When we talk about acidity, the pH scale comes to mind. But there is another concept that is frequently employed by chemists and biochemists to compare the acidity or basicity of different molecules, and that is the pKa value. The pKa is defined as the negative logarithm of the acid dissociation constant (Ka) of a compound. In simpler terms, it reflects the tendency of a molecule to lose a proton (H+) when dissolved in water. The lower the pKa, the stronger the acid, that is, the more likely it is to donate its proton. The reason for this is that a low pKa indicates that the equilibrium between the protonated form and the deprotonated form of the acid lies far to the left, meaning that most of the time, the molecule will exist as protonated. Conversely, a high pKa indicates that the equilibrium lies far to the right, and that the molecule is more likely to remain in its deprotonated form. To put it simply, a higher negative pKa value denotes a less powerful acid.Please provide the negative pKa value of this molecule.