Q42E - Chemistry (OpenStax)

Question

Explain how the diphosphate ion,  \({\left( {{O_3}P - O - P{O_3}} \right)^{4 - }}\)  can function as a water softener that prevents the precipitation of \(F{e^{2 + }}\) as an insoluble iron salt.

Step-by-Step Solution

Answer

Due to its structure, oxygen on one side can form bonds with water and on the other one with       \(F{e^{2 + }}\) as it is bonding with water, \(F{e^{2 + }}\) will remain insoluble.

Step 1 of 2: Lewis structure

The Lewis structure of the diphosphate ion is as follows

Step 2 of 2: Explanation

• As we could see that the negatively charged oxygen atoms on the both sides of the ion which can attract the positively charged \({\rm{F}}{{\rm{e}}^{2 + }}\)ion.
• The other side can form ion-dipole bond with water. 
• As the bonding with water is taking place, the \(F{e^{2 + }}\)will remain insoluble in the water.

Result

Due to its structure, oxygen on one side can form bonds with water and on the other one with \(F{e^{2 + }}\)as it is bonding with water, \(F{e^{2 + }}\)will remain insoluble.