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A #1.961*g# mass of #"salicylic acid"#, #C_6H_4(CO_2H)(OH)# is treated with excess acetic acid. How much #"ASA, i.e. aspirin"#, i.e. #"1,2-C"_6"H"_4"CO"_2"H(O"_2"CCH"_3")"# could be prepared?

Answer 1

Approx. #2.6*g#...................

Initially, we must suggest a stoichiometric equation for the synthesis of aspirin:

#"1,2-C"_6"H"_4("CO"_2"H)(OH)" + "HO"_2"CCH"_3 rarr "1,2-C"_6"H"_4"CO"_2"H(O"_2"CCH"_3) + "H"_2"O"#

Thus, we can observe that the synthesis of ASA is a 1:1 reaction involving acetic acid and salicylic acid. What kind of reaction is this?

#"Moles of salicylic acid"=(1.961*g)/(138.12*g*mol^-1)=0.0142*"mol"#.

Given this molar quantity, and the stoichiometric equation, AT MOST we can make #0.0142*"mol"xx180.16*"g"*"mol"^-1=# #2.56*g# of #"ASA"#.

Because aspirin is one of the most potent, practical, and safe medications known, as well as because it has been prescribed widely as a blood thinner in recent years, aspirin synthesis is carried out on a massive industrial scale.

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Answer 2

Noah Aldrich

The molar mass of salicylic acid is 138.12 g/mol. The molar mass of acetic acid is 60.05 g/mol. The balanced equation for the reaction between salicylic acid and acetic acid to form aspirin is:

C6H4(CO2H)(OH) + CH3COOH -> C6H4(CO2CH3)(CO2H) + H2O

The theoretical yield of aspirin can be calculated using the molar ratio between salicylic acid and aspirin. The molar ratio is 1:1. Therefore, the theoretical yield of aspirin is equal to the mass of salicylic acid (1.961 g) divided by its molar mass, multiplied by the molar mass of aspirin (180.16 g/mol).

Theoretical yield of aspirin = (1.961 g / 138.12 g/mol) * 180.16 g/mol = 2.56 g

Therefore, the maximum amount of aspirin that could be prepared is 2.56 grams.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.