We can use the following equation:

$\overline{){\mathbf{Atomic}}{\mathbf{}}{\mathbf{Mass}}{\mathbf{=}}{{\mathbf{[}}{\mathbf{mass}}{\mathbf{\times}}{\mathbf{f}}{\mathbf{.}}{\mathbf{a}}{\mathbf{.}}{\mathbf{]}}}_{\mathbf{isotope}\mathbf{}\mathbf{1}}{\mathbf{+}}{{\mathbf{[}}{\mathbf{mass}}{\mathbf{\times}}{\mathbf{f}}{\mathbf{.}}{\mathbf{a}}{\mathbf{.}}{\mathbf{]}}}_{\mathbf{isotope}\mathbf{}\mathbf{2}}}$

To get ** f.a.**, we simply need to divide the given percent abundance by 100.

Naturally occurring silver consists of two isotopes: ^{107}Ag (51.84%) with an isotopic mass of 106.9051 amu and ^{109}Ag (48.16%) with an isotopic mass of 108.9048 amu.

What is the atomic weight of silver?

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