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(a) How much concentrated sulfuric acid (H₂SO4) (17.8 M) is needed to prepare 8.4 L of 1.5 M sulfuric acid solution? L of 17.8 M H₂SO4 must be diluted to a volume of 8.4 L (assume volumes are additive) (b) How many moles of H₂SO4 are in each milliliter of the original concentrate? 0.0178 mol H₂SO4 in each mL of the original concentrate (c) How many moles are in each milliliter of the diluted solution? 0.0015 mol H₂SO4 in each mL of the diluted solution

(a) How much concentrated sulfuric acid (H₂SO4) (17.8 M) is needed to prepare 8.4 L of 1.5 M sulfuric acid solution? L of 17.8 M H₂SO4 must be diluted to a volume of 8.4 L (assume volumes are additive) (b) How many moles of H₂SO4 are in each milliliter of the original concentrate? 0.0178 mol H₂SO4 in each mL of the original concentrate (c) How many moles are in each milliliter of the diluted solution? 0.0015 mol H₂SO4 in each mL of the diluted solution

Chemistry
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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I've already put in 7.7L and 7.692L as my answers but they're both wrong.

The exercise displayed on the website is part of a chemistry problem involving dilution and concentration of sulfuric acid (H₂SO₄). The solution's concentration and volume changes are calculated based on the dilution formula. Here is the transcription of the text: --- **Your answer is partially correct.** **(a)** How much concentrated sulfuric acid (H₂SO₄) (17.8 M) is needed to prepare 8.4 L of 1.5 M sulfuric acid solution? ⬛ L of 17.8 M H₂SO₄ must be diluted to a volume of 8.4 L (assume volumes are additive). **(b)** How many moles of H₂SO₄ are in each milliliter of the original concentrate? 0.0178 mol H₂SO₄ in each mL of the original concentrate. **(c)** How many moles are in each milliliter of the diluted solution? 0.0015 mol H₂SO₄ in each mL of the diluted solution. --- **eTextbook and Media** **Hint** \( M_1V_1 = M_2V_2 \) **Assistance Used** --- The dilution formula \( M_1V_1 = M_2V_2 \) is provided as a hint, where \( M_1 \) and \( M_2 \) are the molarities of the concentrated and diluted solutions, respectively, and \( V_1 \) and \( V_2 \) are their respective volumes. This formula is used to solve dilution problems by equating the product of the concentration and volume of the concentrated solution to that of the diluted solution.
Transcribed Image Text:The exercise displayed on the website is part of a chemistry problem involving dilution and concentration of sulfuric acid (H₂SO₄). The solution's concentration and volume changes are calculated based on the dilution formula. Here is the transcription of the text: --- **Your answer is partially correct.** **(a)** How much concentrated sulfuric acid (H₂SO₄) (17.8 M) is needed to prepare 8.4 L of 1.5 M sulfuric acid solution? ⬛ L of 17.8 M H₂SO₄ must be diluted to a volume of 8.4 L (assume volumes are additive). **(b)** How many moles of H₂SO₄ are in each milliliter of the original concentrate? 0.0178 mol H₂SO₄ in each mL of the original concentrate. **(c)** How many moles are in each milliliter of the diluted solution? 0.0015 mol H₂SO₄ in each mL of the diluted solution. --- **eTextbook and Media** **Hint** \( M_1V_1 = M_2V_2 \) **Assistance Used** --- The dilution formula \( M_1V_1 = M_2V_2 \) is provided as a hint, where \( M_1 \) and \( M_2 \) are the molarities of the concentrated and diluted solutions, respectively, and \( V_1 \) and \( V_2 \) are their respective volumes. This formula is used to solve dilution problems by equating the product of the concentration and volume of the concentrated solution to that of the diluted solution.
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