A solution is prepared in which a trace or small amount of Fe2+ is added to a much larger amount of solution in which the [OH-] is 1.0x10^ -2M. Some Fe(OH)2 precipitates. The value of Ksp for Fe(OH)2=8.0x10^ -10.
1. Assuming that the hydroxide ion concentration is 1.0x10^ -2M, calculate the concentration of Fe2+ ions in the solution.
I've been trying to figure this out for days. If you could help me and show me how to work it out, that would be great.
Thanks in advance.
1. Assuming that the hydroxide ion concentration is 1.0x10^ -2M, calculate the concentration of Fe2+ ions in the solution.
I've been trying to figure this out for days. If you could help me and show me how to work it out, that would be great.
Thanks in advance.