How many grams of water are produced if 27.4 mL of the 0.164 M calcium hydroxide solution is reacted with excess hydrochloric acid? Ca(OH)2 (aq) + 2 HCI (aq) – CaCl2 (aq) + 2 H20 (I)
How many grams of water are produced if 27.4 mL of the 0.164 M calcium hydroxide solution is reacted with excess hydrochloric acid? Ca(OH)2 (aq) + 2 HCI (aq) – CaCl2 (aq) + 2 H20 (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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![### Calculation of Water Produced from a Reaction between Calcium Hydroxide and Hydrochloric Acid
**Question:**
How many grams of water are produced if 27.4 mL of the 0.164 M calcium hydroxide solution is reacted with excess hydrochloric acid?
**Chemical Equation:**
\[ \text{Ca(OH)}_2 (aq) + 2 \text{HCl} (aq) \rightarrow \text{CaCl}_2 (aq) + 2 \text{H}_2\text{O} (l) \]
#### Step-by-Step Solution:
1. **Determine Moles of Ca(OH)₂:**
\[ \text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}} \]
Given:
- Volume of Ca(OH)₂ = 27.4 mL = 0.0274 L
- Molarity (M) of Ca(OH)₂ = 0.164 M
\[ \text{Moles of Ca(OH)}_2 = 0.164 \text{ M} \times 0.0274 \text{ L} \]
\[ \text{Moles of Ca(OH)}_2 = 0.0044936 \text{ moles} \]
2. **Stoichiometric Ratio:**
From the balanced chemical equation, 1 mole of Ca(OH)₂ produces 2 moles of H₂O.
\[ \text{Moles of H}_2\text{O} = 0.0044936 \text{ moles} \times 2 = 0.0089872 \text{ moles} \]
3. **Convert Moles of H₂O to Grams:**
\[ \text{Molar mass of H}_2\text{O} = 2(1.008) + 16.00 = 18.016 \text{ g/mol} \]
\[ \text{Mass of H}_2\text{O} = 0.0089872 \text{ moles} \times 18.016 \text{ g/mol} \]
\[ \text{Mass of H}_2\text{O} \approx 0.162 \text{ grams} \]
Hence, when 27.4 mL of the 0.164](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F15ddb6cd-6983-4657-9770-05e88534b1be%2Ff5da4041-71f4-4c51-84c8-b24ebea1a7b0%2Fnqu55cs.jpeg&w=3840&q=75)
Transcribed Image Text:### Calculation of Water Produced from a Reaction between Calcium Hydroxide and Hydrochloric Acid
**Question:**
How many grams of water are produced if 27.4 mL of the 0.164 M calcium hydroxide solution is reacted with excess hydrochloric acid?
**Chemical Equation:**
\[ \text{Ca(OH)}_2 (aq) + 2 \text{HCl} (aq) \rightarrow \text{CaCl}_2 (aq) + 2 \text{H}_2\text{O} (l) \]
#### Step-by-Step Solution:
1. **Determine Moles of Ca(OH)₂:**
\[ \text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}} \]
Given:
- Volume of Ca(OH)₂ = 27.4 mL = 0.0274 L
- Molarity (M) of Ca(OH)₂ = 0.164 M
\[ \text{Moles of Ca(OH)}_2 = 0.164 \text{ M} \times 0.0274 \text{ L} \]
\[ \text{Moles of Ca(OH)}_2 = 0.0044936 \text{ moles} \]
2. **Stoichiometric Ratio:**
From the balanced chemical equation, 1 mole of Ca(OH)₂ produces 2 moles of H₂O.
\[ \text{Moles of H}_2\text{O} = 0.0044936 \text{ moles} \times 2 = 0.0089872 \text{ moles} \]
3. **Convert Moles of H₂O to Grams:**
\[ \text{Molar mass of H}_2\text{O} = 2(1.008) + 16.00 = 18.016 \text{ g/mol} \]
\[ \text{Mass of H}_2\text{O} = 0.0089872 \text{ moles} \times 18.016 \text{ g/mol} \]
\[ \text{Mass of H}_2\text{O} \approx 0.162 \text{ grams} \]
Hence, when 27.4 mL of the 0.164
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