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 ====
Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter6: Solutions And Colloids
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Problem 6.78P: 6-78 (Chemical Connections 6A) Oxides of nitrogen (NO, NO2,N2O3) are also responsible for acid rain....
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![**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.]*](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Febe45f5d-5c04-4921-8d3a-3c73b83ec869%2F7a1f3877-f087-4b1d-9bac-79d81e6bbb04%2Fnt4zne5_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**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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