Calculate the number of milliliters of 0.440 M KOH required to precipitate all of the Fe2+ ions in 187 mL of 0.692 M FeSO4 solution as Fe(OH)2. The equation for the reaction is: FeSO4(aq) + 2KOH(aq) Fe(OH)2(s) + K2SO4(aq)

588.2 mL

Explanation:

First we calculate how many Fe⁺² moles reacted, using the given concentration and volume of FeSO₄ solution (the number of FeSO₄ moles is equal to the number of Fe⁺² moles):

Then we convert Fe⁺² moles to KOH moles, using the stoichiometric ratios:

Finally we calculate the required volume of KOH solution, using the given concentration and the calculated moles:

the correct answer is:

a. formation of precipitation