**Understanding Chemical Reactions: Sulfuric Acid and Water Interaction**Consider the following chemical reaction and the fact that H\(_2\)SO\(_4\) (sulfuric acid) is a strong acid:\[ \text{H}_2\text{SO}_4 + \text{H}_2\text{O} \rightarrow \text{HSO}_4^- + \text{H}_3\text{O}^+ \]If 0.0005 moles of H\(_2\)SO\(_4\) react with water, how many moles of H\(_2\)SO\(_4\) remain?### Options:- ∘ 0- ∘ 0.0005- ∘ 0.001- ∘ 1### Explanation:In this reaction, H\(_2\)SO\(_4\) dissociates completely in water, as it is a strong acid. Therefore, the number of moles of H\(_2\)SO\(_4\) that react would be completely converted into HSO\(_4\)⁻ and H\(_3\)O\(^+\). Thus, 0.0005 moles of H\(_2\)SO\(_4\) will be entirely used up in the reaction, leaving 0 moles remaining.Understanding this complete dissociation is crucial for solving similar problems in chemistry, highlighting the nature of strong acids in aqueous solutions.*[No graphs or diagrams accompany this problem in the provided image.]*

Acids are chemical compounds that give H+ ions in the aqueous solution and dissociate completely.

Consider the following chemical reaction and that H₂SO4 is a strong acid: H₂SO4 + H₂O HSO4 + H3O+. If 0.0005 moles of H₂SO4 reacts with water, how many moles of H₂SO4 remain? 0 0.0005 0.001 1 ====

Consider the following chemical reaction and that H₂SO4 is a strong acid: H₂SO4 + H₂O HSO4 + H3O+. If 0.0005 moles of H₂SO4 reacts with water, how many moles of H₂SO4 remain? 0 0.0005 0.001 1 ====

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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Question

**Understanding Chemical Reactions: Sulfuric Acid and Water Interaction**

Consider the following chemical reaction and the fact that H\(_2\)SO\(_4\) (sulfuric acid) is a strong acid:

\[ \text{H}_2\text{SO}_4 + \text{H}_2\text{O} \rightarrow \text{HSO}_4^- + \text{H}_3\text{O}^+ \]

If 0.0005 moles of H\(_2\)SO\(_4\) react with water, how many moles of H\(_2\)SO\(_4\) remain?

### Options:

- ∘ 0
- ∘ 0.0005
- ∘ 0.001
- ∘ 1

### Explanation:

In this reaction, H\(_2\)SO\(_4\) dissociates completely in water, as it is a strong acid. Therefore, the number of moles of H\(_2\)SO\(_4\) that react would be completely converted into HSO\(_4\)⁻ and H\(_3\)O\(^+\). Thus, 0.0005 moles of H\(_2\)SO\(_4\) will be entirely used up in the reaction, leaving 0 moles remaining.

Understanding this complete dissociation is crucial for solving similar problems in chemistry, highlighting the nature of strong acids in aqueous solutions.

*[No graphs or diagrams accompany this problem in the provided image.]*

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