The concentration of suphide ion in `0.1 M HCl` solution saturated with hydrogen sulphide is `1.0xx10^(-19)M`. If `10 mL` of this is added to `5 mL` of `0.04 M` solution of the following: `FeSO_(4), MnCl_(2), ZnCl_(z)` and `CdCl_(2)`. In which of these solutions precipitation will take place?

Explanation

To determine in which of the given solutions precipitation will occur when 10 mL of a solution saturated with hydrogen sulfide is added to 5 mL of 0.04 M solutions of FeSO4, MnCl2, ZnCl2, and CdCl2, we will follow these steps:

### Step 1: Understand the Concept of Precipitation
Precipitation occurs when the ionic product (Qsp) of a solution exceeds the solubility product (Ksp) of the salt that could form. If Qsp > Ksp, precipitation will occur.

### Step 2: Calculate the Concentration of Sulfide Ion
The concentration of sulfide ion in the saturated solution is given as \(1.0 \times 10^{-19} \, M\).

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