Question

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

Answer 1

5.07×10^-2

Step-by-step explanation:

in case they want it to be written out instead of the plain answer

Answer 2

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* 10^(-4)moles`

Formula used :

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

or,
`\text{ Mass of ascorbic acid}=\text{ Moles of ascorbic acid}* \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* 10^(-4)moles)* (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.