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

18. Aqueous Equilibrium

Acid-Base Indicators

General Chemistry

18. Aqueous Equilibrium

Acid-Base Indicators

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Multiple Choice

A 60.0 mL solution of 0.115 M sodium hypochlorite (NaOCl) is titrated with 0.222 M NaOH. Calculate the pH of the solution after 6.05 mL of NaOH is added. The pKa of hypochlorous acid (HOCl) is 7.53.

8.00

10.00

7.53

9.00

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Verified step by step guidance

Determine the initial moles of sodium hypochlorite (NaOCl) in the solution using the formula: \( \text{moles} = \text{volume (L)} \times \text{molarity (M)} \). Convert 60.0 mL to liters and multiply by 0.115 M.

Calculate the moles of NaOH added using the formula: \( \text{moles} = \text{volume (L)} \times \text{molarity (M)} \). Convert 6.05 mL to liters and multiply by 0.222 M.

Determine the reaction between NaOCl and NaOH. NaOH will react with NaOCl to form hypochlorite ion (OCl\(^-\)) and water. Write the balanced chemical equation for this reaction.

Calculate the new concentrations of OCl\(^-\) and HOCl after the addition of NaOH. Use the initial moles of NaOCl and the moles of NaOH added to find the change in moles and adjust the concentrations accordingly.

Use the Henderson-Hasselbalch equation to calculate the pH of the solution: \( \text{pH} = \text{pKa} + \log \left( \frac{[\text{OCl}^-]}{[\text{HOCl}]} \right) \). Substitute the values for pKa, and the concentrations of OCl\(^-\) and HOCl to find the pH.