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Zn salt is mixed with (NH4)2S of molarity 0.021 M. What amount of Zn+2 will remain unprecipitated in 12 mL of the solution ? KSP of ZnS is 4.5 × 10^-24
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Zn salt is mixed with (NH4)2S of molarity 0.021 M. What amount of Zn+2...

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Zn salt is mixed with (NH4)2S of molarity 0.021 M. What amount of Zn+2...
Given:
- Molarity of (NH4)2S = 0.021 M
- Volume of the solution = 12 mL
- Ksp of ZnS = 4.5 × 10^-24

To find:
- Amount of Zn^2+ that remains unprecipitated

Solution:

1. Write the balanced chemical equation:
ZnS(s) ⇌ Zn^2+(aq) + S^2-(aq)

2. Calculate the concentration of Zn^2+ and S^2- ions:
Since (NH4)2S is a strong electrolyte, it will dissociate completely.

- [S^2-] = [NH4)2S] = 0.021 M (from the given molarity)
- [Zn^2+] = [S^2-] (stoichiometry of the balanced equation)

3. Calculate the solubility of ZnS:
Ksp = [Zn^2+][S^2-]
4.5 × 10^-24 = [Zn^2+] × [S^2-]
4.5 × 10^-24 = ([S^2-])^2
4.5 × 10^-24 = (0.021)^2
[S^2-] = √(4.5 × 10^-24) = 6.71 × 10^-12 M

4. Calculate the amount of unprecipitated Zn^2+:
We have the concentration of Zn^2+ (which is equal to [S^2-]) and the volume of the solution.

Amount of Zn^2+ = [Zn^2+] × Volume of the solution
Amount of Zn^2+ = 6.71 × 10^-12 M × 12 mL

5. Convert the volume from mL to L:
1 mL = 0.001 L
Volume of the solution = 12 mL × 0.001 L/mL = 0.012 L

6. Calculate the amount of unprecipitated Zn^2+:
Amount of Zn^2+ = 6.71 × 10^-12 M × 0.012 L

7. Express the answer in scientific notation:
Amount of Zn^2+ = 8.052 × 10^-14 mol

8. Conclusion:
The amount of Zn^2+ that remains unprecipitated in 12 mL of the solution is 8.052 × 10^-14 mol.
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Zn salt is mixed with (NH4)2S of molarity 0.021 M. What amount of Zn+2 will remain unprecipitated in 12 mL of the solution ? KSP of ZnS is 4.5 × 10^-24
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