Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

17. Acid and Base Equilibrium

Acids Introduction

General Chemistry

17. Acid and Base Equilibrium

Acids Introduction

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Multiple Choice

Which of the following represents the correct equilibrium expression for the first dissociation of Malonic Acid (H2C3H2O4) in water?

Ka1 = [H2C3H2O4][H^+]/[HC3H2O4^-]

Ka1 = [HC3H2O4^-][H^+]/[H2C3H2O4]

Ka1 = [HC3H2O4^-]/[H2C3H2O4][H^+]

Ka1 = [H2C3H2O4]/[HC3H2O4^-][H^+]

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Verified step by step guidance

Understand the concept of acid dissociation: When an acid dissociates in water, it releases hydrogen ions (H^+) and forms its conjugate base. The equilibrium expression for this process is based on the concentrations of the products and reactants at equilibrium.

Identify the chemical species involved in the first dissociation of Malonic Acid (H2C3H2O4): The dissociation can be represented as H2C3H2O4 ⇌ HC3H2O4^- + H^+. Here, H2C3H2O4 is the acid, HC3H2O4^- is the conjugate base, and H^+ is the hydrogen ion.

Write the general form of the equilibrium expression for the dissociation: The equilibrium constant (Ka1) is expressed as the ratio of the product concentrations to the reactant concentration. For the dissociation of H2C3H2O4, it is Ka1 = [HC3H2O4^-][H^+]/[H2C3H2O4].

Compare the given options with the correct equilibrium expression: The correct expression should have the concentrations of the products (HC3H2O4^- and H^+) in the numerator and the concentration of the reactant (H2C3H2O4) in the denominator.

Select the correct option: Based on the comparison, the correct equilibrium expression for the first dissociation of Malonic Acid is Ka1 = [HC3H2O4^-][H^+]/[H2C3H2O4].