Domanda del libro di testo
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
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Ch.16 - Acid-Base Equilibria
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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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 47
Calculate the concentration of an aqueous solution of NaOH that has a pH of 11.50.
Guida verificata passo dopo passo1
Step 1: Understand that pH is a measure of the hydrogen ion concentration in a solution. The pH is related to the pOH by the equation: \( \text{pH} + \text{pOH} = 14 \).
Step 2: Calculate the pOH of the solution using the given pH value: \( \text{pOH} = 14 - \text{pH} \). Substitute the given pH of 11.50 into the equation.
Step 3: Convert the pOH to hydroxide ion concentration \([\text{OH}^-]\) using the formula: \([\text{OH}^-] = 10^{-\text{pOH}}\).
Step 4: Recognize that the concentration of NaOH in the solution is equal to the concentration of \([\text{OH}^-]\) because NaOH dissociates completely in water.
Step 5: Use the calculated \([\text{OH}^-]\) concentration as the concentration of the NaOH solution.
Concetti chiave
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pH Scale
The pH scale measures the acidity or basicity of a solution, ranging from 0 to 14. A pH of 7 is neutral, while values below 7 indicate acidity and above 7 indicate basicity. Each unit change in pH represents a tenfold change in hydrogen ion concentration, making it crucial for understanding the behavior of acids and bases in solution.
Video consigliato:
Percorso guidato
02:33
The pH Scale
Concentration of Hydroxide Ions
In basic solutions, the concentration of hydroxide ions (OH-) is significant. The relationship between pH and hydroxide ion concentration can be derived from the equation pOH = 14 - pH. For a pH of 11.50, the pOH can be calculated, allowing for the determination of the hydroxide ion concentration, which is essential for calculating the concentration of NaOH in the solution.
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Percorso guidato
06:12Hydroxide Ion Concentration Example
Stoichiometry of NaOH Dissociation
Sodium hydroxide (NaOH) is a strong base that completely dissociates in water into sodium ions (Na+) and hydroxide ions (OH-). The stoichiometry of this dissociation means that the concentration of NaOH is equal to the concentration of OH- produced. Understanding this relationship is vital for calculating the concentration of the NaOH solution based on the hydroxide ion concentration derived from the pH.
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Percorso guidato
01:16Stoichiometry Concept
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Calculate the concentration of an aqueous solution of Ca1OH22 that has a pH of 10.05.
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Domanda del libro di testo
Write the chemical equation and the Ka expression for the acid dissociation of each of the following acids in aqueous solution. First show the reaction with H+(a)q as a product and then with the hydronium ion: (a) C6H5COOH (b) HCO3-
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