Answer:
The approximate ratio of isotopes in a naturally occurring sample of silver can be calculated by considering the natural abundances of silver-107 and silver-109.
The atomic weight of silver is the weighted average of the atomic masses of its isotopes, taking into account their natural abundances. Using the atomic masses of silver-107 and silver-109 (106.90509 u and 108.90476 u, respectively) and their natural abundances (51.84% and 48.16%, respectively), we can calculate the atomic weight of silver:
Atomic weight of silver = (106.90509 u x 0.5184) + (108.90476 u x 0.4816) = 107.8682 u
This means that a naturally occurring sample of silver contains a mixture of the two isotopes in the ratio of their natural abundances, which is approximately 107.8682:100 or about 1.08:1. Therefore, for every 1.08 atoms of silver-107, there would be 1 atom of silver-109 in a naturally occurring sample of silver.