General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343



General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343
Textbook Problem

Write the balanced chemical equation for the reaction of an aqueous oxacid that contains the phosphate anion with solid magnesium hydroxide. The reaction produces liquid dihydrogen monoxide and a solid ionic compound formed from the combination of magnesium cations and phosphate anions.

Interpretation Introduction


The balanced chemical equation for the given reaction has to be written.

Concept Introduction:

When a chemical reaction occurs, the total number of atoms in the reactant has to be same as that in the product formed.  Chemical reaction can be entered in form of chemical equation with all necessary conditions.  The chemical equation has to be balanced by adding coefficients only before the elements or compounds to make the atoms on both sides of arrow equal.  This is known as balanced chemical equation.


The product obtained is water and a compound that contains magnesium cations and phosphate anion.  The metal atom present in the compound is magnesium.  This is present in “2+” oxidation state.  There is phosphate group present in the compound.  Each phosphate anion carries “3-” charge.  To make the compound neutral, there has to be three magnesium cation and two phosphate anion.  The formula can be given as Mg3(PO4)2 .

Oxoacid that contains phosphate anion is phosphoric acid.  This reacts with magnesium hydroxide to form water and Mg3(PO4)2 .  The raw equation can be written as,

H3PO4 +Mg(OH)2H2O+ Mg3(PO4)2

First balance the magnesium atom.  This can be done by adding coefficient “3” to the magnesium hydroxide in the reactant side

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