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

Titrations: Strong Acid-Strong Base

General Chemistry

18. Aqueous Equilibrium

Titrations: Strong Acid-Strong Base

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Multiple Choice

In the titration of a 35.0 mL sample of 0.175 M HBr with 0.210 M KOH, what is the pH after adding 5.0 mL of base beyond the equivalence point?

2.85

7.00

11.00

12.15

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Verified step by step guidance

Determine the moles of HBr initially present using the formula: \( \text{moles of HBr} = \text{volume (L)} \times \text{molarity (M)} \).

Calculate the moles of KOH added at the equivalence point using the formula: \( \text{moles of KOH} = \text{volume (L)} \times \text{molarity (M)} \).

Find the moles of KOH added beyond the equivalence point by calculating the moles in the additional 5.0 mL of KOH.

Determine the excess moles of KOH by subtracting the initial moles of HBr from the total moles of KOH added.

Calculate the concentration of OH\(^-\) ions in the solution using the excess moles of KOH and the total volume of the solution, then find the pOH and convert it to pH using the relation: \( \text{pH} = 14 - \text{pOH} \).