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Calculate the molar solubility of fe(oh)2 in pure water. (the value of ksp for fe(oh)2 is 4.87×10−17.)

Kaitlin Dean

in Chemistry

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Nicholas Rivera on January 6, 2019

When we have this equation balanced for the reaction:Fe(OH)2(s) ↔ Fe+2 + 2OH-when the Fe(OH)2 to give 1 mol of Fe+2 and 2 moles of OH-for what we can assume [Fe+2] = X and [OH-] = 2 X when Ksp = [Fe+2][OH-]^2-and have Ksp = 4.87x10^-17 [Fe+2]= X[OH-] = 2Xso by substitution 4.87x10^-17 = X*(2X)^2∴X^3 = 4.8x10^-17 / 4∴the solubility molar X = 2.3x10^-6 M


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