| Sections | |||
|---|---|---|---|
| Identifying Acids and Bases | 52 mins | 0 completed | Learn Summary |
| Arrhenius Acid and Base | 7 mins | 0 completed | Learn Summary |
| Bronsted Lowry Acid and Base | 18 mins | 0 completed | Learn Summary |
| Amphoteric | 6 mins | 0 completed | Learn |
| Lewis Acid and Base | 14 mins | 0 completed | Learn Summary |
| pH and pOH | 64 mins | 0 completed | Learn Summary |
| Ka and Kb | 21 mins | 0 completed | Learn |
| Ionic Salts | 46 mins | 0 completed | Learn |
| Diprotic Acid | 31 mins | 0 completed | Learn Summary |
| Polyprotic Acid | 24 mins | 0 completed | Learn |
| Additional Practice |
|---|
| Strong Acid-Base Calculations |
| Weak Acids |
| Additional Guides |
|---|
| Strong Acids and Strong Bases (IGNORE) |
| Conjugate Acids and Bases |
| Weak Bases |
A diprotic acid is an acid that can donate two hydronium ions (H+).
Diprotic Acids
Since a diprotic acid has two acidic hydrogens it would have 2 equilibrium equations.
The diprotic bases would also have 2 equilibrium equations.
Concept #3: As a result of these equations for diprotic acids and bases the relationship between Ka and Kb can be established.
Example #1: Sulfurous acid, H2SO3, represents a diprotic acid with a Ka1 = 1.6 x 10-2 and Ka2 = 4.6 x 10-5. Calculate the pH and concentrations of H2SO3, HSO3– and SO32– when given 0.250 M H2SO3.
Example #2: Determine the pH of 0.115 M Na2S. Hydrosulfuric acid, H2S, contains Ka1 = 1.0 x 10-7 and Ka2 = 9.1 x 10-8.
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Additional Problems
Identify the weak diprotic acid.
A) CH3COOH
B) HCOOH
C) H3PO4
D) H2SO4
E) H2CO3
What is the difference between (a) a monoprotic acid and a diprotic acid?
Explain the following observations: (c) although sulfuric acid is a strong electrolyte, an aqueous solution of H2SO4 contains more HSO4– ions than SO42– ions.
Identify the weak diprotic acid.A) CH3COOHB) HCOOHC) H3PO4D) H2SO4E) H2CO3
Calculate the concentration of H+ ions in a 0.010 M aqueous solution of sulfuric acid.Express your answer to three decimal places and include the appropriate units.
H2CO3 is a diprotic acid. The pKa for H2CO3 is 6.35 and the pKa for HCO3- = 10.33. At pH = 9.0, what is the approximate relative quantities of H2CO3, HCO3-, and CO32-?
a. 1 H2CO3, 10 HCO3-, and 1 CO32-
b. Negligible H2CO3, 95 HCO3-, and 5 CO32-
c. 1 H2CO3, 90 HCO3-, and 10 CO32-
d. Negligible H2CO3, 75 HCO3-, and 25 CO32-
For the diprotic weak acid H2A, Ka1 = 3.1 X 10-6 and Ka2 = 5.1 X 10-9. What is the pH of a 0.0500 M solution of H2A? What are the equilibrium concentrations of H2A and A2- in this solution?pH = ?H2A = ?A2- = ?
Calculate the equilibrium concentration of C2O42− in a 0.20 M solution of oxalic acid.Express your answer to two significant figures and include the appropriate units.
Which one of the following is a diprotic acid?a. sulfuric acidb. nitric acidc. barium hydroxided. chloric acid
Calculate the pH of a 0.080 M carbonic acid solution, H 2CO3(aq), that has the stepwise dissociation constants Ka1 = 4.3 × 10 -7 and Ka2 = 5.6 × 10 -11.A) 1.10B) 3.73C) 6.37D) 10.25
Complete the Ka2 expression for H2CO3 in an aqueous solution. Ka2 = 4.69 x 10-11