A titration flask contains 0.00425 moles of an acetic acid sample a. Determine the moles of the base (NaOH) required to completely neutralize the acid. b. If the molarity of the based added from the buret was 0.200 M, determine the volume of the base (in mL) required to reach the end point of this titration. H Type here to search NG Info W
A titration flask contains 0.00425 moles of an acetic acid sample a. Determine the moles of the base (NaOH) required to completely neutralize the acid. b. If the molarity of the based added from the buret was 0.200 M, determine the volume of the base (in mL) required to reach the end point of this titration. H Type here to search NG Info W
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...
Related questions
Concept explainers
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Question
100%
![### Titration Problem and Solution Explanation
#### Problem Statement:
4. A titration flask contains 0.00425 moles of an acetic acid sample.
a. Determine the moles of the base (NaOH) required to completely neutralize the acid.
b. If the molarity of the base added from the buret was 0.200 M, determine the volume of the base (in mL) required to reach the endpoint of this titration.
#### Solution:
**Part a:**
To determine the moles of the base (NaOH) required to completely neutralize the acid, consider that acetic acid (CH₃COOH) reacts with sodium hydroxide (NaOH) in a 1:1 molar ratio. The balanced chemical equation for this reaction is:
\[ \text{CH}_3\text{COOH} + \text{NaOH} \rightarrow \text{CH}_3\text{COONa} + \text{H}_2\text{O} \]
From the equation, it is clear that 1 mole of acetic acid reacts with 1 mole of NaOH.
Given:
\[ \text{Moles of acetic acid} = 0.00425 \text{ moles} \]
Since the molar ratio is 1:1:
\[ \text{Moles of NaOH required} = 0.00425 \text{ moles} \]
**Part b:**
To find the volume of the base (NaOH) needed, we use the molarity (M) of the NaOH solution provided:
\[ \text{Molarity (M)} = \frac{\text{Moles of solute}}{\text{Liters of solution}} \]
Given the molarity of the NaOH solution:
\[ \text{Molarity (M)} = 0.200 \text{ M} \]
We need to determine the volume (V) of the NaOH solution required to provide 0.00425 moles of NaOH.
Using the formula:
\[ \text{Moles} = \text{Molarity} \times \text{Volume (L)} \]
\[ 0.00425 = 0.200 \times V \]
Solving for V:
\[ V = \frac{0.00425}{0.200} \]
\[ V = 0.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6c1368ea-8a90-45d4-955c-b2170f8018f8%2Fb9779ca7-be8d-4d51-9e35-35e4a1575754%2F1lqfybc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Titration Problem and Solution Explanation
#### Problem Statement:
4. A titration flask contains 0.00425 moles of an acetic acid sample.
a. Determine the moles of the base (NaOH) required to completely neutralize the acid.
b. If the molarity of the base added from the buret was 0.200 M, determine the volume of the base (in mL) required to reach the endpoint of this titration.
#### Solution:
**Part a:**
To determine the moles of the base (NaOH) required to completely neutralize the acid, consider that acetic acid (CH₃COOH) reacts with sodium hydroxide (NaOH) in a 1:1 molar ratio. The balanced chemical equation for this reaction is:
\[ \text{CH}_3\text{COOH} + \text{NaOH} \rightarrow \text{CH}_3\text{COONa} + \text{H}_2\text{O} \]
From the equation, it is clear that 1 mole of acetic acid reacts with 1 mole of NaOH.
Given:
\[ \text{Moles of acetic acid} = 0.00425 \text{ moles} \]
Since the molar ratio is 1:1:
\[ \text{Moles of NaOH required} = 0.00425 \text{ moles} \]
**Part b:**
To find the volume of the base (NaOH) needed, we use the molarity (M) of the NaOH solution provided:
\[ \text{Molarity (M)} = \frac{\text{Moles of solute}}{\text{Liters of solution}} \]
Given the molarity of the NaOH solution:
\[ \text{Molarity (M)} = 0.200 \text{ M} \]
We need to determine the volume (V) of the NaOH solution required to provide 0.00425 moles of NaOH.
Using the formula:
\[ \text{Moles} = \text{Molarity} \times \text{Volume (L)} \]
\[ 0.00425 = 0.200 \times V \]
Solving for V:
\[ V = \frac{0.00425}{0.200} \]
\[ V = 0.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 1 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY