Ch.15 - Acid and Base EquilibriumWorksheetSee all chapters
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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
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Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

polyprotic acid possesses more than 2 hydronium ions (H+). 

Polyprotic Acids

Our understanding of diprotic acids and bases can be used to understand polyprotic acids and bases. 

Concept #1: The most common type of polyprotic acid is the triprotic acid, which contains 3 acidic hydronium ions. 

Concept #2: Triprotic bases contain 3 Kb values, so they would have 3 equilibrium equations. 

Concept #3: As a result of these equations for polyprotic acids and bases the relationship between Ka and Kb can be established. 

Example #1: 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

Example #2: 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

Additional Problems
Identify the triprotic acid. A) HNO3 B) H3PO4 C) H2CO3 D) HFO4 E) H2SO4
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.  1. 4.36 2. 7.11 3. 4.65 4. 7.40 5. 9.95 6. 1.81
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? 1. 2.15 2. 2.25  3. 2.02 4. 2.35 5. 2.54
In a triprotic acid, which Ka has the highest value? A) Ka1 B) Ka2 C) Ka3 D) Kb1 E) Kb2
Which below correctly describes the relationship amongst the successive p Ka and Kb values for most polyprotic acids?  a) pKa1 > pKa2 > pKa3 b) pKa3 > pKa2 > pKa1 c) Kb1 > Kb2 > Kb3 d) Ka1 < Kb1 e) cannot be predicted
In a triprotic acid which Ka value is largest in value? a) Ka1 b) Ka2 c) Ka3 d) They are all equal. 
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? A) 0.85 B) 1.95 C) 3.90 D) 4.51
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+ ⇌ H3PO43. HPO42− ⇌ PO43− + H+4. H2PO4− ⇌ HPO42− + H+5. H3PO4 ⇌ H2PO4− + H+ 
What is the pH of a solution of 0.25 M K3PO4, potassium phosphate? GivenKa1 = 7.5 * 10-3Ka2 = 6.2 * 10-8Ka3 = 4.2 * 10-13
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+  
Identify the weak triprotic acid.A) CH3COOHB) H3PO3C) H3PO4D) H2SO4E) H2SO3
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.
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
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?