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

A 16.4 mL aliquot of 0.182 M H3PO4 is to be titrated with 0.267 M NaOH. What volume (in mL) of the base will it take to reach the equivalence point?

37.4 mL

41.2 mL

24.8 mL

33.5 mL

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Verified step by step guidance

Identify the balanced chemical equation for the reaction: \( \text{H}_3\text{PO}_4 + 3\text{NaOH} \rightarrow \text{Na}_3\text{PO}_4 + 3\text{H}_2\text{O} \). This shows that one mole of \( \text{H}_3\text{PO}_4 \) reacts with three moles of \( \text{NaOH} \).

Calculate the moles of \( \text{H}_3\text{PO}_4 \) in the aliquot using the formula: \( \text{moles} = \text{concentration} \times \text{volume} \). Convert the volume from mL to L by dividing by 1000.

Determine the moles of \( \text{NaOH} \) required to reach the equivalence point. Since the stoichiometry of the reaction is 1:3, multiply the moles of \( \text{H}_3\text{PO}_4 \) by 3.

Calculate the volume of \( \text{NaOH} \) solution needed using the formula: \( \text{volume} = \frac{\text{moles}}{\text{concentration}} \). Ensure the concentration is in mol/L and convert the final volume from L to mL by multiplying by 1000.

Verify the calculation by checking the units and ensuring the stoichiometry of the reaction is correctly applied. Compare the calculated volume with the given options to find the correct answer.