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Chapter 4: Problem 100

Some of the substances commonly used in stomach antacids are \(\mathrm{MgO}, \mathrm{Mg}(\mathrm{OH})_{2}\), and \(\mathrm{Al}(\mathrm{OH})_{3} .\) a. Write a balanced equation for the neutralization of hydrochloric acid by each of these substances. b. Which of these substances will neutralize the greatest amount of \(0.10 M \mathrm{HCl}\) per gram?

Short Answer

Expert verified
The balanced equations for the neutralization of HCl by MgO, Mg(OH)₂, and Al(OH)₃ are: 1. \( \mathrm{MgO} + 2 \mathrm{HCl} \rightarrow \mathrm{MgCl}_2 + \mathrm{H_2O} \) 2. \( \mathrm{Mg(OH)}_2 + 2 \mathrm{HCl} \rightarrow \mathrm{MgCl}_2 + 2 \mathrm{H_2O} \) 3. \( \mathrm{Al(OH)}_3 + 3 \mathrm{HCl} \rightarrow \mathrm{AlCl}_3 + 3 \mathrm{H_2O} \) To neutralize 0.10 moles of HCl, the required masses of these substances are: 1. MgO: 2.0155 g 2. Mg(OH)₂: 2.9165 g 3. Al(OH)₃: 2.6 g Hence, magnesium oxide (MgO) requires the least amount of mass to neutralize the same amount of HCl, making it the most effective substance per gram from the provided options in stomach antacids.

Step by step solution

01

Magnesium Oxide with Hydrochloric Acid

The reaction between magnesium oxide (MgO) and hydrochloric acid (HCl) can be written as follows: \[ \mathrm{MgO} + 2 \mathrm{HCl} \rightarrow \mathrm{MgCl}_2 + \mathrm{H_2O} \] The balanced equation shows that 1 mole of MgO reacts with 2 moles of HCl to produce 1 mole of magnesium chloride (MgCl₂) and 1 mole of water (H₂O).
02

Magnesium Hydroxide with Hydrochloric Acid

The reaction of magnesium hydroxide (Mg(OH)₂) with hydrochloric acid (HCl) can be represented as: \[ \mathrm{Mg(OH)}_2 + 2 \mathrm{HCl} \rightarrow \mathrm{MgCl}_2 + 2 \mathrm{H_2O} \] The balanced equation indicates that 1 mole of Mg(OH)₂ reacts with 2 moles of HCl to produce 1 mole of MgCl₂ and 2 moles of H₂O.
03

Aluminum Hydroxide with Hydrochloric Acid

Lastly, the reaction between aluminum hydroxide (Al(OH)₃) and hydrochloric acid (HCl) can be notated as: \[ \mathrm{Al(OH)}_3 + 3 \mathrm{HCl} \rightarrow \mathrm{AlCl}_3 + 3 \mathrm{H_2O} \] In this balanced reaction, 1 mole of Al(OH)₃ reacts with 3 moles of HCl to produce 1 mole of aluminum chloride (AlCl₃) and 3 moles of H₂O. #b. Determine the substance which neutralizes the most acid per gram#
04

Calculation for magnesium oxide (MgO)

First, we need to identify the molar mass of MgO: MgO: \( (24.31 + 16.00)g/mol = 40.31 g/mol \) Next, we will use stoichiometry to determine the mass of MgO required to neutralize 0.10 moles of HCl: \( 1 \: \text{mol MgO} \)/\( 2 \: \text{mol HCl} \) × \( 40.31 \: \text{g MgO} \)/\( 1 \: \text{mol MgO} \) × 0.10 mol HCl = 2.0155 g MgO
05

Calculation for magnesium hydroxide (Mg(OH)₂)

Find the molar mass of Mg(OH)₂: Mg(OH)₂: \( (24.31 + 2 * (16.00 + 1.008))g/mol = 58.33 g/mol \) Now, calculate the mass of Mg(OH)₂ required to neutralize 0.10 moles of HCl using stoichiometry: \( 1 \: \text{mol Mg(OH)}_2 \)/\( 2 \: \text{mol HCl} \) × \( 58.33 \: \text{g Mg(OH)}_2 \)/\( 1 \: \text{mol Mg(OH)}_2 \) × 0.10 mol HCl = 2.9165 g Mg(OH)₂
06

Calculation for aluminum hydroxide (Al(OH)₃)

Determine the molar mass of Al(OH)₃ Al(OH)₃: \( (26.98 + 3 * (16.00 + 1.008))g/mol = 78.00 g/mol \) Next, determine the mass of Al(OH)₃ needed to neutralize 0.10 moles of HCl using stoichiometry: \( 1 \: \text{mol Al(OH)}_3 \)/\( 3 \: \text{mol HCl} \) × \( 78.00 \: \text{g Al(OH)}_3 \)/\( 1 \: \text{mol Al(OH)}_3 \) × 0.10 mol HCl = 2.6 g Al(OH)₃
07

Comparing the masses of the substances required for neutralization

Comparing the mass needed for each substance to neutralize 0.10 moles of HCl, we have: - MgO: 2.0155 g - Mg(OH)₂: 2.9165 g - Al(OH)₃: 2.6 g So, magnesium oxide (MgO) requires the least amount of mass to neutralize the same amount of hydrochloric acid, making it the most effective substance per gram from the provided options in stomach antacids.

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