Salicylic acid (FW = 138.12 g/mol), a reagent used to make aspirin, can itself b

Question

Salicylic acid (FW = 138.12 g/mol), a reagent used to make aspirin, can itself be produced from oil of wintergreen (methyl salicylate, FW = 152.15 g/mol, d = 1.18 g/mol at 20 ºC), by reacting it with sodium hydroxide. This reaction is shown below. You measured out 7.14 mL of oil of wintergreen and 9.59 g of sodium hydroxide (FW = 39.997 g/mol). Experimentally, you produced 6.48 g of salicylic acid. What is your percent yield for this reaction?

C8H8O3 + NaOH C7H6O3 + NaOCH3

Please provide me with aright answer and clear handwriting. Urgent

Explanation / Answer

from standard reaction it is clear that 1 mole of methyl salicylate will reacts with 1 mole of sodium hydroxide will produce 1 mole of salicylic acid.

here weight of methyl salicylate = 7.14 ml * 1.18 gm /cc = 8.4252 gm

mole of methyl salicylate = given weight/ molecular weight = 8.4252 gm / 152.15 g/mol = 0.055 mole

mole of sodium hydroxide = 9.59 gm / 39.997 g/mol = 0.239 mole.

therefore, methyl salicylate will be the limiting reagent. so, 0.055 mole of Salicylic acid will be formed.

weight of Salicylic acid will be = 0.055 mole * 138.12 g/mol = 7.5966 gm

experimentally, produced product is 6.48 gm

percent yield will be = ( 6.48 gm / 7.5966 gm) *100 % = 85.3 %

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