15:I[8216,["972","static/chunks/972-b28da0de92681928.js","47","static/chunks/47-a7f06e9eda1ac756.js","115","static/chunks/app/%5Bexam%5D/questions/%5Byear%5D/%5Bsubject%5D/%5Bchapter%5D/%5BquestionId%5D/page-7b6f0a12b9cc0206.js"],"BackButton"] 16:I[1553,["972","static/chunks/972-b28da0de92681928.js","47","static/chunks/47-a7f06e9eda1ac756.js","115","static/chunks/app/%5Bexam%5D/questions/%5Byear%5D/%5Bsubject%5D/%5Bchapter%5D/%5BquestionId%5D/page-7b6f0a12b9cc0206.js"],"QuestionViewer"] 17:T5bf,

To determine the number of moles of ions produced by complete dissociation of one mole of Mohr's salt in water, we first need to understand its chemical composition and how it dissociates.

Mohr's salt is a double salt with the chemical formula $$ \text{FeSO}_4 \cdot (\text{NH}_4)_2\text{SO}_4 \cdot 6\text{H}_2\text{O} $$. When it dissociates completely in water, it produces ions from each of its constituent compounds.

The dissociation can be represented as follows:

$$ \text{FeSO}_4 \cdot (\text{NH}_4)_2\text{SO}_4 \cdot 6\text{H}_2\text{O} \rightarrow \text{Fe}^{2+} + \text{SO}_4^{2-} + 2\text{NH}_4^{+} + \text{SO}_4^{2-} + 6\text{H}_2\text{O} $$

Let's break this down step by step:

1. One mole of $$ \text{FeSO}_4 $$ produces:

1 mole of $$ \text{Fe}^{2+} $$

1 mole of $$ \text{SO}_4^{2-} $$

2. One mole of $$ (\text{NH}_4)_2\text{SO}_4 $$ produces:

2 moles of $$ \text{NH}_4^{+} $$

1 mole of $$ \text{SO}_4^{2-} $$

Summing up all the ions produced, we get:

1 mole of $$ \text{Fe}^{2+} $$
2 moles of $$ \text{SO}_4^{2-} $$
2 moles of $$ \text{NH}_4^{+} $$

Therefore total number of moles of ions produced by complete dissociation of one mole of Mohr's salt are:

$$ 1 + 2 + 2 = 5 \text{ moles of ions} $$

Thus, the correct answer is:

Option C: 5

Ionic Equilibrum

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