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](https://tex.z-dn.net/?f=2.88%5Ctimes%2010%5E%7B-4%7Dmoles)
Formula used :
![Moles=\frac{Mass}{\text{ Molar mass}}](https://tex.z-dn.net/?f=Moles%3D%5Cfrac%7BMass%7D%7B%5Ctext%7B%20Molar%20mass%7D%7D)
or, ![\text{ Mass of ascorbic acid}=\text{ Moles of ascorbic acid}\times \text{ Molar mass of ascorbic acid}](https://tex.z-dn.net/?f=%5Ctext%7B%20Mass%20of%20ascorbic%20acid%7D%3D%5Ctext%7B%20Moles%20of%20ascorbic%20acid%7D%5Ctimes%20%5Ctext%7B%20Molar%20mass%20of%20ascorbic%20acid%7D)
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](https://tex.z-dn.net/?f=%5Ctext%7B%20Mass%20of%20ascorbic%20acid%7D%3D%282.88%5Ctimes%2010%5E%7B-4%7Dmoles%29%5Ctimes%20%28176g%2Fmole%29%3D0.050688g%3D50.69mg)
Conversion : ![(1g=1000mg)](https://tex.z-dn.net/?f=%281g%3D1000mg%29)
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.
Solutions containing two substances in the aqueous phase are usually described in volume percentages. Therefore, if a solution has 30% of ethanol, then it has 30% ethanol by volume. The remaining volume is of water, which will be 70%. Calculating:
70% x 100
= 70 ml of water in the solution
Answer:
<h3>They contain member-bond organelles. </h3>
Explanation:
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Answer:
Here's where orbital hybridization came into play. According to this theory, when the carbon atom is in an excited state, one of the two electrons located in the 2s orbital will get promoted to the empty 2pz orbital. As a result, carbon now has 4 unpaired valence electrons with which it can form four bonds.
Explanation: