Textbook Question
What is the mass/volume percent concentration of the following solutions?
a. 0.078 mol KCl in 75 mL of solution
b. 0.044 mol sucrose (C12H22O11) in 380 mL of solution
Ch.9 Solutions
McMurry8th EditionFundamentals of General, Organic, and Biological ChemistryISBN: 9780134015187
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Table of contents
- Ch.1 Matter and Measurements27
- Ch.2 Atoms and the Periodic Table20
- Ch.3 Ionic Compounds8
- Ch.4 Molecular Compounds23
- Ch.5 Classification & Balancing of Chemical Reactions12
- Ch.6 Chemical Reactions: Mole and Mass Relationships28
- Ch.7 Chemical Reactions: Energy, Rate and Equilibrium64
- Ch.8 Gases, Liquids and Solids24
- Ch.9 Solutions52
- Ch.10 Acids and Bases25
- Ch.11 Nuclear Chemistry22
- Ch.12 Introduction to Organic Chemistry: Alkanes57
- Ch.13 Alkenes, Alkynes, and Aromatic Compounds47
- Ch.14 Some Compounds with Oxygen, Sulfur, or a Halogen50
- Ch.15 Aldehydes and Ketones45
- Ch.16 Amines42
- Ch.17 Carboxylic Acids and Their Derivatives57
- Ch.18 Amino Acids and Proteins82
- Ch.19 Enzymes and Vitamins63
- Ch.20 Carbohydrates44
- Ch.21 The Generation of Biochemical Energy65
- Ch.22 Carbohydrate Metabolism45
- Ch.23 Lipids42
- Ch.24 Lipid Metabolism33
- Ch.25 Protein and Amino Acid Metabolism24
- Ch.26 Nucleic Acids and Protein Synthesis45
McMurry8th EditionFundamentals of General, Organic, and Biological ChemistryISBN: 9780134015187Not the one you use?Change textbook
Chapter 9, Problem 39b
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?
Verified step by step guidance1
Step 1: Understand the relationship between gas solubility and pressure using Henry's Law. Henry's Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. The formula is: , where is the solubility, is the Henry's Law constant, and is the partial pressure of the gas.
Step 2: Calculate the Henry's Law constant, , using the given solubility and pressure in part (a). Rearrange the formula to solve for : . Substitute = 0.15 g/100 mL and = 760 mmHg (convert to atm: 760 mmHg = 1 atm).
Step 3: Use the calculated Henry's Law constant, , to determine the solubility of CO₂ at the new partial pressure of 0.00038 atm. Apply the formula , substituting the new pressure value.
Step 4: Compare the solubility of CO₂ at the new pressure (calculated in Step 3) to the original solubility (0.15 g/100 mL). Calculate the percentage of CO₂ remaining in solution using the formula: .
Step 5: Interpret the result. The percentage calculated in Step 4 represents the fraction of CO₂ that remains dissolved in the solution after equilibrium is reached with the ambient atmosphere.
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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 changes in pressure affect the solubility of gases like CO₂ in water, which is essential for calculating the equilibrium concentration in the soft drink.
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Henry's Law Calculations Concept 1
Equilibrium
Equilibrium in a chemical context refers to the state where the rate of the forward reaction equals the rate of the reverse reaction, resulting in constant concentrations of reactants and products. In this scenario, it describes the balance between CO₂ dissolved in the soft drink and the CO₂ in the atmosphere, influencing how much gas remains in solution after exposure to ambient conditions.
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Parts Per Million (ppm)
Parts per million (ppm) is a unit of measurement used to describe the concentration of one substance in a million parts of another. In this question, the atmospheric concentration of CO₂ is given in ppm, which helps to determine its partial pressure and how it relates to the solubility of CO₂ in the soft drink, impacting the final equilibrium concentration.
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Related Practice
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?
Textbook Question
How is volume/volume percent concentration defined and for what types of solutions is it typically used?
1
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Textbook Question
A dilute aqueous solution of boric acid, H3BO3 is often used as an eyewash. How would you prepare 500.0 mL of a 0.50% (m/v) boric acid solution?
Textbook Question
Why does water not dissolve motor oil?
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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?