Table of contents

1. A Review of General Chemistry5h 5m
2. Molecular Representations1h 14m
3. Acids and Bases2h 46m
4. Alkanes and Cycloalkanes4h 17m
5. Chirality3h 39m
6. Thermodynamics and Kinetics1h 22m
7. Substitution Reactions1h 48m
8. Elimination Reactions2h 30m
9. Alkenes and Alkynes2h 9m
10. Addition Reactions3h 19m
11. Radical Reactions1h 58m
12. Alcohols, Ethers, Epoxides and Thiols2h 42m
13. Alcohols and Carbonyl Compounds2h 17m
14. Synthetic Techniques1h 26m
15. Analytical Techniques:IR, NMR, Mass Spect7h 3m
16. Conjugated Systems6h 13m
17. Ultraviolet Spectroscopy51m
18. Aromaticity2h 34m
19. Reactions of Aromatics: EAS and Beyond5h 1m
20. Phenols55m
21. Aldehydes and Ketones: Nucleophilic Addition4h 56m
22. Carboxylic Acid Derivatives: NAS2h 51m
23. The Chemistry of Thioesters, Phophate Ester and Phosphate Anhydrides1h 10m
24. Enolate Chemistry: Reactions at the Alpha-Carbon1h 53m
25. Condensation Chemistry2h 9m
26. Amines1h 43m
27. Heterocycles2h 0m
28. Carbohydrates5h 53m
29. Amino Acids4h 20m
30. Peptides and Proteins2h 42m
31. Catalysis in Organic Reactions1h 30m
32. Lipids 2h 50m
33. The Organic Chemistry of Metabolic Pathways2h 52m
34. Nucleic Acids1h 32m
35. Transition Metals6h 14m
36. Synthetic Polymers1h 49m

3. Acids and Bases

Equilibrium Constant

Organic Chemistry

3. Acids and Bases

Equilibrium Constant

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3:52 minutes

Problem 24b

Textbook Question

For the following acid–base reaction, (b) calculate the equilibrium constant.

Verified step by step guidance

Identify the acid and base on both sides of the reaction. Determine the conjugate acid and conjugate base formed after the reaction.

Look up the pKa values of the acid on the reactant side and the conjugate acid on the product side. These values are essential for calculating the equilibrium constant.

Use the relationship between the equilibrium constant (K_eq) and the pKa values: \( K_{eq} = 10^{\text{pKa (acid on product side)} - \text{pKa (acid on reactant side)}} \).

Substitute the pKa values into the equation. Ensure that the pKa values are correctly assigned to the respective acids.

Simplify the expression to calculate \( K_{eq} \). This will give you the equilibrium constant for the acid-base reaction.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In these reactions, acids donate protons while bases accept them. Understanding the nature of the acids and bases involved is crucial for predicting the direction of the reaction and calculating equilibrium constants.

Equilibrium Constant (K)

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction. It is calculated using the formula K = [products]/[reactants], where the concentrations are raised to the power of their coefficients in the balanced equation. A larger K value indicates a reaction that favors products, while a smaller K suggests a preference for reactants.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is disturbed, the system will adjust to counteract the disturbance and restore a new equilibrium. This principle is essential for understanding how changes in concentration, pressure, or temperature affect the position of equilibrium and, consequently, the value of the equilibrium constant.

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Related Practice

Textbook Question

For the following acid–base pairs, (iii) predict the favored side of equilibrium; (iv) calculate ;

(f)

Textbook Question

Calculate K_eq for these acid–base reactions.

(c)

Textbook Question

Given that the indicated pK_a values correspond to the acid dissociation reactions shown, calculate the ratio of acid to conjugate base for the reactions shown.

(b)

Textbook Question

Hydrogen gas (H₂) has a relatively high pK_a value. Is it a stable or unstable acid? Do you expect it to participate in acid–base reactions?

Textbook Question

For each of the following acid–base reactions, (ii) calculate K_eq. If a pK_a is not one of the ten common ones we learned in Chapter 4, it will be given to you.

(a)

Textbook Question

Estimate the K_eq for the following reactions based on the stability of the anions involved.

(c)

Textbook Question

Estimate the K_eq for the following reactions based on the stability of the anions involved.

(b)

Textbook Question

Using pKₐ values, calculate K_eq for the following acid–base reaction.

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