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Vinil7 [7]
2 years ago
14

The solubility of gold (V) oxalate, Au2(C2O4)5 is 2.58 g/L. Calculate Ksp from this information.

Chemistry
1 answer:
makvit [3.9K]2 years ago
8 0

Answer:

Ksp=3.39x10^{-14}

Explanation:

Hello,

In this case, since the dissociation of gold (V) oxalate is:

Au_2(C_2O_4)_5(s)\rightleftharpoons 2Au^{5+}(aq)+5(C_2O_4)^{2-}(aq)

In such a way, the equilibrium expression is:

Ksp=[Au^{5+}]^2[(C_2O_4)^{2-}]^5

Thus, since the molar solubility of the gold (V) oxalate is computed by considering its molar mass (834 g/mol):

[Au_2(C_2O_4)_5]=2.58\frac{g}{L} *\frac{1mol}{834g} =3.09M

In such a way, since gold (V) is in a 2:1 molar ratio with the salt and the oxalate in a 5:1 in the chemical reaction, the corresponding concentrations at equilibrium are:

[Au^{5+}]=3.09x10^{-3}\frac{mol}{L} *\frac{2molAu^{5+}}{1mol} =6.19x10^{-3}M

[(C_2O_4)^{2-}]=3.09x10^{-3}\frac{mol}{L} *\frac{5mol(C_2O_4)^{2-}}{1mol} =0.0155M

Therefore, the solubility product turns out:

Ksp=(6.19x10^{-3})^2*(0.0155)^5\\\\Ksp=3.39x10^{-14}

Regards.

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