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

pH of Weak Acids

General Chemistry

17. Acid and Base Equilibrium

pH of Weak Acids

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Multiple Choice

What is the ratio of HCO₃⁻ to H₂CO₃ in blood with a pH of 7.4?

20:1

5:1

1:1

10:1

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Verified step by step guidance

Understand that the problem involves the bicarbonate buffer system in blood, which consists of HCO₃⁻ (bicarbonate ion) and H₂CO₃ (carbonic acid). The Henderson-Hasselbalch equation is used to relate the pH to the ratio of these components.

Recall the Henderson-Hasselbalch equation:

pH = pK + log (\frac{{HCO}_{3}}{H_{2}})

. This equation will help us find the ratio of HCO₃⁻ to H₂CO₃.

Identify the pKₐ value for carbonic acid (H₂CO₃), which is approximately 6.1. This value is crucial for applying the Henderson-Hasselbalch equation.

Substitute the given pH value (7.4) and the pKₐ value (6.1) into the Henderson-Hasselbalch equation:

7.4 = 6.1 + log (\frac{{HCO}_{3}}{H_{2}})

. Solve for the log term to find the ratio.

Calculate the antilog of the result from the previous step to determine the ratio of HCO₃⁻ to H₂CO₃. This will give you the ratio that corresponds to the pH of 7.4.