Let’s consider the dissociation of phosphoric acid H3PO4. All four possible protonation states, with H number...

Let’s consider the dissociation of phosphoric acid H3PO4. All four possible protonation states, with H number from zero to three, must co-exist in equilibrium.

H3PO4 <-> H2PO4- <-> HPO42- <-> PO43-

pK1=2 pK2=7 pK3=12

Find relative populations of all four states at the pH of the human blood, ~7.4.

Expert Solution

queen_honey_blossom answered 2 years ago

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39. Phosphoric acid (H3PO4) is a triprotic weak acid. Calculate the pH, [H3PO4], [H2PO4 -], [HPO4 2-], and [PO4 3-] of a 4.5 M H3PO4 aqueous solution. H3PO4 (aq) + H2O (l) ⇌ H3PO4 - (aq) + H3O+ (aq) Ka1 = 7.5 × 10-3 H3PO4 - (aq) + H2O (l) ⇌ HPO4 2- (aq) + H3O+ (aq) Ka2 = 6.2 × 10-8 HPO4 2- (aq) + H2O (l) ⇌ PO4 3- (aq) + H3O+ (aq) Ka3 = 4.2 × 10-13

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