Answer :
AgBr should precipitate first.
The concentration of
when CuBr just begins to precipitate is, 
Percent of
remains is, 0.0018 %
Explanation :
for CuBr is 
for AgBr is 
As we know that these two salts would both dissociate in the same way. So, we can say that as the Ksp value of AgBr has a smaller than CuBr then AgBr should precipitate first.
Now we have to calculate the concentration of bromide ion.
The solubility equilibrium reaction will be:

The expression for solubility constant for this reaction will be,
![K_{sp}=[Cu^+][Br^-]](https://tex.z-dn.net/?f=K_%7Bsp%7D%3D%5BCu%5E%2B%5D%5BBr%5E-%5D)
![4.2\times 10^{-8}=0.073\times [Br^-]](https://tex.z-dn.net/?f=4.2%5Ctimes%2010%5E%7B-8%7D%3D0.073%5Ctimes%20%5BBr%5E-%5D)
![[Br^-]=5.75\times 10^{-7}M](https://tex.z-dn.net/?f=%5BBr%5E-%5D%3D5.75%5Ctimes%2010%5E%7B-7%7DM)
Now we have to calculate the concentration of silver ion.
The solubility equilibrium reaction will be:

The expression for solubility constant for this reaction will be,
![K_{sp}=[Ag^+][Br^-]](https://tex.z-dn.net/?f=K_%7Bsp%7D%3D%5BAg%5E%2B%5D%5BBr%5E-%5D)
![7.7\times 10^{-13}=[Ag^+]\times 5.75\times 10^{-7}M](https://tex.z-dn.net/?f=7.7%5Ctimes%2010%5E%7B-13%7D%3D%5BAg%5E%2B%5D%5Ctimes%205.75%5Ctimes%2010%5E%7B-7%7DM)
![[Ag^+]=1.34\times 10^{-6}M](https://tex.z-dn.net/?f=%5BAg%5E%2B%5D%3D1.34%5Ctimes%2010%5E%7B-6%7DM)
Now we have to calculate the percent of
remains in solution at this point.
Percent of
remains = 
Percent of
remains = 0.0018 %