If the solubility products of $AgCl$ and $AgBr$ are $1.0 \times 10^{-10}$ and $3.5 \times 10^{-13}$ respectively,then the relation between the solubilities (denoted by the symbol $S$) of these salts can correctly be represented as:
- A$S$ of $AgBr$ is less than that of $AgCl$
- B$S$ of $AgBr$ is greater than that of $AgCl$
- C$S$ of $AgBr$ is equal to that of $AgCl$
- D$S$ of $AgBr$ is $10^6$ times greater than that of $AgCl$
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