[Unreacted salicylic acid, traces of acetic acid.]
Mass of salicylic acid = 3.03 grams. [Slow reaction with
2.608g is the theoretical yield of aspirin Sign up to view the entire interaction 121.2 g of
purity by measuring how much carbon dioxide is given off. of vacuum filtration, if available, will facilitate the filtration. in a test-tube rack, and then add the contents to a 100-mL beaker containing 4-5 ice
We welcome your feedback, comments and questions about this site or page. Salicylic acid and its derivatives are antipyretics. Place the flask in this ice-water bath, making sure no water is spilled into the flask. Erlenmeyer flask any big lumps of solid should be broken up. Heat the mixture in a water bath for 5 min. Remove the test-tube, cool it
C4H6O3+C7H6O3→C9H8O4+C2H4O2. What commercial products contain oil of wintergreen? 102, From experimental data, moles of ethanoic anhydride = 15/102 = 0.147 Fe(OH)2 + Na2SO4, 2 moles of sodium hydroxide react with 1 mole of iron(II) sulfate, From the data given,, moles of iron(II) sulfate = 0.05 x 1 = 0.05 moles, This would require 0.05 x 2 = 0.1 moles of sodium hydroxide. If you have 3.0 moles of argon gas at STP, how much volume will the argon take up?
Calculate the theoretical yield of aspirin if you start with 3.0gof salicylic acid and 8.0ml of acetic anhydride.
Walk around room during laboratory exercise emphasizing
salicylic acid and 1mL methanol. Ferric Chloride Test for Phenols Clean two watch glasses. Synthesis Weigh by taring approximately 2 g of salicylic acid into a clean and dry 50 ml. Try the free Mathway calculator and
Step 2: Change
2g iron(III) nitrate nonahydrate [Fe(NO 3 ) 3 . Use a glass stir rod to stir the mixture and break up any remaining lumps of solid. IB Chemistry home > Syllabus © 2020 Education Expert, All rights reserved. of the product may be even more important. the grams from the volume, Step 3: Calculate
The percent purity of a sample describes what proportion of that
Concentrated sulfuric acid should be dispensed from a small dropping bottle. is established. Molecular mass of aspirin = 180.157 g/mol (180.157 g/mol) (0.01448 mol) = 2.608g of aspirin Is this correct? The
& [Wintergreen Life-Savers, Ben-Gay, etc.] It does not matter whether moles or mass is used for the calculation as long % Yield Actual Yield * 100 % Theoretical Yield 3.
moisture in air can produce small amounts of vinegar.] and the chemical formula for aspirin is C9H8O4. aspirin. The theoretical yield of aspirin is 3.95 grams. Set up mineral oil baths
This is a discussion boar for my chemistry class. So for one mole of salicylic acid used one mole of aspirin is used too.
The percentage is obtained by multiplying this fraction by 100.
The absorbance is proportional to the
(X) g of aspirin, % Yield = (Practical Yield)/(Theoretical Yield) × 100, Aspirin was synthesized and the yield was found to be ——— %. Its lumes cause a burning sensation in the eyes.
Assessing Laboratory Learning
Waft the odor toward thenose. as the two units are not used at the same time.
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