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.
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