The constant number (Ka value) for the acidification of phosphoric acid is an important parameter in chemistry for measuring the acidity of phosphoric acid. Phosphoric acid can dissociate in water and solution, and the Ka value indicates the degree of dissociation and reaction.

When phosphoric acid is dissolved in water, there is the following dissociation, solution equilibrium: phosphoric acid (H < PO >) can be dissociated in steps, dissociated, dissociated, first step, dissociated, and dissociated as: H < PO > < H > + H < PO >, its acid, solution constant, is Ka <. At this time, the size of the Kavalue reflects the difficulty and degree of phosphoric acid first, step, dissociation, and release of protons (H 🥰). If the Kavalue is large, then it indicates that phosphoric acid is easier to occur, and the first step, dissociation, dissociation, dissociation, is relatively acidic and strong; if the Kavalue is small, then the first step, dissociation, dissociation, dissolution, is more difficult, and the acidity is relatively weak.

Secondly, H 2O PO can be further dissociated: H 2O PO H 🥰 + HPO ², this step, dissociation, dissociation, acid dissociation, constant number, is Ka ². Similarly, the Ka ² value affects the degree of dissociation. Usually, for multi-component acids, Ka > Ka < unk > Ka < unk >, because with the proton's step-by-step release, with negative charge, acid radical, ion, the attraction to the proton gradually increases, making the subsequent dissociation and solution more and more difficult. At the end of

, the step dissociation is: HPO ² H 🥰 + PO ³, acid, the solution constant is Ka 🥰. Phosphoric acid, among other things, Ka values at all levels are crucial for the study of the chemistry, reaction, acid-base neutralization, and related chemical equilibrium in which phosphoric acid is involved.