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: Weak Acid-Strong Base

General Chemistry

18. Aqueous Equilibrium

Titrations: Weak Acid-Strong Base

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Multiple Choice

You are given a solution of HCOOH (formic acid) with an approximate concentration of 0.20 M and you will titrate this with a 0.1105 M NaOH. If you add 20.00 mL of HCOOH to the beaker before titrating, approximately what volume of NaOH will be required to reach the equivalence point?

40.00 mL

18.00 mL

36.20 mL

22.00 mL

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Verified step by step guidance

Start by understanding that at the equivalence point in a titration, the moles of acid will equal the moles of base. Here, formic acid (HCOOH) is being titrated with sodium hydroxide (NaOH).

Calculate the moles of HCOOH initially present in the solution. Use the formula: \( \text{moles} = \text{concentration} \times \text{volume} \). The concentration of HCOOH is 0.20 M and the volume is 20.00 mL (convert this to liters by dividing by 1000).

Next, determine the moles of NaOH required to reach the equivalence point. Since the reaction between HCOOH and NaOH is a 1:1 stoichiometry, the moles of NaOH needed will be equal to the moles of HCOOH calculated in the previous step.

Use the concentration of NaOH (0.1105 M) to find the volume of NaOH needed. Rearrange the formula \( \text{moles} = \text{concentration} \times \text{volume} \) to solve for volume: \( \text{volume} = \frac{\text{moles}}{\text{concentration}} \).

Convert the volume of NaOH from liters to milliliters by multiplying by 1000, as the final answer should be in milliliters.