Suppose you are titrating a sulfuric acid solution of unknown concentration with a sodium hydroxide solution according to the equation H2SO4 + 2 NaOH →2 H2O + Na2SO4 If you require 29.66 mL of 0.605 M NAOH solution to titrate 195.9 mL of H,SO4 solution, what is the concentration of the H2SO4 solution? Type answer:
Suppose you are titrating a sulfuric acid solution of unknown concentration with a sodium hydroxide solution according to the equation H2SO4 + 2 NaOH →2 H2O + Na2SO4 If you require 29.66 mL of 0.605 M NAOH solution to titrate 195.9 mL of H,SO4 solution, what is the concentration of the H2SO4 solution? Type answer:
Chemistry
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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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Question
![**Determining the Concentration of Sulfuric Acid through Titration**
Suppose you are titrating a sulfuric acid solution of unknown concentration with a sodium hydroxide solution according to the equation:
\[ \text{H}_2\text{SO}_4 + 2\text{NaOH} \longrightarrow 2\text{H}_2\text{O} + \text{Na}_2\text{SO}_4 \]
If you require 29.66 mL of 0.605 M \(\text{NaOH}\) solution to titrate 195.9 mL of \(\text{H}_2\text{SO}_4\) solution, what is the concentration of the \(\text{H}_2\text{SO}_4\) solution?
Type answer:
[ ]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffbfefd57-6cd5-45bf-b890-c343c2fceb41%2F908b12b2-f09d-40b9-8ed1-461cce58b7b6%2Frahy1g_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Determining the Concentration of Sulfuric Acid through Titration**
Suppose you are titrating a sulfuric acid solution of unknown concentration with a sodium hydroxide solution according to the equation:
\[ \text{H}_2\text{SO}_4 + 2\text{NaOH} \longrightarrow 2\text{H}_2\text{O} + \text{Na}_2\text{SO}_4 \]
If you require 29.66 mL of 0.605 M \(\text{NaOH}\) solution to titrate 195.9 mL of \(\text{H}_2\text{SO}_4\) solution, what is the concentration of the \(\text{H}_2\text{SO}_4\) solution?
Type answer:
[ ]
![### Titrating Vinegar (Acetic Acid Solution)
**Problem:**
Suppose you are titrating vinegar, which is an acetic acid solution of unknown concentration, with a sodium hydroxide solution according to the equation:
\[ \text{HC}_2\text{H}_3\text{O}_2 + \text{NaOH} \rightarrow \text{H}_2\text{O} + \text{NaC}_2\text{H}_3\text{O}_2 \]
If you require 33.45 mL of 0.1408 M NaOH solution to titrate 10.0 mL of HC₂H₃O₂ solution, what is the molar concentration of acetic acid in the vinegar?
**Type answer:**
[Answer text box for students to input their calculation]
### Explanation:
To find the molar concentration of acetic acid (\( \text{HC}_2\text{H}_3\text{O}_2 \)) in the vinegar, you can use the following steps:
1. **Write the balanced chemical equation**:
\[ \text{HC}_2\text{H}_3\text{O}_2 + \text{NaOH} \rightarrow \text{H}_2\text{O} + \text{NaC}_2\text{H}_3\text{O}_2 \]
2. **Convert the volume of NaOH solution used in the titration to liters**:
\[ 33.45 \, \text{mL} = 0.03345 \, \text{L} \]
3. **Calculate the moles of NaOH used**:
\[ \text{moles of NaOH} = \text{Molarity} \times \text{Volume} \]
\[ = 0.1408 \, \text{M} \times 0.03345 \, \text{L} \]
\[ = 0.00471116 \, \text{moles of NaOH} \]
4. **Use the stoichiometry of the balanced equation to determine the moles of acetic acid**:
From the balanced equation, we know that 1 mole of NaOH reacts with 1 mole of HC₂H₃O₂.
\[ \text{moles of HC}_2\text{H}_3](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffbfefd57-6cd5-45bf-b890-c343c2fceb41%2F908b12b2-f09d-40b9-8ed1-461cce58b7b6%2Fxphynxw_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Titrating Vinegar (Acetic Acid Solution)
**Problem:**
Suppose you are titrating vinegar, which is an acetic acid solution of unknown concentration, with a sodium hydroxide solution according to the equation:
\[ \text{HC}_2\text{H}_3\text{O}_2 + \text{NaOH} \rightarrow \text{H}_2\text{O} + \text{NaC}_2\text{H}_3\text{O}_2 \]
If you require 33.45 mL of 0.1408 M NaOH solution to titrate 10.0 mL of HC₂H₃O₂ solution, what is the molar concentration of acetic acid in the vinegar?
**Type answer:**
[Answer text box for students to input their calculation]
### Explanation:
To find the molar concentration of acetic acid (\( \text{HC}_2\text{H}_3\text{O}_2 \)) in the vinegar, you can use the following steps:
1. **Write the balanced chemical equation**:
\[ \text{HC}_2\text{H}_3\text{O}_2 + \text{NaOH} \rightarrow \text{H}_2\text{O} + \text{NaC}_2\text{H}_3\text{O}_2 \]
2. **Convert the volume of NaOH solution used in the titration to liters**:
\[ 33.45 \, \text{mL} = 0.03345 \, \text{L} \]
3. **Calculate the moles of NaOH used**:
\[ \text{moles of NaOH} = \text{Molarity} \times \text{Volume} \]
\[ = 0.1408 \, \text{M} \times 0.03345 \, \text{L} \]
\[ = 0.00471116 \, \text{moles of NaOH} \]
4. **Use the stoichiometry of the balanced equation to determine the moles of acetic acid**:
From the balanced equation, we know that 1 mole of NaOH reacts with 1 mole of HC₂H₃O₂.
\[ \text{moles of HC}_2\text{H}_3
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