Ch.18 - Aqueous Ionic Equilibrium

Tro - Chemistry: A Molecular Approach 6th Edition

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Tro 6th Edition

Ch.18 - Aqueous Ionic Equilibrium

Problem 73c

Chapter 18, Problem 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

Name: Chemistry: A Molecular Approach
Author: Tro
ISBN: 9780137832217

Verified step by step guidance

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.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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.

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.

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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Related Practice

Textbook Question

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

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

Consider the curve shown here for the titration of a weak base with a strong acid and answer each question.

d. At what volume of added acid is the pH calculated by working an equilibrium problem based on the concentration and K_a of the conjugate acid?

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Textbook Question

Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine each quantity. b. the volume of added base required to reach the equivalence point

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Textbook Question

Consider the titration of a 25.0-mL sample of 0.115 M RbOH with 0.100 M HCl. Determine each quantity. b. the volume of added acid required to reach the equivalence point

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