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Amiraneli [1.4K]
3 years ago
14

Ascorbic acid, or vitamin C (C6H8O6, molar mass = 176 g/mol), is a naturally occurring organic compound with antioxidant propert

ies. A healthy adult’s daily requirement of vitamin C is 70-90 mg. A sweet lime contains 2.88×10−4 mol of ascorbic acid. To determine whether the ascorbic acid in a sweet lime meets the daily requirement, calculate the mass of ascorbic acid in 2.88×10−4 mol of ascorbic acid.
Chemistry
1 answer:
nydimaria [60]3 years ago
5 0

Answer : 50.69 mg of ascorbic acid does not meet the daily requirement.

Solution : Given,

Molar mass of Ascorbic acid = 176 g/mole

Moles of Ascorbic acid = 2.88\times 10^{-4}moles

Formula used :

Moles=\frac{Mass}{\text{ Molar mass}}

or, \text{ Mass of ascorbic acid}=\text{ Moles of ascorbic acid}\times \text{ Molar mass of ascorbic acid}

Now put all the given values in this formula, we get the mass of ascorbic acid.

\text{ Mass of ascorbic acid}=(2.88\times 10^{-4}moles)\times (176g/mole)=0.050688g=50.69mg

Conversion : (1g=1000mg)

As per question, a healthy adult’s daily requirement of vitamin C is 70-90 mg. But calculate mass of vitamin C is 50.69 mg. So, 50.69 mg of ascorbic acid does not meet the daily requirement.

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