A solution contains 0.1 M NaCl, 0.01 M NaBr and 0.001 M Nal. Solid ${\text{AgNO}}_{\text{3}}$ is gradually added to the solution and its addition does not change the volume of solution :

 ${\text{K}}_{\text{sp}}\left(\text{AgCl}\right){\text{\hspace{0.17em}=\hspace{0.17em}10}}^{\text{-10}}{\text{,\hspace{0.17em}K}}_{\text{SP}}\left(\text{AgBr}\right){\text{\hspace{0.17em}=\hspace{0.17em}10}}^{\text{-13}}{\text{,\hspace{0.17em}K}}_{\text{SP}}\left(\text{Agl}\right){\text{\hspace{0.17em}=\hspace{0.17em}10}}^{\text{-17}}$   . Choose the correct statement.

When the precipitation of AgCl just starts, $\left[{\text{I}}^{-}\right]$ in the solution is  ${10}^{-8}$M

If sufficient Nal is added to a saturated solution of AgCl, precipitate of Agl is obtained 

Agl precipitates first 

The maximum  $\left[{\text{Ag}}^{\text{+}}\right]$ which can be maintained in the solution so that only Agl is precipitated

is  ${10}^{-11}\text{M}$