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SOLVED: Suppose a chemist started with 152 g of salicylic acid and 86.8 g of acetic anhydride and produced 133 g of aspirin. What is the yield of this reaction? The balanced
VIDEO ANSWER: The balanced chemical reaction is provided with 2 moles alcilic acid, with 1 mole acidic and hydrate yields 2 moles of asperin. So we need to det…
numerade.com
2021年9月25日
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SOLVED: Write the equation, using the structural formula, for the neutralization reaction. Label the acid, base, conjugate acid, and conjugate base.The reaction for aspirin with sodium hydroxide:C9H8O4 (aq) NaOH (aq) → C9H7O4- Na H2O
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SOLVED: Aspirin can be made in the laboratory by reacting acetic anhydride (C4H6O3) with salicylic acid (C7H6O3) to form aspirin (C9H8O4) and acetic acid (C2H4O2). The balanced equation is: C4H6O3 C7H6O3-C9H8O4 C2H4O2In a laboratory synthesis, a student begins with 3.00 mL of acetic anhydride (density = 1.08 g>mL) and 1.25 g of salicylic acid. Once the reaction is complete, the student collects 1.22 g of aspirin. Determine the limiting reactant, theoretical yield of aspirin, and percent yiel
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SOLVED: Determine the percentage and milligrams of aspirin in each sample titrated. Back titration was used: Aspirin Tablet Weight: 0.68726788.2 mL total NaOH titrated HCl Titration: 20.4 mL HCl Final NaOH Titration: 2.5 mL NaOH Molarity of NaOH: 0.0907 M
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Purple violets contain salicylic acid, which is the chemical compound found in aspirin. Which means it's very good at reliving mild pain. It supports the respiratory system and cleanses the lymphatic system. Purple violets are rich in rutin, which is an antioxidant and helps reduce inflammation in the body. Keep in mind that when foraging, it's very important to do your own research from several trusted sources and do your own research. . . . . . #bringingbacklostskills #backyardforaging #purple
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Aspirin can be made in the laboratory by reacting acetic anhydride (C4H6O3) with salicylic acid (C7H6O3) to form aspirin (C9H8O4) and acetic acid (C2H4O2). The balanced equation is: C4H6O3 C7H6O3-C9H8O4 C2H4O2 In a laboratory synthesis, a student begins with 3.00 mL of acetic anhydride (density = 1.08 g>mL) and 1.25 g of salicylic acid. Once the reaction is complete, the student collects 1.22 g of aspirin. Determine the limiting reactant, theoretical yield of aspirin, and percent yield for t
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