Answer
The balanced equation for that neutralization reaction is:
$3 HCl(aq) + Fe(OH)_3(s) \longrightarrow 3H_2O(l) + FeCl_3(aq)$
Work Step by Step
1. Identify the type of Acid-Base reaction:
$Fe(OH)_3$ has the $OH^-$ ion, and it is reacting with an acid ($HCl$). 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 $HCl$ will donate a $H^+$ ion (since it is an acid). The "$Cl^{-}$" will remain alone.
The iron(III) hydroxide ($Fe(OH)_3$) will donate $OH^-$ ions, leaving the iron(III) ion ($Fe^{3+}$) alone.
Therefore, the produced salt is a mixture of $Fe^{3+}$ and $Cl^{-}$. To balance the charge, 3 $HCl$ should react with a $Fe(OH)_3$ to produce $FeCl_3$.
3. Follow the pattern:
$3 HCl(aq) + Fe(OH)_3(s) \longrightarrow H_2O(l) + FeCl_3(aq)$
** The equation isn't balanced, there is a total of 6 hydrogens on the reactants side, and only 2 on the products side. To fix that, we shall put a 3 as the coefficient of $H_2O$:
$3 HCl(aq) + Fe(OH)_3(s) \longrightarrow 3H_2O(l) + FeCl_3(aq)$
Now, the equation is balanced.
