3) If a 35.75 mL sample of 0.175 M HCI (aq) solution is neutralized with 0.125 M Mg(OH)2, how much Mg(OH)2 will be needed? 2 HCI (aq) + Mg(OH), (aq) → MgCl2(aq) + 2 HOH (I)
3) If a 35.75 mL sample of 0.175 M HCI (aq) solution is neutralized with 0.125 M Mg(OH)2, how much Mg(OH)2 will be needed? 2 HCI (aq) + Mg(OH), (aq) → MgCl2(aq) + 2 HOH (I)
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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![### Chemistry Problem: Neutralization Reaction
**Problem Statement:**
If a 35.75 mL sample of 0.175 M HCl (\(aq\)) solution is neutralized with 0.125 M Mg(OH)\(_2\), how much Mg(OH)\(_2\) will be needed?
**Chemical Equation:**
\[ 2 \, \text{HCl} \, (aq) + \text{Mg(OH)}_2 \, (aq) \rightarrow \text{MgCl}_2 \, (aq) + 2 \, \text{HOH} \, (l) \]
**Explanation:**
This problem involves a neutralization reaction, where hydrochloric acid (HCl) reacts with magnesium hydroxide (Mg(OH)\(_2\)) to form magnesium chloride (MgCl\(_2\)) and water (H\(_2\)O), represented as HOH here. The balanced equation shows that two moles of HCl react with one mole of Mg(OH)\(_2\).
To find the amount of Mg(OH)\(_2\) needed:
1. Calculate the moles of HCl present in the sample using the volume and molarity.
2. Use the stoichiometry of the reaction (2:1 ratio) to find the moles of Mg(OH)\(_2\) needed.
3. Convert the moles of Mg(OH)\(_2\) to the required volume using its molarity.
This exercise demonstrates stoichiometry concepts in chemistry, focusing on balancing reactions and using molarity in calculations.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5f6319fd-3db3-4131-945e-33c3df9bac4f%2Fd7ba1164-37dc-49cc-9053-62389e6be058%2Fwr8qy1_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemistry Problem: Neutralization Reaction
**Problem Statement:**
If a 35.75 mL sample of 0.175 M HCl (\(aq\)) solution is neutralized with 0.125 M Mg(OH)\(_2\), how much Mg(OH)\(_2\) will be needed?
**Chemical Equation:**
\[ 2 \, \text{HCl} \, (aq) + \text{Mg(OH)}_2 \, (aq) \rightarrow \text{MgCl}_2 \, (aq) + 2 \, \text{HOH} \, (l) \]
**Explanation:**
This problem involves a neutralization reaction, where hydrochloric acid (HCl) reacts with magnesium hydroxide (Mg(OH)\(_2\)) to form magnesium chloride (MgCl\(_2\)) and water (H\(_2\)O), represented as HOH here. The balanced equation shows that two moles of HCl react with one mole of Mg(OH)\(_2\).
To find the amount of Mg(OH)\(_2\) needed:
1. Calculate the moles of HCl present in the sample using the volume and molarity.
2. Use the stoichiometry of the reaction (2:1 ratio) to find the moles of Mg(OH)\(_2\) needed.
3. Convert the moles of Mg(OH)\(_2\) to the required volume using its molarity.
This exercise demonstrates stoichiometry concepts in chemistry, focusing on balancing reactions and using molarity in calculations.
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