Domanda del libro di testo
Calculate the pH of each of the following strong acid solutions: (b) 0.225 g of HClO3 in 2.00 L of solution
782
views
Ch.16 - Acid-Base Equilibria
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
Non è quello che usi tu?Cambia libro di testoScegli un libro di testo diverso
TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 16, Problema 43b
Calculate the pH of each of the following strong acid solutions: (b) 1.52 g of HNO3 in 575 mL of solution
Guida verificata passo dopo passo1
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^+].
Risposta video verificata per un problema simile:
Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
3mConcetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
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.
Video consigliato:
Percorso guidato
01:09
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.
Video consigliato:
Percorso guidato
02:33The pH Scale
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.
Video consigliato:
Percorso guidato
07:35Calculate Concentration of the Basic Form