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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I need help with how many miles there must have been in the sample?
![**Lab: Titration of HCl with Standardized NaOH**
**Purpose:**
To determine the molarity of an HCl solution using titration.
**Materials:**
- NaOH: a caustic base, wear goggles.
- HCl: a caustic acid, wear goggles.
**Data:**
- Draw a sketch of your titration set-up with labels.
**Trial 1:**
- Volume of HCl sample = 15 mL
- Molarity of standardized NaOH solution = 0.0826 M
- Initial burette reading = 3.25 mL NaOH
- Final burette reading = 32.22 mL NaOH
**Trial 2:**
- Volume of HCl sample = 15 mL
- Molarity of standardized NaOH solution = 0.0826 M
- Initial burette reading = 3.00 mL NaOH
- Final burette reading = 32.25 mL NaOH
**Calculations:**
Write the equation for the neutralization of HCl with NaOH:
\[ \text{HCl} + \text{NaOH} \rightarrow \text{NaCl} + \text{H}_2\text{O} \]
**Volume of NaOH used:**
\[ \text{Volume of NaOH used} = \_\_\_\_ \]
1. **How many moles of NaOH were used to reach the equivalence point?**
(Show your work)
\[ 0.029 \]
2. **How many moles of HCl must therefore have been in the sample?**
\[ n = c \cdot v \]
3. **What then is the molarity of the HCl sample?**
(Show your work)
\[ 0.1064 \, \text{M} \]
*Note: The sketch includes a basic representation of a titration setup with a labeled burette, flask, and the liquids involved.*](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F28746eb8-fb04-40b3-ae3d-9a87714544e8%2Fe6e97fc5-eecb-489c-8b64-77a8f68b8ae7%2Fj6jygk.jpeg&w=3840&q=75)
Transcribed Image Text:**Lab: Titration of HCl with Standardized NaOH**
**Purpose:**
To determine the molarity of an HCl solution using titration.
**Materials:**
- NaOH: a caustic base, wear goggles.
- HCl: a caustic acid, wear goggles.
**Data:**
- Draw a sketch of your titration set-up with labels.
**Trial 1:**
- Volume of HCl sample = 15 mL
- Molarity of standardized NaOH solution = 0.0826 M
- Initial burette reading = 3.25 mL NaOH
- Final burette reading = 32.22 mL NaOH
**Trial 2:**
- Volume of HCl sample = 15 mL
- Molarity of standardized NaOH solution = 0.0826 M
- Initial burette reading = 3.00 mL NaOH
- Final burette reading = 32.25 mL NaOH
**Calculations:**
Write the equation for the neutralization of HCl with NaOH:
\[ \text{HCl} + \text{NaOH} \rightarrow \text{NaCl} + \text{H}_2\text{O} \]
**Volume of NaOH used:**
\[ \text{Volume of NaOH used} = \_\_\_\_ \]
1. **How many moles of NaOH were used to reach the equivalence point?**
(Show your work)
\[ 0.029 \]
2. **How many moles of HCl must therefore have been in the sample?**
\[ n = c \cdot v \]
3. **What then is the molarity of the HCl sample?**
(Show your work)
\[ 0.1064 \, \text{M} \]
*Note: The sketch includes a basic representation of a titration setup with a labeled burette, flask, and the liquids involved.*
Expert Solution
Step 1
Using the data provided, the number of moles of NaOH used in the titration can be calculated. This can then be used to arrive at the number of moles of HCl that must have been present in the sample as one mole of NaOH can neutralize one mole of HCl
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