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

Which of the following is the correct pH of a solution formed by mixing 1.3 L of 0.45 M HCl with 5.5 L of 1.95 M HI?

0.30

0.15

0.70

1.20

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Verified step by step guidance

Step 1: Calculate the moles of HCl in the solution. Use the formula \( \text{moles} = \text{volume} \times \text{molarity} \). For HCl, \( \text{moles of HCl} = 1.3 \text{ L} \times 0.45 \text{ M} \).

Step 2: Calculate the moles of HI in the solution using the same formula. For HI, \( \text{moles of HI} = 5.5 \text{ L} \times 1.95 \text{ M} \).

Step 3: Add the moles of HCl and HI together to find the total moles of hydrogen ions \( \text{H}^+ \) in the solution, since both HCl and HI are strong acids and dissociate completely.

Step 4: Calculate the total volume of the solution by adding the volumes of HCl and HI solutions: \( \text{total volume} = 1.3 \text{ L} + 5.5 \text{ L} \).

Step 5: Determine the concentration of \( \text{H}^+ \) ions in the solution by dividing the total moles of \( \text{H}^+ \) by the total volume of the solution. Then, calculate the pH using the formula \( \text{pH} = -\log[\text{H}^+] \).