**Text Transcription for Educational Website:**---**Topic: Calculation of Dissolved CO₂ in Water**CO₂ concentration is 440 ppm in the atmosphere. How much CO₂ is dissolved in water (in terms of mg/L) when pH=4, 7, and 10? Assume steady-state, atmospheric pressure at 1 atm and temperature at 298 K.---**Explanation:**This text discusses the dissolution of carbon dioxide (CO₂) in water under specific environmental conditions. Given an atmospheric CO₂ concentration of 440 parts per million (ppm), the task is to calculate how much CO₂ will dissolve in water at three different pH levels: pH 4, pH 7, and pH 10. This calculation assumes a steady-state environment, with constant atmospheric pressure of 1 atmosphere (atm) and a temperature of 298 Kelvin (approximately 25°C).**Points to Consider:**1. **Understanding Gas Solubility:** Solubility of gases like CO₂ in water is influenced by temperature, pressure, and the pH of the solution. Henry's law often helps with calculating the solubility of gases.2. **Henry's Law Constant:** Calculating the dissolved concentration might require using Henry's law, which relates the concentration of a gas in a liquid to its partial pressure above the liquid, through the Henry's law constant.3. **Effect of pH:** The pH affects the forms of dissolved CO₂, which can be present as carbonic acid (H₂CO₃), bicarbonate (HCO₃⁻), or carbonate (CO₃²⁻). The dominant species depend on the pH level of the solution.4. **Assumptions:** - The system is in equilibrium, implying that the CO₂ has fully dissolved to its maximum capacity at the given conditions. - The temperature and pressure conditions remain constant throughout the experiment.---**Note:** This exercise emphasizes the importance of environmental conditions in determining the solubility of gases in water, a concept widely applicable in environmental and chemical engineering studies.

at pH = 4. -log[H+] = 4 [H+] = 10-4 [H+] = 0.0001 M since, CO2 + H2O -----> H+ +…

CO2 concentration is 440 ppm in the atmosphere. How much CO2 is dissolved in water (in terms of mg/L) when pH=4, 7, and 10? Assume steady-state, atmospheric pressure at 1 atm and temperature at 298 K.

CO2 concentration is 440 ppm in the atmosphere. How much CO2 is dissolved in water (in terms of mg/L) when pH=4, 7, and 10? Assume steady-state, atmospheric pressure at 1 atm and temperature at 298 K.

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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**Text Transcription for Educational Website:**

---

**Topic: Calculation of Dissolved CO₂ in Water**

CO₂ concentration is 440 ppm in the atmosphere. How much CO₂ is dissolved in water (in terms of mg/L) when pH=4, 7, and 10? Assume steady-state, atmospheric pressure at 1 atm and temperature at 298 K.

---

**Explanation:**

This text discusses the dissolution of carbon dioxide (CO₂) in water under specific environmental conditions. Given an atmospheric CO₂ concentration of 440 parts per million (ppm), the task is to calculate how much CO₂ will dissolve in water at three different pH levels: pH 4, pH 7, and pH 10. This calculation assumes a steady-state environment, with constant atmospheric pressure of 1 atmosphere (atm) and a temperature of 298 Kelvin (approximately 25°C).

**Points to Consider:**

1. **Understanding Gas Solubility:**
Solubility of gases like CO₂ in water is influenced by temperature, pressure, and the pH of the solution. Henry's law often helps with calculating the solubility of gases.

2. **Henry's Law Constant:**
Calculating the dissolved concentration might require using Henry's law, which relates the concentration of a gas in a liquid to its partial pressure above the liquid, through the Henry's law constant.

3. **Effect of pH:**
The pH affects the forms of dissolved CO₂, which can be present as carbonic acid (H₂CO₃), bicarbonate (HCO₃⁻), or carbonate (CO₃²⁻). The dominant species depend on the pH level of the solution.

4. **Assumptions:**
- The system is in equilibrium, implying that the CO₂ has fully dissolved to its maximum capacity at the given conditions.
- The temperature and pressure conditions remain constant throughout the experiment.

---

**Note:** This exercise emphasizes the importance of environmental conditions in determining the solubility of gases in water, a concept widely applicable in environmental and chemical engineering studies.

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