Kindly answer my query as early as possible.Please solve the complete question
A solution contains 0.01M Ag+ and 0.001M Ba+2 .
ksp of Ag2CrO4 = 2.4*10e-12
ksp of BaCrO4 = 1.17*10e-10
A solution of K2CrO4 is added to this solution.
Which will precipitate first,Silver chromate or barium Chromate?
What would be the concentration of the first metal ion to precipitate at the moment the other metal ion starts to precipitate?
What would be the concentration of the second metal ion so that both Silver chromate and barium Chromate precipitate simultaneously?
To determine which chromate will precipitate first when K2CrO4 is added to the solution, we need to compare the solubility products (Ksp) of Ag2CrO4 and BaCrO4.
1. Comparing Ksp values:
The Ksp value of Ag2CrO4 is 2.4 * 10^(-12), and the Ksp value of BaCrO4 is 1.17 * 10^(-10).
It's important to note that the lower the Ksp value, the less soluble the compound.
Since Ag2CrO4 has a lower Ksp value than BaCrO4, it means that Ag2CrO4 is less soluble and will precipitate first when K2CrO4 is added to the solution.
2. Concentration of the first metal ion to precipitate at the moment the other metal ion starts to precipitate:
To determine this concentration, we need to find the concentration at which the Ksp values for both Ag2CrO4 and BaCrO4 are equal.
- For Ag2CrO4: Ksp = [Ag+][CrO4^2-] = 2.4 * 10^(-12)
The concentration of Ag+ is initially 0.01 M.
Thus, [CrO4^2-] = Ksp / [Ag+] = (2.4 * 10^(-12)) / (0.01) = 2.4 * 10^(-10) M.
- For BaCrO4: Ksp = [Ba+2][CrO4^2-] = 1.17 * 10^(-10)
The concentration of Ba+2 is initially 0.001 M.
Thus, [CrO4^2-] = Ksp / [Ba+2] = (1.17 * 10^(-10)) / (0.001) = 1.17 * 10^(-7) M.
At the moment the other metal ion starts to precipitate, the concentration of the first metal ion (Ag+) is 2.4 * 10^(-10) M.
3. Concentration of the second metal ion for simultaneous precipitation of both chromates:
For both Ag2CrO4 and BaCrO4 to precipitate simultaneously, the concentration of CrO4^2- should be equal to or lower than the concentrations of both Ag+ and Ba+2.
Taking the lower concentration (Ag+) as a reference:
The concentration of Ag+ is initially 0.01 M.
Therefore, we need to adjust the concentration of CrO4^2- to be equal to or lower than 0.01 M.
Since the initial concentration of CrO4^2- is 0.001 M, which is lower than 0.01 M, there is no need to adjust the concentration.
Hence, the concentration of CrO4^2- should be maintained at 0.001 M for both Ag2CrO4 and BaCrO4 to precipitate simultaneously.
In summary:
- Silver chromate (Ag2CrO4) will precipitate first.
- The concentration of Ag+ at the moment Ba+2 starts to precipitate is 2.4 * 10^(-10) M.
- To precipitate both chromates simultaneously, the concentration of CrO4^2- should be 0.001 M.