Calculate the average atomic mass of hydrogen using the following data:

Isotope	% Natural abundance	Molar mass
${}^{1}H$	99.985	1
${}^{2}H$	0.015	2

Solution: For isotopes ${}^{1}H,$ % of natural abundance $=99.985$ Similarly, for isotopes ${}^{2}H,$ % of natural abundance $=0.015$

Formula used:
Here, A denotes Abundance
Average atomic mass =

(A(${}^{1}H$)


Average atomic mass = ( ($99.985\times 1$) + $(0.015\times 2))$ / (100)Average atomic mass = 1.00015 uHence, the average atomic mass of H comes out to be 1.00015 u

Hence, from the above solution it is concluded that the average atomic mass of H comes out to be 1.00015 u.