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

Given that the concentration of [HX] in the reagent bottle is 1.0 M, the pH is 2.43, and the temperature is 22.1 degrees Celsius, with an equilibrium concentration of [HX] at 0.996 M and [X^-] at 4 x 10^-3 M, what is the equilibrium concentration of [H3O^+]?

1.0 x 10^-2 M

4.0 x 10^-3 M

2.5 x 10^-3 M

3.7 x 10^-3 M

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Verified step by step guidance

Start by understanding that the problem involves a weak acid HX dissociating in water to form H3O^+ and X^-. The equilibrium expression for this dissociation is: \( K_a = \frac{[H_3O^+][X^-]}{[HX]} \).

Given the equilibrium concentrations: [HX] = 0.996 M and [X^-] = 4 \times 10^{-3} M, we need to find the equilibrium concentration of [H3O^+].

Assume that the concentration of [H3O^+] at equilibrium is equal to the concentration of [X^-] because each molecule of HX that dissociates produces one H3O^+ and one X^-. Therefore, [H3O^+] = 4 \times 10^{-3} M.

Verify this assumption by calculating the pH from the given concentration of [H3O^+]. Use the formula: \( \text{pH} = -\log[H_3O^+] \). Substitute [H3O^+] = 4 \times 10^{-3} M into the equation to check if it matches the given pH of 2.43.

If the calculated pH matches the given pH, then the assumption is correct, and the equilibrium concentration of [H3O^+] is indeed 4 \times 10^{-3} M. If not, re-evaluate the assumptions or calculations.