Chemistry Forum

A chemist dissolves 37.0 g of magnesium hydroxide in
one beaker of water, and 24.0 g of iron(III) bromide in a
second beaker of water. Everything dissolves.
When the two solutions are poured together, solid
iron(III) hydroxide precipitates.
a) Write a balanced molecular equation.
b) Determine the identity of the limiting reactant.
c) Predict the mass of iron(III) hydroxide product.


I try to solve the molecular equation but i don’t know where Mg or Br go to

Magnesium hydroxide has very poor soloubility, only 9mg/l. So what is described is not possible.

But generally, what are the formula of both components.

Develop the correct equation and combine them that you get the product.

For the limiting reactant calculate the moles of each and combine with the theoretically value.

Thank you very much for your help I am now able to do the parts to this problem. Sorry if English is bad. Have a good day

Post your result.