What type of reaction is this? How do you balance it? Hg(OH)_2 + H_3PO_4 -> Hg(PO_4)_2 + H_2O

Jan 22, 2017

It's a neutralization reaction.

$3 H g {\left(O H\right)}_{\text{2" + 2 H_"3"PO_"4" -> Hg_"3"(PO_"4")_"2" + 6 H_"2}} O$

Explanation:

This is a neutralization reaction between a strong acid and a strong base.

First off, you missed a subscript of 3, in mercury (II) phosphate; should be $H {g}_{\text{3"(PO_"4")_"2}}$

To balance it, you have to consider the subscripts and use coefficients effectively, so there is an equal amount of elements on either side of the equal sign.

$3 H g {\left(O H\right)}_{\text{2" + 2 H_"3"PO_"4" -> Hg_"3"(PO_"4")_"2" + 6 H_"2}} O$

Hope this helps :)