How many mL of 0.150 M Ca(OH)2(aq) will be required to completely react with 150. mL of 0. 100 M HCl(aq) solution. Express your answer in decimal notation.
How many mL of 0.150 M Ca(OH)2(aq) will be required to completely react with 150. mL of 0. 100 M HCl(aq) solution. Express your answer in decimal notation.
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: Reaction of Calcium Hydroxide and Hydrochloric Acid
**Problem Statement:**
How many mL of 0.150 M Ca(OH)₂(aq) will be required to completely react with 150. mL of 0.100 M HCl(aq) solution.
**Instructions:**
Express your answer in decimal notation.
**Concept Review:**
This problem involves a neutralization reaction between calcium hydroxide \[Ca(OH)₂\] and hydrochloric acid \[HCl\]. The balanced chemical equation for this reaction is:
\[ Ca(OH)_2(aq) + 2 HCl(aq) \rightarrow CaCl_2(aq) + 2 H_2O(l) \]
To solve this, we need to use the concept of molarity and stoichiometry.
**Solution Steps:**
1. **Calculate moles of HCl:**
\[ \text{Moles of HCl} = \text{Volume} \times \text{Molarity} \]
\[ \text{Moles of HCl} = 150.0 \text{ mL} \times \frac{1 \text{ L}}{1000 \text{ mL}} \times 0.100 \text{ M} \]
\[ \text{Moles of HCl} = 0.0150 \text{ moles} \]
2. **Determine moles of Ca(OH)₂ needed:**
According to the balanced equation, 1 mole of \(Ca(OH)₂\) reacts with 2 moles of \(HCl\).
\[ \text{Moles of Ca(OH)₂} = \frac{0.0150 \text{ moles HCl}}{2} \]
\[ \text{Moles of Ca(OH)₂} = 0.00750 \text{ moles} \]
3. **Calculate volume of 0.150 M Ca(OH)₂ solution required:**
\[ \text{Volume} = \frac{\text{Moles of Ca(OH)₂}}{\text{Molarity of Ca(OH)₂}} \]
\[ \text{Volume} = \frac{0.00750 \text{ moles}}{0.150 \text{ M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9413ee1b-018f-4e4f-9457-fb88f0adac84%2Fc807ff1f-027d-440a-a37d-fc5f65e274e0%2F2ysr6o_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemistry Problem: Reaction of Calcium Hydroxide and Hydrochloric Acid
**Problem Statement:**
How many mL of 0.150 M Ca(OH)₂(aq) will be required to completely react with 150. mL of 0.100 M HCl(aq) solution.
**Instructions:**
Express your answer in decimal notation.
**Concept Review:**
This problem involves a neutralization reaction between calcium hydroxide \[Ca(OH)₂\] and hydrochloric acid \[HCl\]. The balanced chemical equation for this reaction is:
\[ Ca(OH)_2(aq) + 2 HCl(aq) \rightarrow CaCl_2(aq) + 2 H_2O(l) \]
To solve this, we need to use the concept of molarity and stoichiometry.
**Solution Steps:**
1. **Calculate moles of HCl:**
\[ \text{Moles of HCl} = \text{Volume} \times \text{Molarity} \]
\[ \text{Moles of HCl} = 150.0 \text{ mL} \times \frac{1 \text{ L}}{1000 \text{ mL}} \times 0.100 \text{ M} \]
\[ \text{Moles of HCl} = 0.0150 \text{ moles} \]
2. **Determine moles of Ca(OH)₂ needed:**
According to the balanced equation, 1 mole of \(Ca(OH)₂\) reacts with 2 moles of \(HCl\).
\[ \text{Moles of Ca(OH)₂} = \frac{0.0150 \text{ moles HCl}}{2} \]
\[ \text{Moles of Ca(OH)₂} = 0.00750 \text{ moles} \]
3. **Calculate volume of 0.150 M Ca(OH)₂ solution required:**
\[ \text{Volume} = \frac{\text{Moles of Ca(OH)₂}}{\text{Molarity of Ca(OH)₂}} \]
\[ \text{Volume} = \frac{0.00750 \text{ moles}}{0.150 \text{ M
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