Textbook Question
How many equivalents of an acid or base are in the following?
a. 0.25 mol Mg(OH)2
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Ch.10 Acids and Bases
McMurry8th EditionFundamentals of GOBISBN: 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
Chapter 10, Problem 98a
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 guidance1
Step 1: Use the ideal gas law to calculate the number of moles of HCl gas. The ideal gas law is given by: , 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): . 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).
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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.
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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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Related Practice
Textbook Question
What are the molarity and the normality of a solution made by dissolving 5.0 g of Ca(OH)2 in enough water to make 500.0 mL of solution?
1357
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Textbook Question
What are the molarity and the normality of a solution made by dissolving 25 g of citric acid (triprotic, C6H5O7H3) in enough water to make 800 mL of solution?
980
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Textbook Question
The dissociation of water into H3O+ and OH– ions depends on temperature. At 0 °C the [H3O+] = 3.38 x 10–8 M, at 25 °C the [H3O+] = 1.00 x 10–7 M, and at 50 °C the [H3O+] = 2.34 x 10–7 M.
b. What is the value of Kw at 0 °C and 50 °C?
1737
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Textbook Question
The dissociation of water into H3O+ and OH– ions depends on temperature. At 0 °C the [H3O+] = 3.38 x 10–8 M, at 25 °C the [H3O+] = 1.00 x 10–7 M, and at 50 °C the [H3O+] = 2.34 x 10–7 M.
c. Is the dissociation of water endothermic or exothermic?
2241
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Textbook Question
One of the buffer systems used to control the pH of blood involves the equilibrium between H2PO4– and H2PO42–. The pKa for H2PO42– is 7.21.
a. Write the Henderson-Hasselbalch equation for this buffer system.
847
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