Calculate the volume (in mL) of a 0.300 M aqueous NaOH solution required to react completely with 32.5 mL of a 0.200 M aqueous solution of H,S04. H2SO4(aq) + 2 NaOH(aq) → NażSO4(aq) + 2 H20(1)
Calculate the volume (in mL) of a 0.300 M aqueous NaOH solution required to react completely with 32.5 mL of a 0.200 M aqueous solution of H,S04. H2SO4(aq) + 2 NaOH(aq) → NażSO4(aq) + 2 H20(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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![### Test Bank, Question 14.114
Calculate the volume (in mL) of a **0.300 M** aqueous NaOH solution required to react completely with **32.5 mL** of a **0.200 M** aqueous solution of **H₂SO₄**.
**Chemical reaction:**
\[ \text{H}_2\text{SO}_4(\text{aq}) + 2 \text{NaOH}(\text{aq}) \rightarrow \text{Na}_2\text{SO}_4(\text{aq}) + 2 \text{H}_2\text{O}(\text{l}) \]
\[ \text{Volume:} \quad \_\_\_\_\_\_\_\_ \text{mL} \]
**Note:** The tolerance is +/- 2%.
**Explanation:**
This problem involves using stoichiometry to determine the volume of a base (NaOH) needed to completely neutralize a given volume of an acid (H₂SO₄).
The balanced chemical equation shows that 1 mole of H₂SO₄ reacts with 2 moles of NaOH. Given the molarity and volume of H₂SO₄, you can find moles of H₂SO₄ and then use the stoichiometric relationship to find moles of NaOH required. Finally, using the molarity of the NaOH solution, you can determine the volume needed.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2f9e96de-8215-4532-a7d0-6f1fdf87f241%2Fb6f1b523-d519-464f-a7d0-a8bbb22ce807%2Ffzuysth.png&w=3840&q=75)
Transcribed Image Text:### Test Bank, Question 14.114
Calculate the volume (in mL) of a **0.300 M** aqueous NaOH solution required to react completely with **32.5 mL** of a **0.200 M** aqueous solution of **H₂SO₄**.
**Chemical reaction:**
\[ \text{H}_2\text{SO}_4(\text{aq}) + 2 \text{NaOH}(\text{aq}) \rightarrow \text{Na}_2\text{SO}_4(\text{aq}) + 2 \text{H}_2\text{O}(\text{l}) \]
\[ \text{Volume:} \quad \_\_\_\_\_\_\_\_ \text{mL} \]
**Note:** The tolerance is +/- 2%.
**Explanation:**
This problem involves using stoichiometry to determine the volume of a base (NaOH) needed to completely neutralize a given volume of an acid (H₂SO₄).
The balanced chemical equation shows that 1 mole of H₂SO₄ reacts with 2 moles of NaOH. Given the molarity and volume of H₂SO₄, you can find moles of H₂SO₄ and then use the stoichiometric relationship to find moles of NaOH required. Finally, using the molarity of the NaOH solution, you can determine the volume needed.
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