Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Titration Problem: Calculating Halfway Point Volume**
**Question:**
In the titration of 180.0 mL of 0.4000 M HONH₂ with 0.2000 M HBr, how many mL of HBr are required to reach the halfway point?
**Instructions:**
In this problem, you are tasked with determining the volume of hydrobromic acid (HBr) solution needed to reach the halfway point in the titration process with hydroxylamine (HONH₂).
**Understanding the Halfway Point:**
The halfway point in a titration involving a weak base (such as HONH₂) and a strong acid (HBr) is where half of the base has reacted with the acid. At this stage, the concentration of the base equals the concentration of its conjugate acid.
**Calculation Steps:**
1. Determine the initial moles of HONH₂ using its volume and molarity:
\[
\text{Moles of HONH₂} = 180.0 \, \text{mL} \times 0.4000 \, \frac{\text{mol}}{\text{L}}
\]
2. Calculate the moles required to reach the halfway point:
\[
\text{Halfway moles of HONH₂} = \frac{\text{Initial moles of HONH₂}}{2}
\]
3. Calculate the volume of 0.2000 M HBr needed to deliver the halfway moles:
\[
\text{Volume of HBr} = \frac{\text{Halfway moles of HONH₂}}{0.2000 \, \frac{\text{mol}}{\text{L}}}
\]
Use the interface calculator to input these calculations and find the required volume of HBr.
**Interface:**
This page features a calculator with standard numerical entry and functions, useful for performing the required calculations to solve the problem.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6895f9cd-8521-4c9a-bc62-df11c4ac3cae%2F56cffff1-0d92-4d38-8e73-12aeff33f092%2Fy4zucqr_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Titration Problem: Calculating Halfway Point Volume**
**Question:**
In the titration of 180.0 mL of 0.4000 M HONH₂ with 0.2000 M HBr, how many mL of HBr are required to reach the halfway point?
**Instructions:**
In this problem, you are tasked with determining the volume of hydrobromic acid (HBr) solution needed to reach the halfway point in the titration process with hydroxylamine (HONH₂).
**Understanding the Halfway Point:**
The halfway point in a titration involving a weak base (such as HONH₂) and a strong acid (HBr) is where half of the base has reacted with the acid. At this stage, the concentration of the base equals the concentration of its conjugate acid.
**Calculation Steps:**
1. Determine the initial moles of HONH₂ using its volume and molarity:
\[
\text{Moles of HONH₂} = 180.0 \, \text{mL} \times 0.4000 \, \frac{\text{mol}}{\text{L}}
\]
2. Calculate the moles required to reach the halfway point:
\[
\text{Halfway moles of HONH₂} = \frac{\text{Initial moles of HONH₂}}{2}
\]
3. Calculate the volume of 0.2000 M HBr needed to deliver the halfway moles:
\[
\text{Volume of HBr} = \frac{\text{Halfway moles of HONH₂}}{0.2000 \, \frac{\text{mol}}{\text{L}}}
\]
Use the interface calculator to input these calculations and find the required volume of HBr.
**Interface:**
This page features a calculator with standard numerical entry and functions, useful for performing the required calculations to solve the problem.
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