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

Answer 1

It's a neutralization reaction.

#3 Hg(OH)_"2" + 2 H_"3"PO_"4" -> Hg_"3"(PO_"4")_"2" + 6 H_"2"O#

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 #Hg_"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 Hg(OH)_"2" + 2 H_"3"PO_"4" -> Hg_"3"(PO_"4")_"2" + 6 H_"2"O#

Hope this helps :)

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Answer 2

Peyton Adams

This is a double displacement reaction. To balance it, use the coefficients: Hg(OH)_2 + 2 H_3PO_4 -> Hg(PO_4)_2 + 6 H_2O.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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

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