Answer
$H_2SO_4(aq) + Mg(OH)_2(s) \longrightarrow 2H_2O(l) + MgSO_4(aq)$
Work Step by Step
1. Identify the type of Acid-Base reaction:
$Mg(OH)_2$ has the $OH^-$ ion, and it is reacting with an acid ($H_2SO_4$). Therefore, this is a reaction between an acid and an hydroxide.
$Acid + Hydroxide \longrightarrow H_2O(l) + Salt$
2. Find the identity of the salt.
The $H_2SO_4$ will donate its $H^+$ ions (since it is an acid). The "$SO_4^{2-}$" will remain in the solution.
The magnesium hydroxide ($Mg(OH)_2)$ will donate its $OH^-$ ions, leaving the magnesium ion ($Mg^{2+}$) alone.
Therefore, the produced salt is: $MgSO_4$.
3. Follow the pattern:
$H_2SO_4(aq) + Mg(OH)_2(s) \longrightarrow H_2O(l) + MgSO_4(aq)$
** Notice, the equation isn't balanced, there is a total of 4 hydrogens on the reactants side, and only 2 on the products side. To fix that, we shall put a 2 as the coefficient of $H_2O$:
$H_2SO_4(aq) + Mg(OH)_2(s) \longrightarrow 2H_2O(l) + MgSO_4(aq)$
Now, the equation is balanced.
