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A solution has 0.05M Mg^(2+) and 0.05M N...

A solution has `0.05M Mg^(2+)` and `0.05M NH_(3)`. Calculate the concentration of `NH_(4)CI` required to prevent the formation of `Mg(Oh)_(2)` in solution. `K_(SP)` for `Mg(OH)_(2)=9.0xx10^(-12)` and ionisation constant of `NH_(3)` is `1.8xx10^(-5)`.

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To solve the problem, we need to calculate the concentration of NH4Cl required to prevent the formation of Mg(OH)2 in a solution containing 0.05 M Mg²⁺ and 0.05 M NH3. We will use the Ksp of Mg(OH)2 and the ionization constant of NH3 to find the necessary concentration of NH4Cl. ### Step-by-Step Solution: 1. **Identify the Ksp Expression for Mg(OH)2**: The solubility product (Ksp) expression for Mg(OH)2 is given by: \[ K_{sp} = [Mg^{2+}][OH^-]^2 ...
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