Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

9. Solutions

Henry's Law Calculations

GOB Chemistry

9. Solutions

Henry's Law Calculations

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2:44 minutes

Problem 5

Textbook Question

At a total atmospheric pressure of 1.00 atm, the partial pressure of CO₂ in air is approximately 4.0 × 10^-4atm. Using the data in Problem 9.4, what is the solubility of CO₂ in an open bottle of seltzer water at 20 °C?

Verified step by step guidance

Identify the relationship between gas solubility and partial pressure using Henry's Law: \( C = k_H \cdot P \), where \( C \) is the solubility of the gas (in mol/L), \( k_H \) is the Henry's Law constant (in mol/L·atm), and \( P \) is the partial pressure of the gas (in atm).

From Problem 9.4, determine the Henry's Law constant \( k_H \) for CO₂ at 20 °C. If not provided, consult a reliable source or reference table for the value of \( k_H \) at this temperature.

Substitute the given partial pressure of CO₂, \( P = 4.0 \times 10^{-4} \ \text{atm} \), and the Henry's Law constant \( k_H \) into the equation \( C = k_H \cdot P \).

Perform the multiplication to calculate the solubility \( C \) of CO₂ in the seltzer water. Ensure the units are consistent (e.g., mol/L).

Interpret the result: The calculated solubility represents the concentration of CO₂ dissolved in the seltzer water at equilibrium under the given conditions of temperature and pressure.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Henry's Law

Henry's Law states that the amount of gas that dissolves in a liquid at a given temperature is directly proportional to the partial pressure of that gas above the liquid. This principle is crucial for understanding how gases like CO₂ behave in solutions, particularly in carbonated beverages, where the pressure of CO₂ influences its solubility.

Solubility

Solubility refers to the maximum amount of a substance that can dissolve in a solvent at a specific temperature and pressure. In the context of the question, it pertains to how much CO₂ can be dissolved in seltzer water at 20 °C, which is influenced by both temperature and the partial pressure of CO₂.

Partial Pressure

Partial pressure is the pressure exerted by a single component of a mixture of gases. In this scenario, the partial pressure of CO₂ in the air is given, and it is essential for calculating the solubility of CO₂ in seltzer water using Henry's Law, as it directly affects how much CO₂ can be dissolved in the liquid.

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Related Practice

Textbook Question

The solubility of CO₂ gas in water is 0.15 g/100 mL at a CO₂ pressure of 760 mmHg.

b. An atmospheric concentration of 380 ppm, CO₂ corresponds to a partial pressure of 0.00038 atm. What percentage of the CO₂ originally dissolved in the solution in part (a) remains in solution after the soft drink reaches equilibrium with the ambient atmosphere?

Multiple Choice

Henry's Law Constant for nitrogen in water is 1.67 x 10^–4 M•atm^–1. If a closed canister contains 0.103 M nitrogen, what would be its pressure in atm?

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Multiple Choice

At 0ºC and 1.00 atm, as much as 0.84 g of O₂ can dissolve in 1.0 L of water. At 0ºC and 4.00 atm, how many grams of O₂ dissolve in 1.0 L of water?

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Multiple Choice

The atmospheric pressure in a lab is calculated as 1.3 atm. If oxygen gas contributes 62% of this atmospheric pressure, determine its mass (in g) dissolved at room temperature in 25 L of water. The Henry's Law Constant for oxygen in water at this temperature is 5.3 x 10^-5 M/atm.

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Textbook Question

The solubility of NH₃ gas in water at an NH₃ pressure of 760.0 mmHg and 25°C is 51.8 g/100 mL and 27.0 g/100 mL at 50°C.

a.What is the solubility of NH₃ if its partial pressure is reduced to 225.0 mmHg?

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Textbook Question

The solubility of NH₃ gas in water at an NH₃ pressure of 760.0 mmHg and 25°C is 51.8 g/100 mL and 27.0 g/100 mL at 50°C.

b. How many moles of NH₃ would be released from 1.0 L of a saturated NH₃ solution if the temperature was increased from 25 to 50 °C?

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Textbook Question

The solubility of CO₂ gas in water is 0.15 g/100 mL at a CO₂ pressure of 760 mmHg.

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At a total atmospheric pressure of 1.00 atm, the partial pressure of CO2 in air is approximately 4.0 × 10-4atm. Using the data in Problem 9.4, what is the solubility of CO2 in an open bottle of seltzer water at 20 °C?

Key Concepts

Henry's Law

Solubility

Partial Pressure

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At a total atmospheric pressure of 1.00 atm, the partial pressure of CO₂ in air is approximately 4.0 × 10^-4atm. Using the data in Problem 9.4, what is the solubility of CO₂ in an open bottle of seltzer water at 20 °C?