A Student Performed A Titration Of $HF(aq)$ With $NaOH(aq)$. The Net Ionic Equation For The Neutralization Reaction That Occurs During The Titration Is Shown Above.(b) Identify Both Of The Brønsted-Lowry Conjugate Acid-base Pairs
Introduction
In chemistry, titration is a laboratory technique used to determine the concentration of a substance in a solution. It involves the reaction of a known concentration of one substance with an unknown concentration of another substance until the reaction is complete. In this experiment, a student performed a titration of hydrofluoric acid (HF) with sodium hydroxide (NaOH). The net ionic equation for the neutralization reaction that occurs during the titration is:
Understanding Brønsted-Lowry Acid-Base Theory
The Brønsted-Lowry theory of acid-base chemistry states that an acid is a substance that donates a proton (H+ ion), while a base is a substance that accepts a proton. In the context of the titration experiment, HF is the acid and NaOH is the base. However, the question asks for the identification of both Brønsted-Lowry conjugate acid-base pairs.
Identifying Conjugate Acid-Base Pairs
A conjugate acid-base pair is a pair of substances that differ by one proton. In the case of the titration experiment, the conjugate acid-base pairs can be identified as follows:
- HF is the conjugate acid of F-, as it has one more proton than F-.
- OH- is the conjugate base of H2O, as it has one less proton than H2O.
Explanation of Conjugate Acid-Base Pairs
In the context of the titration experiment, the conjugate acid-base pairs can be explained as follows:
- When HF donates a proton to OH-, it forms F- and H2O. In this process, HF acts as the acid and OH- acts as the base. The conjugate acid-base pair in this case is HF and F-.
- When OH- accepts a proton from H2O, it forms H2O and OH-. In this process, OH- acts as the base and H2O acts as the acid. The conjugate acid-base pair in this case is OH- and H2O.
Conclusion
In conclusion, the Brønsted-Lowry conjugate acid-base pairs in the titration experiment are HF and F-, and OH- and H2O. These pairs are identified by understanding the acid-base chemistry of the substances involved in the titration experiment.
Key Takeaways
- A conjugate acid-base pair is a pair of substances that differ by one proton.
- In the titration experiment, HF and F- are conjugate acid-base pairs, as well as OH- and H2O.
- Understanding Brønsted-Lowry acid-base theory is essential for identifying conjugate acid-base pairs.
Frequently Asked Questions
- Q: What is the difference between a conjugate acid-base pair and a neutralization reaction? A: A conjugate acid-base pair is a pair of substances that differ by one proton, while a neutralization reaction is a chemical reaction in which an acid and a base react to form a salt and water.
- Q: How do I identify conjugate acid-base pairs in a titration experiment? A: To identify conjugate acid-base pairs in a titration experiment, you need to understand the acid-base chemistry of the substances involved and identify the pairs of substances that differ by one proton.
Additional Resources
- For more information on Brønsted-Lowry acid-base theory, see [1].
- For more information on titration experiments, see [2].
References
[1] Brønsted, J. N., & Lowry, T. M. (1923). The theory of acids and bases. Journal of the American Chemical Society, 45(10), 2673-2684.
[2] Harris, D. C. (2016). Quantitative chemical analysis. W.H. Freeman and Company.
Glossary
- Acid: A substance that donates a proton (H+ ion).
- Base: A substance that accepts a proton (H+ ion).
- Conjugate acid-base pair: A pair of substances that differ by one proton.
- Neutralization reaction: A chemical reaction in which an acid and a base react to form a salt and water.
- Titration: A laboratory technique used to determine the concentration of a substance in a solution.
Introduction
In our previous article, we discussed the titration experiment performed by a student, where hydrofluoric acid (HF) was titrated with sodium hydroxide (NaOH). We also identified the Brønsted-Lowry conjugate acid-base pairs involved in the reaction. In this article, we will answer some frequently asked questions related to the titration experiment and Brønsted-Lowry acid-base theory.
Q&A
Q: What is the difference between a strong acid and a weak acid?
A: A strong acid is an acid that completely dissociates in water to produce hydrogen ions (H+), while a weak acid is an acid that only partially dissociates in water to produce hydrogen ions.
Q: What is the difference between a strong base and a weak base?
A: A strong base is a base that completely dissociates in water to produce hydroxide ions (OH-), while a weak base is a base that only partially dissociates in water to produce hydroxide ions.
Q: How do I determine the concentration of a substance in a solution using titration?
A: To determine the concentration of a substance in a solution using titration, you need to know the concentration of the titrant (the substance being added to the solution) and the volume of the solution. You can then use the volume of the titrant required to reach the endpoint of the reaction to calculate the concentration of the substance in the solution.
Q: What is the endpoint of a titration reaction?
A: The endpoint of a titration reaction is the point at which the reaction is complete, and the solution has reached a stable pH.
Q: How do I identify the conjugate acid-base pairs in a titration reaction?
A: To identify the conjugate acid-base pairs in a titration reaction, you need to understand the acid-base chemistry of the substances involved and identify the pairs of substances that differ by one proton.
Q: What is the difference between a Brønsted-Lowry acid and a Lewis acid?
A: A Brønsted-Lowry acid is a substance that donates a proton (H+ ion), while a Lewis acid is a substance that accepts a pair of electrons.
Q: How do I determine the pH of a solution using a pH indicator?
A: To determine the pH of a solution using a pH indicator, you need to add a small amount of the indicator to the solution and observe the color change. The pH of the solution can then be determined based on the color change.
Q: What is the significance of the pH scale in chemistry?
A: The pH scale is a measure of the concentration of hydrogen ions in a solution, with a pH of 7 being neutral and a pH below 7 being acidic and a pH above 7 being basic.
Conclusion
In conclusion, the titration experiment and Brønsted-Lowry acid-base theory are fundamental concepts in chemistry that are used to understand the behavior of acids and bases. By understanding these concepts, you can answer frequently asked questions related to titration and acid-base chemistry.
Key Takeaways
- A strong acid is an acid that completely dissociates in water to produce hydrogen ions (H+), while a weak acid is an acid that only partially dissociates in water to produce hydrogen ions.
- A strong base is a base that completely dissociates in water to produce hydroxide ions (OH-), while a weak base is a base that only partially dissociates in water to produce hydroxide ions.
- The endpoint of a titration reaction is the point at which the reaction is complete, and the solution has reached a stable pH.
- The conjugate acid-base pairs in a titration reaction can be identified by understanding the acid-base chemistry of the substances involved and identifying the pairs of substances that differ by one proton.
Frequently Asked Questions
- Q: What is the difference between a strong acid and a weak acid? A: A strong acid is an acid that completely dissociates in water to produce hydrogen ions (H+), while a weak acid is an acid that only partially dissociates in water to produce hydrogen ions.
- Q: What is the difference between a strong base and a weak base? A: A strong base is a base that completely dissociates in water to produce hydroxide ions (OH-), while a weak base is a base that only partially dissociates in water to produce hydroxide ions.
Additional Resources
- For more information on titration experiments, see [1].
- For more information on Brønsted-Lowry acid-base theory, see [2].
References
[1] Harris, D. C. (2016). Quantitative chemical analysis. W.H. Freeman and Company.
[2] Brønsted, J. N., & Lowry, T. M. (1923). The theory of acids and bases. Journal of the American Chemical Society, 45(10), 2673-2684.
Glossary
- Acid: A substance that donates a proton (H+ ion).
- Base: A substance that accepts a proton (H+ ion).
- Conjugate acid-base pair: A pair of substances that differ by one proton.
- Neutralization reaction: A chemical reaction in which an acid and a base react to form a salt and water.
- Titration: A laboratory technique used to determine the concentration of a substance in a solution.
- pH: A measure of the concentration of hydrogen ions in a solution, with a pH of 7 being neutral and a pH below 7 being acidic and a pH above 7 being basic.