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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Question
![**Question: Osmolarity Comparison**
**Topic: Chemistry - Solutions and Concentration**
Which solution has a higher osmolarity, 0.40 M LiCl or a 0.30 M solution of Na₂SO₄?
---
**Explanation:**
Osmolarity is a measure of the total concentration of solute particles in a solution. It is calculated by multiplying the molarity of the solution by the number of particles (ions) each solute dissociates into when dissolved in water.
1. **Lithium Chloride (LiCl):**
- The dissociation of LiCl in water is:
\[
\text{LiCl (s)} \rightarrow \text{Li}^+ (\text{aq}) + \text{Cl}^- (\text{aq})
\]
- Each formula unit of LiCl dissociates into 2 ions (1 Li⁺ and 1 Cl⁻).
\[
\text{Osmolarity of LiCl} = 0.40 \text{ M} \times 2 = 0.80 \text{ Osm}
\]
2. **Sodium Sulfate (Na₂SO₄):**
- The dissociation of Na₂SO₄ in water is:
\[
\text{Na}_2\text{SO}_4 (\text{s}) \rightarrow 2\text{Na}^+ (\text{aq}) + \text{SO}_4^{2-} (\text{aq})
\]
- Each formula unit of Na₂SO₄ dissociates into 3 ions (2 Na⁺ and 1 SO₄²⁻).
\[
\text{Osmolarity of Na}_2\text{SO}_4 = 0.30 \text{ M} \times 3 = 0.90 \text{ Osm}
\]
**Conclusion:**
The 0.30 M solution of Na₂SO₄ has a higher osmolarity (0.90 Osm) compared to the 0.40 M solution of LiCl (0.80 Osm).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd840dc46-e3d2-47d1-9b6d-e93b2d8faa77%2F6ea54945-f4f3-42a8-b53b-bd8630187827%2Fkj5b76.jpeg&w=3840&q=75)
Transcribed Image Text:**Question: Osmolarity Comparison**
**Topic: Chemistry - Solutions and Concentration**
Which solution has a higher osmolarity, 0.40 M LiCl or a 0.30 M solution of Na₂SO₄?
---
**Explanation:**
Osmolarity is a measure of the total concentration of solute particles in a solution. It is calculated by multiplying the molarity of the solution by the number of particles (ions) each solute dissociates into when dissolved in water.
1. **Lithium Chloride (LiCl):**
- The dissociation of LiCl in water is:
\[
\text{LiCl (s)} \rightarrow \text{Li}^+ (\text{aq}) + \text{Cl}^- (\text{aq})
\]
- Each formula unit of LiCl dissociates into 2 ions (1 Li⁺ and 1 Cl⁻).
\[
\text{Osmolarity of LiCl} = 0.40 \text{ M} \times 2 = 0.80 \text{ Osm}
\]
2. **Sodium Sulfate (Na₂SO₄):**
- The dissociation of Na₂SO₄ in water is:
\[
\text{Na}_2\text{SO}_4 (\text{s}) \rightarrow 2\text{Na}^+ (\text{aq}) + \text{SO}_4^{2-} (\text{aq})
\]
- Each formula unit of Na₂SO₄ dissociates into 3 ions (2 Na⁺ and 1 SO₄²⁻).
\[
\text{Osmolarity of Na}_2\text{SO}_4 = 0.30 \text{ M} \times 3 = 0.90 \text{ Osm}
\]
**Conclusion:**
The 0.30 M solution of Na₂SO₄ has a higher osmolarity (0.90 Osm) compared to the 0.40 M solution of LiCl (0.80 Osm).
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