2SO4 (aq) -> ? In this reaction, cadmium sulfide (a solid) reacts with sulfuric acid (an aqueous solution) to produce a cadmium sulfate (CdSO4) and hydrogen sulfide (H2S) gas. The balanced molecular equation for this reaction is: CdS (s) + H2SO4 (aq) -> CdSO4 (aq) + H2S (g) Now, let's determine the net ionic equation by identifying the spectator ions and removing them from the equation. The net ionic equation includes only the aqueous ions that undergo a chemical change. For this reaction, the net ionic equation is: CdS (s) + 2H^+ (aq) + SO4^2- (aq) -> Cd^2+(aq) + SO4^2- (aq) + H2S (g) Removing the common ion (spectator ion) SO4^2- from both sides of the equation, the final net ionic equation becomes: CdS (s) + 2H^+ (aq) -> Cd^2+ (aq) + H2S (g)
02

(Reaction b: Magnesium carbonate with perchloric acid)

The reaction between solid magnesium carbonate (MgCO3) and an aqueous solution of perchloric acid (HClO4) can be represented as follows: MgCO3 (s) + HClO4 (aq) -> ? In this reaction, magnesium carbonate (a solid) reacts with perchloric acid (an aqueous solution) to produce magnesium perchlorate (Mg(ClO4)2) and carbon dioxide (CO2) gas. The balanced molecular equation for this reaction is: MgCO3 (s) + 2HClO4 (aq) -> Mg(ClO4)2 (aq) + CO2 (g) + H2O (l) Now, let's determine the net ionic equation by identifying the spectator ions and removing them from the equation. The net ionic equation includes only the aqueous ions that undergo a chemical change. For this reaction, the net ionic equation is: MgCO3 (s) + 2H^+ (aq) + 2ClO4^- (aq) -> Mg^2+(aq) + 2ClO4^-(aq) + CO2 (g) + H2O (l) Removing the common ion (spectator ion) 2ClO4^- from both sides of the equation, the final net ionic equation becomes: MgCO3 (s) + 2H^+ (aq) -> Mg^2+ (aq) + CO2 (g) + H2O (l) So, in conclusion: a) The gas formed in the reaction between solid cadmium sulfide and an aqueous solution of sulfuric acid is hydrogen sulfide (H2S). b) The gas formed in the reaction between solid magnesium carbonate and an aqueous solution of perchloric acid is carbon dioxide (CO2).

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Most popular questions from this chapter

The arsenic in a 1.22-g sample of a pesticide was converted to \(\mathrm{AsO}_{4}^{3-}\) by suitable chemical treatment. It was then titrated using \(\mathrm{Ag}^{+}\) to form \(\mathrm{Ag}_{3} \mathrm{AsO}_{4}\) as a precipitate. (a) What is the oxidation state of As in \(\mathrm{AsO}_{4}{ }^{3-} ?\) (b) Name \(\mathrm{Ag}_{3} \mathrm{AsO}_{4}\) by analogy to the corresponding compound containing phosphorus in place of arsenic. (c) If it took \(25.0 \mathrm{~mL}\) of \(0.102 \mathrm{M} \mathrm{Ag}^{+}\) to reach the equivalence point in this titration, what is the mass percentage of arsenic in the pesticide?

A \(1.248-\mathrm{g}\) sample of limestone rock is pulverized and then treated with \(30.00 \mathrm{~mL}\) of \(1.035 \mathrm{M} \mathrm{HCl}\) solution. The excess acid then requires \(11.56 \mathrm{~mL}\) of \(1.010 \mathrm{M} \mathrm{NaOH}\) for neutralization. Calculate the percent by mass of calcium carbonate in the rock, assuming that it is the only substance reacting with the HCl solution.

Indicate the concentration of each ion present in the solution formed by mixing (a) \(42.0 \mathrm{~mL}\) of \(0.170 \mathrm{M} \mathrm{NaOH}\) and \(37.6 \mathrm{~mL}\) of \(0.400 \mathrm{M} \mathrm{NaOH}\), (b) \(44.0 \mathrm{~mL}\) of \(0.100 \mathrm{M}\) and \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and \(25.0 \mathrm{~mL}\) of \(0.150 \mathrm{M} \mathrm{KCl},(\mathrm {c}) 3.60 \mathrm{~g} \mathrm{KCl}\) in \(75.0 \mathrm{~mL}\) of \(0.250 \mathrm{M}\) \(\mathrm{CaCl}_{2}\) solution. Assume that the volumes are additive.

Calculate (a) the number of grams of solute in \(0.250 \mathrm{~L}\) of \(0.175 \mathrm{M} \mathrm{KBr},\) (b) the molar concentration of a solution containing \(14.75 \mathrm{~g}\) of \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) in \(1.375 \mathrm{~L},\) (c) the volume of \(1.50 \mathrm{M} \mathrm{Na}_{3} \mathrm{PO}_{4}\) in milliliters that contains \(2.50 \mathrm{~g}\) of solute.

You are presented with a white solid and told that due to careless labeling it is not clear if the substance is barium chloride, lead chloride, or zinc chloride. When you transfer the solid to a beaker and add water, the solid dissolves to give a clear solution. Next a \(\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)\) solution is added and a white precipitate forms. What is the identity of the unknown white solid? \([\) Section 4.2\(]\)
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