Acid/Base...Help!

[SunChip]

---

Members do not see this ad.

Need help with this question:

A solution is prepared in which a trace or small amount of Fe 2+ is added to a much larger amount of solution in which the [OH-] is 1.0 x 10^-2 M. Some Fe(OH)2 precipitates. The value of Ksp for Fe (OH)2 8.0 x 10 ^ -10.

Assuming that the hydroxide ion concentration is 1.0 x 10-2 M, calculate the concentration of Fe 2+ ions.

Thanks in advance!

 

[RogueUnicorn]

this isn't an acid base question, more of a solubility question

 

[Vanguard23]

I'm assuming none of them are solid or liquid?

Should be Ksp= [Products]/[Reactants]?

I was never that good with solubility.

 

[RogueUnicorn]

I'm assuming none of them are solid or liquid?

Should be Ksp= [Products]/[Reactants]?

I was never that good with solubility.

right-o. but if Fe(OH)2 precipitates out, you know it must then be a solid, like most salts. so really in this case, Ksp=[Fe][OH]^2. i think you can take it from here.