Question

Ascorbic acid, or vitamin C (), is an essential vitamin. It cannot be stored by the body and must be present in the diet. What is the molar mass of ascorbic acid? Vitamin C tablets are taken as a dietary supplement. If a typical tablet contains 546.0 mg vitamin C, what amount (moles) and what number of molecules of vitamin C does it contain?

Answer 1

Answer:

Molar mass of ascorbic acid=176.13 g/mol

Number of moles in a  ascorbic acids tablet contain 546 mg =$3.1\times 10^{-3}$

Number of molecules in a tablet of ascorbic acid of mass 546 mg=$1.867\times 10^{21}$ molecules

Explanation:

We are given that ascorbic acid or vitamin C is an essential vitamin

We are given that given mass of ascorbic acid in a tablet =546.0 mg=$546\times 10^{-3}$

We have to find the number of moles and molecules of vitamin in C

We know that the chemical formula of ascorbic acid $C_6H_8O_6$

Molar mass of vitamin C =6(12.011)+8(1.0079)+6(16)=176.13 g/mol

Number of moles=$\frac{Given mass }{Molar mass}$

Number of moles of vitamin C=$\frac{546\times 10^{-3}}{176.13}$

Number of moles of vitamin C=0.0031 moles=$3.1\times 10^{-3}$

Number of molecules of vitamin C=$3.1\times 10^{-3}\times 6.022\times 10^{23}$

Where Avogadro's number =$6.022\times 10^{23}$

Number of molecules of vitamin C=$18.67\times10^{20}$

=$1.867\times 10^{21}$ molecules