**Henry's Law and Solubility of CO₂ in Water**The Henry's law constant at 25 °C for carbon dioxide (CO₂) in water is 0.035 M/atm. To find the solubility of CO₂, expressed in molarity units, in 1.0 L of water when the partial pressure of CO₂ is 1.1 atm, you can use Henry's law. **Henry's Law Formula:**\[ C = k_{\text{H}} \times P \]Where:- \( C \) is the solubility of the gas (in molarity, M)- \( k_{\text{H}} \) is Henry's law constant (0.035 M/atm)- \( P \) is the partial pressure of the gas (1.1 atm)**Calculation:**\[ C = 0.035 \, \text{M/atm} \times 1.1 \, \text{atm} = 0.0385 \, \text{M} \]Thus, the solubility of CO₂ in 1.0 L of water, under a partial pressure of 1.1 atm, is 0.0385 M.

Henry’s Law is C = KH× P Where, C = molarity of gas in solution. KH = Henry’s constant = 0.035…

Answered: The Henry's law constant at 25 °C for…

The Henry's law constant at 25 °C for CO2 in water is 0.035 M/ atm. What is the solubility of CO2, in molarity units, in 1.0 L of water when the partial pressure of CO2 is 1.1 atm?

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

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Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

**Henry's Law and Solubility of CO₂ in Water**

The Henry's law constant at 25 °C for carbon dioxide (CO₂) in water is 0.035 M/atm. To find the solubility of CO₂, expressed in molarity units, in 1.0 L of water when the partial pressure of CO₂ is 1.1 atm, you can use Henry's law.

**Henry's Law Formula:**
\[ C = k_{\text{H}} \times P \]
Where:
- \( C \) is the solubility of the gas (in molarity, M)
- \( k_{\text{H}} \) is Henry's law constant (0.035 M/atm)
- \( P \) is the partial pressure of the gas (1.1 atm)

**Calculation:**
\[ C = 0.035 \, \text{M/atm} \times 1.1 \, \text{atm} = 0.0385 \, \text{M} \]

Thus, the solubility of CO₂ in 1.0 L of water, under a partial pressure of 1.1 atm, is 0.0385 M.

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