Textbook Question
Calculate [OH-] and pH for each of the following strong base solutions: (c) 10.0 mL of 0.0105 M Ca(OH)2 diluted to 500.0 mL
Ch.16 - Acid-Base Equilibria
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 16, Problem 47b
Calculate the pH of each of the following strong acid solutions: (b) 1.52 g of HNO3 in 575 mL of solution
Verified step by step guidance1
Calculate the number of moles of HNO_3 using its molar mass. The molar mass of HNO_3 is approximately 63.01 g/mol.
Convert the mass of HNO_3 (1.52 g) to moles by dividing by the molar mass.
Determine the concentration of HNO_3 in the solution by dividing the number of moles by the volume of the solution in liters (575 mL = 0.575 L).
Since HNO_3 is a strong acid, it dissociates completely in water. Therefore, the concentration of HNO_3 is equal to the concentration of H^+ ions.
Calculate the pH of the solution using the formula pH = -\log[H^+].
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Strong Acids
Strong acids, such as nitric acid (HNO3), completely dissociate in water, meaning that all the acid molecules break apart into their constituent ions. This complete ionization is crucial for calculating the concentration of hydrogen ions (H+) in solution, which directly affects the pH.
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Strong Acid-Strong Base Titration
pH Scale
The pH scale is a logarithmic scale used to measure the acidity or basicity of a solution, ranging from 0 to 14. A pH of 7 is neutral, while values below 7 indicate acidic solutions and values above 7 indicate basic solutions. The pH is calculated using the formula pH = -log[H+], where [H+] is the concentration of hydrogen ions in moles per liter.
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Concentration Calculation
To calculate the concentration of H+ ions in a solution, one must first determine the number of moles of the solute (in this case, HNO3) and then divide by the volume of the solution in liters. The formula used is: concentration (M) = moles of solute / volume of solution (L). This concentration is essential for determining the pH of the solution.
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Related Practice
Textbook Question
Addition of phenolphthalein to an unknown colorless solution does not cause a color change. The addition of bromthymol blue to the same solution leads to a yellow color. (c) What other indicator or indicators would you want to use to determine the pH of the solution more precisely?
Textbook Question
Calculate the pH of each of the following strong acid solutions: (b) 0.225 g of HClO3 in 2.00 L of solution