17. Acid and Base Equilibrium

Diprotic Acids and Bases

17. Acid and Base Equilibrium

Diprotic Acids and Bases

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Ka values of Diprotic Acids

3 forms of Diprotic Acids

Diprotic Acids and Bases Example

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16.2 Binary Acids, Oxoacids, and Polyprotic Acids | General Chemistry

CHEMISTRY 201: Calculating the pH of a strong polyprotic acid

Calculating the pH of a weak diprotic acid solution

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Diprotic acid sulfuric acid (H₂SO₄) pH problem

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Diprotic acid sulfuric acid (H₂SO₄) pH problem

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Multiple Choice

Determine the equilibrium expression for the K_a2 of hydrosulfuric acid, H₂S?

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Textbook Question

State whether each of the following statements is true or false. Justify your answer in each case. (a) Sulfuric acid is a monoprotic acid.

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Textbook Question

State whether each of the following statements is true or false. Justify your answer in each case.

(c) Although sulfuric acid is a strong electrolyte, an aqueous solution of H₂SO₄ contains more HSO₄^- ions than SO₄^2- ions.

Which of the following pictures represents a solution of a weak diprotic acid, H2A? (Water molecules have been omitted for clarity.) Which pictures represent an impossible situation? Explain.

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Textbook Question

Calculate the pH of each of the following solutions (Ka and Kb values are given in Appendix D): (b) 0.100 M hydrogen chromate ion 1HCrO4-2

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Textbook Question

Rainwater is acidic because CO21g2 dissolves in the water, creating carbonic acid, H2CO3. If the rainwater is too acidic, it will react with limestone and seashells (which are principally made of calcium carbonate, CaCO3). Calculate the concentrations of carbonic acid, bicarbonate ion 1HCO3-2 and carbonate ion 1CO32 - 2 that are in a raindrop that has a pH of 5.60, assuming that the sum of all three species in the raindrop is 1.0 * 10-5 M.

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Textbook Question

The pH of a particular raindrop is 5.6. (b) What experiments could you do to test the hypothesis that the rain also contains sulfur-containing species that contribute to its pH? Assume you have a large sample of rain to test.

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Textbook Question

Write balanced net ionic equations and the corresponding equilibrium equations for the stepwise dissociation of the diprotic acid H2SeO4.

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Textbook Question

Calculate the pH and the concentrations of all species present (H2CO3, HCO3-, CO32-, H3O+ , and OH-) in 0.010 M H2CO3 1Ka1 = 4.3 * 10-7; Ka2 = 5.6 * 10-112.

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Textbook Question

Calculate the concentrations of H3O+ and SO4 2- in a solution prepared by mixing equal volumes of 0.2 M HCl and 0.6 M H2SO41Ka2 for H2SO4 is 1.2 * 10-22.

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Textbook Question

Write chemical equations and corresponding equilibrium expressions for each of the two ionization steps of carbonic acid.

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Textbook Question

Calculate the [H3O+] and pH of each polyprotic acid solution. b. 0.350 M H2C2O4

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Textbook Question

The following observations are made about a diprotic acid H2A: (i) A 0.10 M solution of H2A has pH = 3.30. (ii) A 0.10 M solution of the salt NaHA is acidic. Which of the following could be the value of pKa2 for H2A: (i) 3.22, (ii) 5.30, (iii) 7.47, or (iv) 9.82?

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Textbook Question

Calculate the concentration of all species in a 0.155 M solution of H2CO3.

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Textbook Question

What is the pH at 25 C of water saturated with CO2 at a partial pressure of 1.10 atm? The Henry's law constant for CO2 at 25 C is 3.1 * 10-2 mol>L@atm.

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Textbook Question

Atmospheric CO2 levels have risen by nearly 20% over the past 40 years from 320 ppm to 400 ppm. (a) Given that the average pH of clean, unpolluted rain today is 5.4, determine the pH of unpolluted rain 40 years ago. Assume that carbonic acid 1H2CO32 formed by the reaction of CO2 and water is the only factor influencing pH. CO21g2 + H2O1l2 Δ H2CO31aq2

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Open Question

Calculate the expected pH of a 0.050 M aqueous solution of maleic acid using K_a1.

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Open Question

What is the pH of a 0.200 M H₂S solution? K_a1 of H₂S = 8.9 × 10⁻⁸ and K_a2 = 1 × 10⁻¹⁹

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Open Question

What is the concentration of x2- in a 0.150

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17. Acid and Base Equilibrium

Diprotic Acids and Bases

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