After i solve for x, i can find the moles of Mg+2 added, would it be equal to the moles of Mg(OH)2?

How can it be different? This is just a simple stoichiometry that you need to follow.

I will elaborate again what's confusing me, sorry if i sound a bit dense in general chem.

A + B <-------> 2C

If you have 2 molar of C in an equilibrium, would it mean you have 1 molar of A? usually no in many problems that I have done.

i.e

A + B <--------> 2C

2M 2M 0

-x -x +2x

2-x 2-x 2x

2-x doesn't equal 2x in a usual equilbrium problem.

Back to my problem.

I understand that the OH reacts with H+ not in equilbrium and it's 1:1, but I have some magnesium ions left at the end, but it's equilbrium equation

Mg(OH)2 <-----> Mg+2 + 2OH-

Let's say I have 10 moles left of Mg+2, why should the Mg(OH)2 be 10 moles, still it's still an equilbrium like the example of (a/b/c) above?

Am i having a brain attack ? why is this different?

honestly if it was Mg(OH)2 -----> Mg+2 + 2OH-

i would have no problem