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If the barium sulfate precipitate is not dried thoroughly, will the experimentally determined concentration be higher or lower than the true value? Concisely explain based on how the molarity is calculated.

If the barium sulfate precipitate is not dried thoroughly, will the experimentally determined concentration be higher or lower than the true value? Concisely explain based on how the molarity is calculated.

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
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If the barium sulfate precipitate is not dried thoroughly, will the experimentally determined concentration be higher or lower than the true value? Concisely explain based on how the molarity is calculated.
C. Questions 1. Why isn't the mass of potassium sulfate used in any of the calculations? 2. If the barium sulfate precipitate is not dried thoroughly, will the experimentally determined concentration be higher or lower than the true value? Concisely explain based on how the molarity is calculated. 3. An experimenter reacts 30.0 mL of a BaCl, solution with excess AgNO, as shown in the unbalanced equation below. If 2.58 grams of AgCl are obtained, what is the molarity of BaCl₂ solution? Hint: First balance the chemical equation. BaCl₂ (aq) + AgNO3(aq) 22 3)2(aq)
Transcribed Image Text:C. Questions 1. Why isn't the mass of potassium sulfate used in any of the calculations? 2. If the barium sulfate precipitate is not dried thoroughly, will the experimentally determined concentration be higher or lower than the true value? Concisely explain based on how the molarity is calculated. 3. An experimenter reacts 30.0 mL of a BaCl, solution with excess AgNO, as shown in the unbalanced equation below. If 2.58 grams of AgCl are obtained, what is the molarity of BaCl₂ solution? Hint: First balance the chemical equation. BaCl₂ (aq) + AgNO3(aq) 22 3)2(aq)
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