## Titration of Sulfuric Acid with Lithium Hydroxide### Problem StatementA solution of 25.0 mL of 0.40 M \( \text{H}_2\text{SO}_4 \) is titrated with 0.50 M \( \text{LiOH} \).The balanced chemical equation for the reaction is: \[ \text{H}_2\text{SO}_4 + 2\text{LiOH} \rightarrow \text{Li}_2\text{SO}_4 + 2\text{H}_2\text{O} \]### QuestionWhat volume of \( \text{LiOH} \) is required to neutralize the acid completely?### CalculationTo find the volume of \( \text{LiOH} \) needed, you will use the stoichiometry of the balanced equation. Note the mole ratios between \( \text{H}_2\text{SO}_4 \) and \( \text{LiOH} \).\[ \text{Vol LiOH} = \text{? mL} \]### HintBe careful of the mole ratios!### User InteractionYou can input the calculated volume of \( \text{LiOH} \) in the text box below and click "Enter" to check your answer.\[ \text{Vol LiOH (mL)} \quad \boxed{\input{}}\]### ExplanationIn this problem, you are given the following information:- Volume and molarity of \( \text{H}_2\text{SO}_4 \): \( V_{\text{H}_2\text{SO}_4} = 25.0 \) mL and \( M_{\text{H}_2\text{SO}_4} = 0.40 \) M- Molarity of \( \text{LiOH} \): \( M_{\text{LiOH}} = 0.50 \) MYou need to determine the volume of \( \text{LiOH} \) required to neutralize the \( \text{H}_2\text{SO}_4 \). The balanced chemical equation provides you with the mole ratio:\[ 1 \text{ mole } \text{H}_2\text{SO}_4 : 2 \text{ moles } \text{LiOH} \]By using stoichi

Given, H2SO4 + 2LiOH → Li2SO4 + 2H2O Molarity of H2SO4 solution = 0.40 M = 0.40 mol/L Volume of the…

A solution of 25.0 mL of 0.40 M H2SO4 is titrated with 0.50 M of LiOH. H₂SO4 + 2LiOH →>> Li₂SO4 + 2H₂O What volume of LiOH is required to neutralize the acid completely? Vol LiOH [?] mL Hint: Be careful of the mole ratios! Vol LiOH (mL) Enter

A solution of 25.0 mL of 0.40 M H2SO4 is titrated with 0.50 M of LiOH. H₂SO4 + 2LiOH →>> Li₂SO4 + 2H₂O What volume of LiOH is required to neutralize the acid completely? Vol LiOH [?] mL Hint: Be careful of the mole ratios! Vol LiOH (mL) Enter

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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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

## Titration of Sulfuric Acid with Lithium Hydroxide

### Problem Statement

A solution of 25.0 mL of 0.40 M \( \text{H}_2\text{SO}_4 \) is titrated with 0.50 M \( \text{LiOH} \).

The balanced chemical equation for the reaction is:

\[ \text{H}_2\text{SO}_4 + 2\text{LiOH} \rightarrow \text{Li}_2\text{SO}_4 + 2\text{H}_2\text{O} \]

### Question

What volume of \( \text{LiOH} \) is required to neutralize the acid completely?

### Calculation

To find the volume of \( \text{LiOH} \) needed, you will use the stoichiometry of the balanced equation. Note the mole ratios between \( \text{H}_2\text{SO}_4 \) and \( \text{LiOH} \).

\[ \text{Vol LiOH} = \text{? mL} \]

### Hint

Be careful of the mole ratios!

### User Interaction

You can input the calculated volume of \( \text{LiOH} \) in the text box below and click "Enter" to check your answer.

\[ \text{Vol LiOH (mL)} \quad \boxed{\input{}}\]

### Explanation

In this problem, you are given the following information:
- Volume and molarity of \( \text{H}_2\text{SO}_4 \): \( V_{\text{H}_2\text{SO}_4} = 25.0 \) mL and \( M_{\text{H}_2\text{SO}_4} = 0.40 \) M
- Molarity of \( \text{LiOH} \): \( M_{\text{LiOH}} = 0.50 \) M

You need to determine the volume of \( \text{LiOH} \) required to neutralize the \( \text{H}_2\text{SO}_4 \). The balanced chemical equation provides you with the mole ratio:

\[ 1 \text{ mole } \text{H}_2\text{SO}_4 : 2 \text{ moles } \text{LiOH} \]

By using stoichi

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