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Chapter 4: Problem 43

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), how could you distinguish any of the three magnesium substances from the other two?

Short Answer

Expert verified
Magnesium carbonate can be distinguished by the fizzing it produces when reacting with HCl, unlike magnesium oxide and magnesium hydroxide.

Step by step solution

01

Identify the Reactants

We need to determine the reactants involved in these reactions. All three substances mentioned (magnesium carbonate \(\text{MgCO}_3\), magnesium oxide \(\text{MgO}\), and magnesium hydroxide \(\text{Mg(OH)}_2\)) will react with hydrochloric acid (\(\text{HCl}\)).
02

Write the Balanced Molecular Equations

The reactions are as follows: 1. Magnesium carbonate with HCl: \[ \text{MgCO}_3 (s) + 2\text{HCl} (aq) \rightarrow \text{MgCl}_2 (aq) + \text{CO}_2 (g) + \text{H}_2\text{O} (l) \]2. Magnesium oxide with HCl: \[ \text{MgO} (s) + 2\text{HCl} (aq) \rightarrow \text{MgCl}_2 (aq) + \text{H}_2\text{O} (l) \]3. Magnesium hydroxide with HCl: \[ \text{Mg(OH)}_2 (s) + 2\text{HCl} (aq) \rightarrow \text{MgCl}_2 (aq) + 2\text{H}_2\text{O} (l) \]
03

Write the Net Ionic Equations

1. For magnesium carbonate: \[ \text{CO}_3^{2-} (s) + 2\text{H}^+ (aq) \rightarrow \text{CO}_2 (g) + \text{H}_2\text{O} (l) \]2. For magnesium oxide: \[ \text{O}^{2-} (s) + 2\text{H}^+ (aq) \rightarrow \text{H}_2\text{O} (l) \]3. For magnesium hydroxide: \[ \text{Mg(OH)}_2(s) \rightarrow \text{Mg}^{2+}(aq) + 2\text{OH}^{-} \] then \[ 2\text{OH}^- (s) + 2\text{H}^+ (aq) \rightarrow 2\text{H}_2\text{O} (l) \]
04

Determine Observable Differences

Magnesium carbonate's reaction produces carbon dioxide gas, which will cause bubbling or fizzing. Magnesium oxide and magnesium hydroxide do not produce gases when reacting with \(\text{HCl}\). This fizzing can help distinguish magnesium carbonate from the other two.

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Key Concepts

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

Magnesium Compounds
Magnesium compounds, such as magnesium carbonate (\(\text{MgCO}_3\)), magnesium oxide (\(\text{MgO}\)), and magnesium hydroxide (\(\text{Mg(OH)}_2\)), are commonly used in various chemical and industrial applications. Each of these compounds reacts uniquely with acidic solutions, such as hydrochloric acid (\(\text{HCl}\)).
The reactions showcase some typical behaviors of magnesium compounds when they interact with acids.
  • **Magnesium Carbonate (\(\text{MgCO}_3\))**: This compound releases carbon dioxide gas when reacting with an acid, resulting in visible effervescence or fizzing.
  • **Magnesium Oxide (\(\text{MgO}\))**: This reacts with acids to form magnesium chloride and water, with no gas production.
  • **Magnesium Hydroxide (\(\text{Mg(OH)}_2\))**: It dissolves in acid, forming water and contributing magnesium ions to the solution.
Understanding these compounds' reactions is essential in the study of acid-base chemistry.
Balanced Chemical Equations
In chemistry, balanced chemical equations are crucial for representing what happens during a chemical reaction. They show the reactants transforming into products, maintaining the law of conservation of mass. When dealing with reactions involving magnesium compounds and hydrochloric acid, it is important to ensure that both sides of the equation have equal numbers of each type of atom.
Let's see how this works for magnesium compounds:
  • **Magnesium Carbonate**: \( \text{MgCO}_3 (s) + 2\text{HCl} (aq) \rightarrow \text{MgCl}_2 (aq) + \text{CO}_2 (g) + \text{H}_2\text{O} (l) \)
  • **Magnesium Oxide**: \( \text{MgO} (s) + 2\text{HCl} (aq) \rightarrow \text{MgCl}_2 (aq) + \text{H}_2\text{O} (l) \)
  • **Magnesium Hydroxide**: \( \text{Mg(OH)}_2 (s) + 2\text{HCl} (aq) \rightarrow \text{MgCl}_2 (aq) + 2\text{H}_2\text{O} (l) \)
Balancing these equations ensures that the same amount of mass is present before and after the reaction, which is a fundamental principle in chemical reactions.
Net Ionic Equations
Net ionic equations focus on the ions that participate directly in the chemical reaction, excluding the spectator ions, which do not change during the process. These equations help in understanding the actual reacting species and the changes occurring at the molecular level.
Here are the net ionic equations for the reactions with magnesium compounds and hydrochloric acid:
  • **Magnesium Carbonate**: \( \text{CO}_3^{2-} (s) + 2\text{H}^+ (aq) \rightarrow \text{CO}_2 (g) + \text{H}_2\text{O} (l) \)
  • **Magnesium Oxide**: \( \text{O}^{2-} (s) + 2\text{H}^+ (aq) \rightarrow \text{H}_2\text{O} (l) \)
  • **Magnesium Hydroxide**: The initial dissociation is \( \text{Mg(OH)}_2(s) \rightarrow \text{Mg}^{2+}(aq) + 2\text{OH}^- \), then \( 2\text{OH}^- (s) + 2\text{H}^+ (aq) \rightarrow 2\text{H}_2\text{O} (l) \)
Studying net ionic equations sharpens the understanding of which ions are truly involved in the reaction.
Reaction Observations
Observing reactions can provide valuable insights into the chemical processes occurring, especially when distinguishing similar substances. Magnesium carbonate, magnesium oxide, and magnesium hydroxide show different observable behaviors when reacting with a strong acid like hydrochloric acid (\(\text{HCl}\)).
Here's a summary of what you might see:
  • **Magnesium Carbonate**: The reaction produces carbon dioxide gas, resulting in visible bubbles and fizzing.
  • **Magnesium Oxide**: There is no gas produced, so this reaction appears calm, producing only a color change as the solution forms.
  • **Magnesium Hydroxide**: Similar to \(\text{MgO}\), there is no bubbling; instead, the \(\text{Mg(OH)}_2\) dissolves to form a clear solution.
The differences in these observable reactions can help identify which magnesium compound you are dealing with based on visible signs like gas production or dissolution.

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Most popular questions from this chapter

Neurotransmitters are molecules that are released by nerve cells to other cells in our bodies, and are needed for muscle motion, thinking, feeling, and memory. Dopamine is a common neurotransmitter in the human brain.(a) Predict what kind of reaction dopamine is most likely to undergo in water: redox, acid-base, precipitation, or metathesis? Explain your reasoning. (b) Patients with Parkinson's disease suffer from a shortage of dopamine and may need to take it to reduce symptoms. An IV (intravenous fluid) bag is filled with a solution that contains \(400.0 \mathrm{mg}\) dopamine per \(250.0 \mathrm{~mL}\) of solution. What is the concentration of dopamine in the IV bag in units of molarity? (c) Experiments with rats show that if rats are dosed with \(3.0 \mathrm{mg} / \mathrm{kg}\) of cocaine (that is, \(3.0 \mathrm{mg}\) cocaine per \(\mathrm{kg}\) of animal mass \(),\) the concentration of dopamine in their brains increases by \(0.75 \mu M\) after 60 seconds. Calculate how many molecules of dopamine would be produced in a rat (average brain volume \(5.00 \mathrm{~mm}^{3}\) ) after 60 seconds of a \(3.0 \mathrm{mg} / \mathrm{kg}\) dose of cocaine.

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 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 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.) \((\mathbf{c})\) Is this manufacturer in compliance with regulations?

(a) By titration, \(15.0 \mathrm{~mL}\) of \(0.1008 \mathrm{M}\) sodium hydroxide is needed to neutralize a \(0.2053-\mathrm{g}\) 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 \(5.89 \% \mathrm{H}, 70.6 \% \mathrm{C},\) and \(23.5 \% \mathrm{O}\) by mass. What is its molecular formula?

In each of the following pairs, indicate which has the higher concentration of \(\mathrm{Cl}^{-}\) ion: \((\mathbf{a}) 0.10 \mathrm{MAlCl}_{3}\) solution or a \(0.25 \mathrm{MLiCl}\) solution, (b) \(150 \mathrm{~mL}\) of a \(0.05 \mathrm{M} \mathrm{MnCl}_{3}\) solution or \(200 \mathrm{~mL}\) of \(0.10 \mathrm{M} \mathrm{KCl}\) solution, (c) a \(2.8 M \mathrm{HCl}\) solution or a solution made by dissolving \(23.5 \mathrm{~g}\) of KCl in water to make \(100 \mathrm{~mL}\) of solution.

True or false: (a) If a substance is oxidized, there must be more oxygen in the substance. (b) If a substance is oxidized, it must lose at least one electron and form an anion.
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