The concentration of sulphide ion in 0.01 M HCl solution saturated with hydrogen sulphide is `1.0xx10^(-19)`M. If 10 mL of this solution is added to 5 mL of 0.04 M solution of the following : `FeSO_4 , MnCl_2, ZnCl_2` and `CdCl_2`, in which of these solutions precipitation will take place ?
Given `K_(sp)`, values : `FeS=6.3xx10^(-18) , MnS=2.5xx10^(-13),ZnS=1.6xx10^(-24), CdS=8.0xx10^(-27)`

Explanation

To solve the problem, we need to determine whether precipitation will occur when the solution containing sulfide ions is mixed with the given metal salt solutions. We will calculate the ionic product (IP) for each metal sulfide and compare it with the given solubility product constant (Ksp) values.

### Step 1: Calculate the concentration of sulfide ions after mixing
We have a 10 mL solution of sulfide ions with a concentration of \(1.0 \times 10^{-19} \, M\) and we are mixing it with 5 mL of a 0.04 M metal salt solution. The total volume after mixing is:

\[ \text{Total Volume} = 10 \, \text{mL} + 5 \, \text{mL} = 15 \, \text{mL} \]
...