Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react with acidic solutions. (a) Write a balanced molecular equation and a net ionic equation for the reaction that occurs when each substance reacts with a hydrochloric acid solution. (b) By observing the reactions in part (a) could you distinguish any of the three magnesium substances from the other two? If so how? (c) If excess \(\mathrm{HCl}(a q)\) is added, would the clear solutions left behind after the reaction is complete contain the same or different ions in each case?

Short Answer

Expert verified
The reactions of magnesium carbonate, magnesium oxide, and magnesium hydroxide with hydrochloric acid produce the following net ionic equations: 1. \(MgCO_{3(s)} + 2H^+_{(aq)} \rightarrow Mg^{2+}_{(aq)} + H_{2}O_{(l)} + CO_{2(g)}\) 2. \(MgO_{(s)} + 2H^+_{(aq)} \rightarrow Mg^{2+}_{(aq)} + H_{2}O_{(l)} \) 3. \(Mg(OH)_{2(s)} + 2H^+_{(aq)} \rightarrow Mg^{2+}_{(aq)} + 2H_{2}O_{(l)} \) It is not possible to distinguish the magnesium substances based solely on their reactions, as they all produce similar products. If excess hydrochloric acid is added, the clear solutions left behind will all contain the same ions: \(Mg^{2+}\) and \(Cl^-\).

Step by step solution

01

Molecular and Net Ionic Equations for Magnesium Carbonate Reaction

1. Write the molecular equation for the reaction of magnesium carbonate with hydrochloric acid: \(MgCO_{3(s)} + 2HCl_{(aq)} \rightarrow MgCl_{2(aq)} + H_{2}O_{(l)} + CO_{2(g)} \) 2. Remove spectator ions to obtain the net ionic equation: \(MgCO_{3(s)} + 2H^+_{(aq)} \rightarrow Mg^{2+}_{(aq)} + H_{2}O_{(l)} + CO_{2(g)} \)
02

Molecular and Net Ionic Equations for Magnesium Oxide Reaction

1. Write the molecular equation for the reaction of magnesium oxide with hydrochloric acid: \(MgO_{(s)} + 2HCl_{(aq)} \rightarrow MgCl_{2(aq)} + H_{2}O_{(l)} \) 2. Remove spectator ions to obtain the net ionic equation: \(MgO_{(s)} + 2H^+_{(aq)} \rightarrow Mg^{2+}_{(aq)} + H_{2}O_{(l)} \)
03

Molecular and Net Ionic Equations for Magnesium Hydroxide Reaction

1. Write the molecular equation for the reaction of magnesium hydroxide with hydrochloric acid: \(Mg(OH)_{2(s)} + 2HCl_{(aq)} \rightarrow MgCl_{2(aq)} + 2H_{2}O_{(l)} \) 2. Remove spectator ions to obtain the net ionic equation: \(Mg(OH)_{2(s)} + 2H^+_{(aq)} \rightarrow Mg^{2+}_{(aq)} + 2H_{2}O_{(l)} \)
04

Distinguishing Magnesium Substances

It is not possible to distinguish the three magnesium substances based solely on their reactions with hydrochloric acid, as the molecular and net ionic equations all produce magnesium chloride and water, and the only difference is that magnesium carbonate also releases carbon dioxide.
05

Ions in the Clear Solutions

If excess hydrochloric acid is added, all three reactions will go to completion, and the clear solutions left behind will all contain the same ions: \(Mg^{2+}\) and \(Cl^-\), as all three reactions produce magnesium chloride in solution.

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