Question

How many moles of ions are released when 1.6 mol of ammonium phosphate, (NH4)3PO4, is dissolved in water?

Answer 1

Answer: 6.4 moles of ions

Explanation:

When ammonium phosphate, $(NH_4)_3PO_4$, is dissolved in water , it dissociates into ions.

$(NH_4)_3PO_4\rightarrow 3NH_4^++PO_4^{3-}$

According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.

1 mole of $(NH_4)_3PO_4$ gives 3 moles of $NH_4^+$ and 1 mole of $PO_4^{3-}$

1.6 moles of $(NH_4)_3PO_4$ gives $1.6\times3=4.8$ moles of NH_4^+[/tex] and $1.6\times 1 =1.6$ moles of $PO_4^{3-}$

Thus (1.6 + 4.8) = 6.4 moles of ions are released when 1.6 mol of ammonium phosphate, is dissolved in water.

Answer 2

The amount of substance present in an atom, molecule or compound is called moles. 6.4 moles of ions will be released when $\rm (NH_{4})_{3}PO_{4}$ is dissolved in water.

What is the law of conservation?

According to the law, the mass of the substance in a reaction cannot be formed or eliminated and the mass of the reactants on the left side should be equal to the mass of the products on the right side.

When $\rm (NH_{4})_{3}PO_{4}$ is dissolved in water then the ions formed are:

$\rm (NH_{4})_{3}PO_{4} \rightarrow 3NH_{4}^{+} + PO_{4}^{3-}$

From the reaction, it can be deduced that:

1 mole of ammonium phosphate = 3 moles of ammonium ion and 1 mole of phosphate ion.

1.6 moles of ammonium phosphate will give:

Moles of $\rm NH_{4}^{+}$:

$1.6 \times 3 = 4.8 \;\rm moles$

Moles of $\rm PO_{4}^{3-}$:

$1.6 \times 1 = 1.6 \rm \;moles$

Total moles of the product produced will be:

1.6 + 4.8 = 6.4 moles

Therefore, 6.4 moles of ions are released when ammonium phosphate, is dissolved in water.

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