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w officeapps.live.com/op/View.aspR? Download file and easy viewing right in Microsoft Edge. Choose Download file if you want to use it later. Lab 8 Answered v A Accessibility Mode I Download 4. Antacid tablets are used to neutralize stomach acid and relieve indigestion or acid reflux. Many commercial antacids contain magnesium hydroxide, Mg(OH)2, as the active ingredient. If one tablet of antacid contains 15 mg of Mg(OH)2, then calculate the number of tablets required to completely neutralize 5 mL of stomach acid if the stomach acid is 0.2 M HC1.

w officeapps.live.com/op/View.aspR? Download file and easy viewing right in Microsoft Edge. Choose Download file if you want to use it later. Lab 8 Answered v A Accessibility Mode I Download 4. Antacid tablets are used to neutralize stomach acid and relieve indigestion or acid reflux. Many commercial antacids contain magnesium hydroxide, Mg(OH)2, as the active ingredient. If one tablet of antacid contains 15 mg of Mg(OH)2, then calculate the number of tablets required to completely neutralize 5 mL of stomach acid if the stomach acid is 0.2 M HC1.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Lab 8 Answered** 4. Antacid tablets are used to neutralize stomach acid and relieve indigestion or acid reflux. Many commercial antacids contain magnesium hydroxide, Mg(OH)₂, as the active ingredient. If one tablet of antacid contains 15 mg of Mg(OH)₂, then calculate the number of tablets required to completely neutralize 5 mL of stomach acid if the stomach acid is 0.2 M HCl. --- **Explanation of Concepts:** This exercise involves calculating the reaction needed to neutralize stomach acid using a specific active ingredient, magnesium hydroxide (Mg(OH)₂), that reacts with hydrochloric acid (HCl). The solution involves understanding molarity, stoichiometry, and the balanced chemical equation: \[ \text{Mg(OH)}_2 (s) + 2 \text{HCl} (aq) \rightarrow \text{MgCl}_2 (aq) + 2 \text{H}_2\text{O} (l) \] **Calculation Steps:** 1. **Determine the Moles of HCl in 5 mL Solution:** - Molarity (M) is moles of solute per liter of solution. Given the molarity is 0.2 M: \[ \text{Moles of HCl} = 0.2 \, \text{M} \times 0.005 \, \text{L} = 0.001 \, \text{moles} \] 2. **Use Stoichiometry to Find Moles of Mg(OH)₂ Needed:** - From the balanced equation, 1 mole of Mg(OH)₂ neutralizes 2 moles of HCl. Thus, to neutralize 0.001 moles of HCl: \[ \text{Moles of Mg(OH)}_2 = \frac{0.001 \, \text{moles HCl}}{2} = 0.0005 \, \text{moles} \] 3. **Calculate Required Mass and Tablets:** - Molar mass of Mg(OH)₂ = 58.32 g/mol, so: \[ \text{Mass of Mg(OH)}_2 = 0.0005 \, \text{moles} \times 58.32 \
Transcribed Image Text:**Lab 8 Answered** 4. Antacid tablets are used to neutralize stomach acid and relieve indigestion or acid reflux. Many commercial antacids contain magnesium hydroxide, Mg(OH)₂, as the active ingredient. If one tablet of antacid contains 15 mg of Mg(OH)₂, then calculate the number of tablets required to completely neutralize 5 mL of stomach acid if the stomach acid is 0.2 M HCl. --- **Explanation of Concepts:** This exercise involves calculating the reaction needed to neutralize stomach acid using a specific active ingredient, magnesium hydroxide (Mg(OH)₂), that reacts with hydrochloric acid (HCl). The solution involves understanding molarity, stoichiometry, and the balanced chemical equation: \[ \text{Mg(OH)}_2 (s) + 2 \text{HCl} (aq) \rightarrow \text{MgCl}_2 (aq) + 2 \text{H}_2\text{O} (l) \] **Calculation Steps:** 1. **Determine the Moles of HCl in 5 mL Solution:** - Molarity (M) is moles of solute per liter of solution. Given the molarity is 0.2 M: \[ \text{Moles of HCl} = 0.2 \, \text{M} \times 0.005 \, \text{L} = 0.001 \, \text{moles} \] 2. **Use Stoichiometry to Find Moles of Mg(OH)₂ Needed:** - From the balanced equation, 1 mole of Mg(OH)₂ neutralizes 2 moles of HCl. Thus, to neutralize 0.001 moles of HCl: \[ \text{Moles of Mg(OH)}_2 = \frac{0.001 \, \text{moles HCl}}{2} = 0.0005 \, \text{moles} \] 3. **Calculate Required Mass and Tablets:** - Molar mass of Mg(OH)₂ = 58.32 g/mol, so: \[ \text{Mass of Mg(OH)}_2 = 0.0005 \, \text{moles} \times 58.32 \
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