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

Molar mass of ascorbic acid=176.13 g/mol

Number of moles in a ascorbic acids tablet contain 546 mg =
`3.1* 10^(-3)`

Number of molecules in a tablet of ascorbic acid of mass 546 mg=
`1.867* 10^(21)` molecules

Step-by-step 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* 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=
`(Given mass )/(Molar mass)`

Number of moles of vitamin C=
`(546* 10^(-3))/(176.13)`

Number of moles of vitamin C=0.0031 moles=
`3.1* 10^(-3)`

Number of molecules of vitamin C=
`3.1* 10^(-3)* 6.022* 10^(23)`

Where Avogadro's number =
`6.022* 10^(23)`

Number of molecules of vitamin C=
`18.67*10^(20)`

=
`1.867* 10^(21)` molecules