Domanda del libro di testo
Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine each quantity. e. the pH after adding 5.0 mL of base beyond the equivalence point
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Ch.18 - Aqueous Ionic Equilibrium
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
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Capitolo 18, Problema 73c
Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine each quantity. c. the pH at 10.0 mL of added base
Guida verificata passo dopo passo1
Calculate the initial moles of HBr in the solution using the formula: \( \text{moles} = \text{volume (L)} \times \text{molarity} \).
Calculate the moles of KOH added using the formula: \( \text{moles} = \text{volume (L)} \times \text{molarity} \).
Determine the moles of HBr remaining after the reaction with KOH by subtracting the moles of KOH from the initial moles of HBr.
Calculate the concentration of HBr remaining in the solution by dividing the moles of HBr remaining by the total volume of the solution in liters (initial volume of HBr + volume of KOH added).
Use the concentration of HBr to find the pH of the solution. Since HBr is a strong acid, \( \text{pH} = -\log[\text{H}^+] \), where \([\text{H}^+]\) is the concentration of HBr.
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Titration
Titration is a quantitative analytical technique used to determine the concentration of a solute in a solution. It involves the gradual addition of a titrant (in this case, KOH) to a solution of the analyte (HBr) until the reaction reaches its equivalence point, where stoichiometrically equivalent amounts of acid and base have reacted. Understanding the titration process is essential for calculating pH changes during the addition of the titrant.
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Percorso guidato
03:04
Acid-Base Titration
pH Scale
The pH scale measures the acidity or basicity of a solution, ranging from 0 to 14. A pH of 7 is considered neutral, while values below 7 indicate acidity and values above 7 indicate basicity. The pH is calculated using the concentration of hydrogen ions (H+) in the solution, and it is crucial to understand how the addition of an acid or base affects the pH during titration.
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02:33The pH Scale
Neutralization Reaction
A neutralization reaction occurs when an acid reacts with a base to produce water and a salt, effectively neutralizing each other's properties. In this case, HBr (a strong acid) reacts with KOH (a strong base) to form water and KBr. The stoichiometry of the reaction is important for determining the pH at various points during the titration, particularly before, at, and after the equivalence point.
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Percorso guidato
05:56Lewis Dot Structures: Neutral Compounds
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Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine each quantity. a. the initial pH
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Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine each quantity. d. the pH at the equivalence point
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