Carbon exists in nature as three isotopes. given the atomic masses and relative abundance of the isotopes, what is the average atomic mass of carbon? a. 12.000 amu b.12.011 amu c.13.002 amu d.13.003 amu e.14.003 amu

Answer : The correct option is, (B) 12.011 amu

Explanation :

Average atomic mass of an element is defined as the sum of masses of each isotope each multiplied by their natural fractional abundance.

Formula used to calculate average atomic mass follows:

We are assuming that:

Mass of isotope C-12 = 12.000 amu

% abundance of isotope C-12= 98.93% = 0.9893

Mass of isotope C-13 = 13.003 amu

% abundance of isotope C-13 = 1.07% = 0.0107

Mass of isotope C-14= 14.003 amu

% abundance of isotope C-14 = 0.0000000001% =  0.000000000001 =

In this case, the abundance of C-14 is very low. So, their influence is negligible.

Now put all the given values in the above formula, we get:

Therefore, the average atomic mass of carbon is, 12.011 amu

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.

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