Chapter 11, Problem 11.1P

Interpretation Introduction

Interpretation:

The order of increasing acidity of the ions with reasons is to be stated.

Concept introduction:

The higher electro negativity of the species greater is the attraction. Therefore, increasing electro negativity of the atom that shares an electron pair will decrease basicity. Weaker bases have stronger conjugate acids; the electro negativity of an atom increases the acidity of the attached proton.

Answer to Problem 11.1P

The order of increasing acidity of the ions is $\left(\text{B}\right)<\left(\text{C}\right)\text{<}\left(\text{A}\right)\text{<}\left(\text{D}\right)$.

Explanation of Solution

The oxygen is the most electronegative species followed by sulphur and least electronegative is nitrogen. The given ions are shown below.

Figure 1

The most acidic ion is $\left(\text{D}\right)$ because of the presence of oxygen, the most electronegative has strong attraction and more acidic character. The next acidic ion is $\left(\text{A}\right)$. Since there are no protons for donation so least acidic ion is $\left(\text{B}\right)$. Therefore, the order is $\left(\text{B}\right)<\left(\text{C}\right)\text{<}\left(\text{A}\right)\text{<}\left(\text{D}\right)$.

Conclusion

The order of increasing acidity of the given ions is found to be as $\left(\text{B}\right)<\left(\text{C}\right)\text{<}\left(\text{A}\right)\text{<}\left(\text{D}\right)$.