17. Acid and Base Equilibrium

Diprotic Acid

Polyprotic Acids

Diprotic Acids

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.

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

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

CHEMISTRY 201:  Calculating the pH of a strong polyprotic acid

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

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

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.

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

Since a diprotic acid has two acidic hydrogens it would have 2 equilibrium equations.&#160;

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

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?

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

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.

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.
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/c40db6ef60e3c0ce-1672927367045.jpg" alt="" />
(a) <img src="" alt="" />
(b) <img src="" alt="" />
(c) <img src="" alt="" />
(d) <img src="" alt="" />

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 SO42- ions.

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

The diprotic bases would also have 2 equilibrium equations.&#160;

Diprotic acid sulfuric acid (H₂SO₄) pH problem

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.

Calculating the pH of a weak diprotic acid solution

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[BOOK CHEM] Clutch Version

Ionic Salts

Polyprotic Acid

A&#160;polyprotic acid&#160;possesses more than 2 hydronium ions (H+).&#160;

A diprotic acid&#160;is an acid that can donate two hydronium ions (H+).&#160;

Identifying Acids and Bases

Arrhenius Acid and Base

Bronsted Lowry Acid and Base

Lewis Acid and Base

Amphoteric

pH and pOH

Ka and Kb

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