The reaction of divalent manganese with oxygen in aqueous solutions is given as follows: Mn?* + 0.502(a9) + H2O → MnOz«) + 2H* It was found that a surface water sample devoid of oxygen, pH = 8.5, originally contained 0.6 mg/L of Mn²*. The sample was aerated (atmospheric conditions) and after 10 days of saturation with atmospheric oxygen the Mn2 concentration was 0.4 mg/L. (a) Assuming the pH remains constant during reaction, will the precipitate continue to form after the measurement on the tenth day? (b) What should the Mn²+ concentration be at equilibrium?

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The reaction of divalent manganese with oxygen in aqueous solutions is given as follows:
Mn?* + 0.502(a9) + H2O → MnOz«) + 2H*
It was found that a surface water sample devoid of oxygen, pH = 8.5, originally contained 0.6 mg/L of Mn²*.
The sample was aerated (atmospheric conditions) and after 10 days of saturation with atmospheric oxygen
the Mn2 concentration was 0.4 mg/L.
(a) Assuming the pH remains constant during reaction, will the precipitate continue to form after the
measurement on the tenth day?
(b) What should the Mn²+ concentration be at equilibrium?

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The reaction of divalent manganese with oxygen in aqueous solutions is given as follows: Mn?* + 0.502(a9) + H2O → MnOz«) + 2H* It was found that a surface water sample devoid of oxygen, pH = 8.5, originally contained 0.6 mg/L of Mn²*. The sample was aerated (atmospheric conditions) and after 10 days of saturation with atmospheric oxygen the Mn2 concentration was 0.4 mg/L. (a) Assuming the pH remains constant during reaction, will the precipitate continue to form after the measurement on the tenth day? (b) What should the Mn²+ concentration be at equilibrium?

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