Q.If the solubility product of $AgBr$ is $5 \times 10^{-13}$ , the concentration of $Ag^+$ required to just start precipitation of $AgBr$ from a $0.01 \text{ M } Br^-$ solution is:

5 \times 10^{-11} \text{ M}

5 \times 10^{-15} \text{ M}

2.5 \times 10^{-13} \text{ M}

1.0 \times 10^{-10} \text{ M}

The correct solution involves applying the fundamental concept to derive the final value step by step...

Already a member? Login here

Q.If the solubility product of AgBrAgBrAgBr is 5×10−135 \times 10^{-13}5×10−13, the concentration of Ag+Ag^+Ag+ required to just start precipitation of AgBrAgBrAgBr from a 0.01 M Br−0.01 \text{ M } Br^-0.01 M Br− solution is: