Textbook Question
How is volume/volume percent concentration defined and for what types of solutions is it typically used?
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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 38a
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?
Verified step by step guidance1
Step 1: Understand the relationship between gas solubility and pressure. According to Henry's Law, 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 proportionality constant, and is the partial pressure.
Step 2: Use the given data to calculate the proportionality constant at 25°C. Rearrange Henry's Law to solve for : . Substitute the solubility of NH₃ (51.8 g/100 mL) and the pressure (760.0 mmHg) into the equation.
Step 3: Once is determined, use it to calculate the solubility of NH₃ at the reduced pressure of 225.0 mmHg. Rearrange Henry's Law to solve for solubility: . Substitute the value of and the new pressure (225.0 mmHg) into the equation.
Step 4: Perform the calculation to find the solubility of NH₃ at 225.0 mmHg. Ensure that the units of solubility remain consistent (e.g., g/100 mL).
Step 5: Verify the result by checking the proportionality between solubility and pressure. The solubility at 225.0 mmHg should be lower than the solubility at 760.0 mmHg, as the pressure has decreased.
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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, such as NH₃, in water.
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Henry's Law Calculations Concept 1
Solubility
Solubility refers to the maximum amount of a substance that can dissolve in a given quantity of solvent at a specific temperature and pressure. In this context, it is important to know how solubility values change with temperature and pressure to calculate the new solubility of NH₃ at a reduced pressure.
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Temperature Effects on Solubility
Temperature can significantly influence the solubility of gases in liquids. Generally, as temperature increases, the solubility of gases decreases. Understanding this relationship helps in predicting how the solubility of NH₃ will change when the temperature is altered, as seen in the provided solubility data.
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Related Practice
Textbook Question
How can you tell a solution from a colloid?
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?
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?
Textbook Question
HF is a weak electrolyte and HBr is a strong electrolyte. Which of the curves in the figure represents the change in the boiling point of an aqueous solution when 1 mole of HF is added to 1 kg of water, and which represents the change when 1 mol of HBr is added?
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