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Calculate the equilibrium constants of e...

Calculate the equilibrium constants of each of the indicated species necessary to reduce an initial `0.2M Zn^(2+)` solution to `1.0 xx 10^(-4)Zn^(2+)`.
`overset(Theta)OH` in equilibrium with `Zn(OH)_(2)(s)`.
Given.
`K_(sp)ZN(OH)_(2) = 1.8 xx 10^(-14)`.
`K_(f)Zn(OH)_(4)^(2-) = 5 xx 10^(14)`.

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To solve the problem, we need to calculate the concentration of hydroxide ions (OH⁻) required to reduce the concentration of zinc ions (Zn²⁺) from 0.2 M to 1.0 x 10⁻⁴ M, using the provided solubility product constant (Ksp) for Zn(OH)₂ and the formation constant (Kf) for Zn(OH)₄²⁻. ### Step-by-Step Solution: 1. **Write the Equilibrium Reaction**: The dissolution of zinc hydroxide can be represented as: \[ \text{Zn(OH)}_2(s) \rightleftharpoons \text{Zn}^{2+} + 2\text{OH}^- ...
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