How many moles of fe (oh) 2 [ksp = 1.8 ' 10-15] will dissolve in 1.0 liter of water buffered at ph = 10.37?

Question

Darian Olson

Chemistry

21 September, 00:16

How many moles of fe (oh) 2 [ksp = 1.8 ' 10-15] will dissolve in 1.0 liter of water buffered at ph = 10.37?

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Answers (1)

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Ulises Rocha · Answer 1

When PH + POH = 14

∴ POH = 14 - 10.37 = 3.63

and when POH = - ㏒ [OH-]

3.63 = - ㏒ [OH-]

∴[OH-] = 2.34x10^-4 M

when Ksp = [Fe2+]*[OH-]^2

so by substitution:

1.8x10^-15 = [Fe2+] * (2.34x10^-4)

∴[Fe2+] = (1.8x10^-15) / (2.34 x 10^-4)

= 7.69 x 10^-12 moles of Fe (OH) 2