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

Intro to Acid-Base Titration Curves

General Chemistry

18. Aqueous Equilibrium

Intro to Acid-Base Titration Curves

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Multiple Choice

Consider the titration of 60.0 mL of 0.200 M H₃PO₃ solution with 0.350 M potassium hydroxide, KOH solution. How many milliliters of base would be required to reach each of its equivalence points?

First:34.3 mL, Second:34.3 mL, Third:34.3 mL

First:34.3 mL, Second:68.6 mL, Third:102.9 mL

First:34.3 mL, Second:68.6 mL, Third:137.2 mL

First:105 mL, Second:210 mL, Third:315 mL

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Verified step by step guidance

Identify the chemical reaction involved in the titration. Phosphorous acid (H3PO3) is a diprotic acid, meaning it can donate two protons (H+ ions). The reaction with potassium hydroxide (KOH) can be represented as: H3PO3 + 2KOH → K2HPO3 + 2H2O.

Calculate the moles of H3PO3 present in the solution. Use the formula: moles = concentration (M) × volume (L). Convert the volume from mL to L by dividing by 1000.

Determine the stoichiometry of the reaction. Since H3PO3 is diprotic, it will react with KOH in a 1:2 ratio. This means that for every mole of H3PO3, two moles of KOH are required to reach the first equivalence point.

Calculate the volume of KOH needed to reach the first equivalence point. Use the formula: volume (L) = moles of KOH / concentration of KOH (M). Convert the volume from L to mL by multiplying by 1000.

For the second equivalence point, consider that the first equivalence point has been reached and additional KOH is needed to react with the remaining acidic hydrogen. Calculate the additional volume of KOH required using the same stoichiometry and method as before, and add it to the volume calculated for the first equivalence point.