A solution is 0.1 M in each KCl, KBr and K2CrO4 to this solution, solid AgNO3 is gradually added. Assuming that there is no change in the volume of the solution given, The concentration (in M) of first ion when the second ion starts precipitating is about . Given: Ksp of AgCl = 1.7×10−10 Ksp of AgBr = 5.0×10−13 Ksp (K2CrO4)=1.9×10−12

A solution is 0.1 M in each KCl, KBr and K2CrO4 to this solution, so

1.	A solution is 0.1 M in each KCl, KBr and K2CrO4 to this solution, solid AgNO3 is gradually added. Assuming that there is no change in the volume of the solution given, The concentration (in M) of first ion when the second ion starts precipitating is about . Given: Ksp of AgCl = 1.7×10−10 Ksp of AgBr = 5.0×10−13 Ksp (K2CrO4)=1.9×10−12
Answer» A solution is 0.1 M in each $K C l$ , $K B r$ and $K _{2} C r O_{4}$ to this solution, solid $A g N O_{3}$ is gradually added. Assuming that there is no change in the volume of the solution given, The concentration (in M) of first ion when the second ion starts precipitating is about . Given: Ksp of $A g C l$ = $1.7 \times 10^{- 10}$ Ksp of $A g B r$ = $5.0 \times 10^{- 13}$ Ksp $(K_{2} C r O_{4}) = 1.9 \times 10^{- 12}$