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. c. the pH at 10.0 mL of added base
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Ch.18 - Aqueous Ionic Equilibrium
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving117
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds128
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions84
- Ch.6 - Gases112
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements86
- Ch.10 - Chemical Bonding I: The Lewis Model91
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials48
- Ch.14 - Solutions93
- Ch.15 - Chemical Kinetics114
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases137
- Ch.18 - Aqueous Ionic Equilibrium154
- Ch.19 - Free Energy & Thermodynamics91
- Ch.20 - Electrochemistry105
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry141
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Capitolo 18, Problema 67d
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
Guida verificata passo dopo passo1
Identify the type of titration: This is a strong acid (HBr) with a strong base (KOH) titration.
Determine the moles of HBr initially present using the formula: \( \text{moles} = \text{concentration} \times \text{volume} \).
Calculate the volume of KOH needed to reach the equivalence point using the stoichiometry of the reaction: \( \text{HBr} + \text{KOH} \rightarrow \text{KBr} + \text{H}_2\text{O} \).
At the equivalence point, all the HBr has reacted with KOH to form KBr and water. Since both are strong, the solution is neutral, and the pH is determined by the water, which is 7 at 25°C.
Conclude that the pH at the equivalence point for a strong acid-strong base titration is 7.
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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 (a solution of known concentration) to a sample solution until the reaction reaches its equivalence point, where the amount of titrant equals the amount of substance in the sample. Understanding the stoichiometry of the reaction is crucial for calculating concentrations and pH at various points during the titration.
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Percorso guidato
03:04
Acid-Base Titration
Equivalence Point
The equivalence point in a titration is the stage at which the amount of titrant added is stoichiometrically equivalent to the amount of substance present in the sample solution. At this point, the reaction between the acid and base is complete, and the pH of the solution can change dramatically. For strong acid-strong base titrations, the pH at the equivalence point is typically around 7, as the resulting solution contains only water and the salt formed from the neutralization.
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01:07At the Equivalence Point
pH Calculation
pH is a measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration. At the equivalence point of a strong acid-strong base titration, the pH can be calculated based on the complete neutralization of the acid and base. In this case, since HBr is a strong acid and KOH is a strong base, the resulting solution will have a neutral pH of 7, assuming no other factors influence the pH.
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02:15pH Calculation Example
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