Chemistry Equilibrium of a Sparingly Soluble Ionic Compound

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The discussion centers on calculating the highest concentration of OH- in a sparingly soluble ionic compound without causing precipitation, with a focus on achieving an accurate result. The initial answer provided is 6.61g, but discrepancies arise due to rounding errors in the concentration of OH-. Maintaining precision in intermediate calculations is emphasized, specifically not rounding [OH-] too early. Participants suggest keeping extra digits throughout the calculation and only rounding at the final step to ensure accuracy. The conversation highlights the importance of precision in chemical calculations to avoid errors in results.
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Homework Statement
I can't get the correct answer, isn't it if Ksp>[Mn2+][OH-]^2, there is no precipitation. How to get the specific concentration of [OH-]?
Relevant Equations
Kb = [NH4+][OH-]/[NH3]
Ksp=[Mn2+][OH-]^2
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Answer given is 6.61g.
 
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You are looking for the highest concentration of OH- that doesn't produce precipitation, don't you?
 
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May I know which step is wrong? thanks
 
You have worked out the concentration in g/L. What is the mass in the actual solution?
 
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Is this correct ? thanks.
 
It is not quite equal to the given answer; I think that's because you rounded off [OH-] to 1.4e-6 M instead of 1.435e-6 M. Keep the extra digits through the calculation, and round off to the appropriate sig figs at the end.
 

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