A polyprotic acid possesses more than 2 hydronium ions (H+).
Our understanding of diprotic acids and bases can be used to understand polyprotic acids and bases.
Concept: The most common type of polyprotic acid is the triprotic acid, which contains 3 acidic hydronium ions.4m
Concept: Triprotic bases contain 3 Kb values, so they would have 3 equilibrium equations.5m
Concept: As a result of these equations for polyprotic acids and bases the relationship between Ka and Kb can be established.5m
Example: Determine the pH of 0.300 M sodium hydrogen phosphate, Na2HPO4. Phosphoric acid, H3PO4, contains Ka1 = 7.5 x 10-3, Ka2 = 6.2 x 10-8 and Ka3 = 4.2 x 10-13.6m
Example: Determine the pH of 0.300 M citric acid, H3C6H5O7 it possesses Ka1 = 7.4 x 10-4, Ka2 = 1.7 x 10-5 and Ka3 = 4.0 x 10-7.7m
Phosphorous acid dissociates to form dihydrogen phosphate and hydronium ion. Phosphorous acid has Ka of 5.0 x 10-2.
Write the equation dissociation for phosphorous acid. Express your answer as a chemical equation. Identify all of the phases in your answer.
What is the expression constant dissociation for phosphorous acid?
Phosphoric acid is a triprotic acid (Ka1 = 6.9 x 10^-3, Ka2 = 6.2x 10^-8, and Ka3 = 4.8 x10^-13). To find the pH of a buffer composed of H2PO4^- (aq) and HPO4^2- (aq), which pKa value would you use in the Henderson-Hasselbalch equation?
Calculate the pH of a buffer solution obtained by dissolving 13.0 g of KH2PO4(s) and 26.0 g of Na2HPO4(S) in water and then diluting to 1.00 L
Cysteine is an amino acid with R=-CH2SH, which ionizes according to:
The three Pka's of cysteine are: pKA'=1.71, pKA''=8.33, and pKA=10.78
If one prepares 0.40 M solution of cysteine and the pH is adjusted to pH=8.75, calculate the molar concentrations, [Cys] and [Cys-], in the resulting solution.
Identify the triprotic acid.
Farmers who raise cotton once used arsenic acid, H3AsO4 , as a defoliant at harvest time. Arsenic acid is a polyprotic acid with K1 = 2.5 x 10-4 , K 2 = 5.6 x 10-8 , and K3 = 3 x 10-13 . What is the pH of a 0.500 M solution of arsenic acid?
Consider a solution that is 0.10 M in a weak triprotic acid which is represented by the general formula H3A with ionization constants K1 = 1.0 × 10−3 , K2 = 1.0 × 10−8 , and K3 = 1.0 × 10−12. What is the pH of the solution?
Determine the pH of a 0.03 M solution of NaH 2PO4? Assume H3PO4 has a pKa1 of 2.1 and a pKa2 of 7.2 and a pKa3 of 12.7.
Identify the weak triprotic acid.
For the polyprotic acid H3PO4 (phosphoric acid), which of the following expressions would correspond to Ka3?
1. H3PO4 ⇌ PO43− + 3 H+
2. PO43− + 3 H+ ⇌ H3PO4
3. HPO42− ⇌ PO43− + H+
4. H2PO4− ⇌ HPO42− + H+
5. H3PO4 ⇌ H2PO4− + H+
Phosphoric acid (H3PO4) is characterized by three reactions for stepwise dissociation. Arrange the following species in the order of decreasing concentration in an aqueous solution of H3PO4. Clearly indicate the order of concentration change. JUSTIFY your answer.
H3PO4 H 2PO4- HPO 42- PO 43- H 3O+