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Knowing K

_{s}=6⋅10^{−38 }for Fe(OH)_{3}in neutral solutions, calculate the minimum pH of an acidic solution in order to completely dissolve 10 mg of Fe(OH)_{3}. Data: Volume = 0.1 L.**I set out the equation for the equilibrium constant. having first calculated the concentration or iron ions (**

*9.35899*10*), and left the hydroxide concentration as an unknown:^{-4}M**K**

_{s}=*9.35899*10*^{-4}M * 27 C^{3}**Solving for**

Is this approach and solution correct?

*C*, I get*1.334*10*and so my guess is that the concentration of the hydronium ions must be the difference, as it has to neutralise the hydroxide ions in order to move the equilibrium towards the left. Doing this, I get^{-12}M,*9.35899*10*concentration for hydronium ions, which corresponds to pH = 3.03.^{-4}MIs this approach and solution correct?

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