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

8. Gases, Liquids and Solids

The Ideal Gas Law

GOB Chemistry

8. Gases, Liquids and Solids

The Ideal Gas Law

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1:42 minutes

Problem 98a

Textbook Question

A solution is prepared by bubbling 15.0 L of HCl(g) at 25 °C and 1 atm into 250.0 mL of water.
a. Assuming all the HCl dissolves in the water, how many moles of HCl are in solution?

Verified step by step guidance

Step 1: Use the ideal gas law to calculate the number of moles of HCl gas. The ideal gas law is given by:

P V = n R T

, where P is pressure (1 atm), V is volume (15.0 L), R is the gas constant (0.0821 L·atm/(mol·K)), and T is temperature in Kelvin (convert 25 °C to Kelvin by adding 273.15).

Step 2: Rearrange the ideal gas law to solve for n (number of moles):

n = \frac{P V}{R T}

. Substitute the values for P, V, R, and T into the equation.

Step 3: Perform the calculation to determine the number of moles of HCl gas. This will give you the total moles of HCl that dissolve in the water, as the problem states that all the HCl dissolves.

Step 4: Note that the volume of water (250.0 mL) does not directly affect the calculation of moles of HCl, as the problem focuses on the gas dissolving into the solution. However, this volume may be relevant for subsequent calculations, such as determining molarity.

Step 5: Conclude that the number of moles of HCl calculated in Step 3 represents the total moles of HCl in the solution.

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Key Concepts

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

Ideal Gas Law

The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. In this context, it allows us to calculate the number of moles of HCl gas by using the given volume (15.0 L), pressure (1 atm), and temperature (25 °C).

Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. While the question focuses on the moles of HCl, understanding molarity is essential for determining how concentrated the resulting solution will be after the gas dissolves in water.

Dissolution Process

The dissolution process refers to how a solute (in this case, HCl gas) interacts with a solvent (water) to form a solution. It is important to recognize that when HCl gas dissolves in water, it ionizes to form H⁺ and Cl⁻ ions, which is crucial for understanding the properties of the resulting solution.

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