25) Ammonia and sulfuric acid react according to the equation given below. SA 2 NH3(aq) + H₂SO4(aq) → (NH4)2SO4(aq) How many milliliters of 0.110 M sulfuric acid are required to exactly neutralize 25.0 mL of 0.0840 M NH3 solution?
25) Ammonia and sulfuric acid react according to the equation given below. SA 2 NH3(aq) + H₂SO4(aq) → (NH4)2SO4(aq) How many milliliters of 0.110 M sulfuric acid are required to exactly neutralize 25.0 mL of 0.0840 M NH3 solution?
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.
Question
![**Problem Statement:**
Ammonia and sulfuric acid react according to the equation given below.
\[2 \text{NH}_3(\text{aq}) + \text{H}_2\text{SO}_4(\text{aq}) \rightarrow (\text{NH}_4)_2\text{SO}_4(\text{aq})\]
**Question:**
How many milliliters of 0.110 M sulfuric acid are required to exactly neutralize 25.0 mL of 0.0840 M NH₃ solution?
**Explanation:**
The chemical equation shows that 2 moles of NH₃ react with 1 mole of H₂SO₄ to produce ammonium sulfate. The stoichiometry from the balanced equation is used to determine the amount of sulfuric acid needed to neutralize the given ammonia solution.
**Calculations:**
1. Determine the moles of NH₃:
\[\text{Moles of NH}_3 = \text{Volume} \times \text{Molarity} = 0.0250 \, \text{L} \times 0.0840 \, \text{mol/L}\]
2. Use the stoichiometry of the reaction to find the moles of H₂SO₄ required.
3. Calculate the volume of H₂SO₄ needed using its molarity:
\[\text{Volume of H}_2\text{SO}_4 = \frac{\text{Moles of H}_2\text{SO}_4}{\text{Molarity of H}_2\text{SO}_4}\]
By following these steps, you will be able to determine the exact volume of sulfuric acid required for the neutralization.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F527d0796-f7b0-4877-ad88-5fb65d7b09e0%2F878aa7a1-c2ed-4ceb-aae6-7bb059cf4f35%2Flfuzrnr_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
Ammonia and sulfuric acid react according to the equation given below.
\[2 \text{NH}_3(\text{aq}) + \text{H}_2\text{SO}_4(\text{aq}) \rightarrow (\text{NH}_4)_2\text{SO}_4(\text{aq})\]
**Question:**
How many milliliters of 0.110 M sulfuric acid are required to exactly neutralize 25.0 mL of 0.0840 M NH₃ solution?
**Explanation:**
The chemical equation shows that 2 moles of NH₃ react with 1 mole of H₂SO₄ to produce ammonium sulfate. The stoichiometry from the balanced equation is used to determine the amount of sulfuric acid needed to neutralize the given ammonia solution.
**Calculations:**
1. Determine the moles of NH₃:
\[\text{Moles of NH}_3 = \text{Volume} \times \text{Molarity} = 0.0250 \, \text{L} \times 0.0840 \, \text{mol/L}\]
2. Use the stoichiometry of the reaction to find the moles of H₂SO₄ required.
3. Calculate the volume of H₂SO₄ needed using its molarity:
\[\text{Volume of H}_2\text{SO}_4 = \frac{\text{Moles of H}_2\text{SO}_4}{\text{Molarity of H}_2\text{SO}_4}\]
By following these steps, you will be able to determine the exact volume of sulfuric acid required for the neutralization.
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