Consider This Reaction: ${ HCO _3^{-} + H _2 S \rightarrow H _2 CO _3 + HS ^{-} }$Which Is The Bronsted-Lowry Base?A. { H _2 S $}$ B. { HCO _3^{-} $}$ C. { HS ^{-} $}$ D. { H _2 CO _3 $}$

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Introduction

In chemistry, the Bronsted-Lowry theory is a fundamental concept used to describe acid-base reactions. This theory defines an acid as a substance that donates a proton (H+ ion) and a base as a substance that accepts a proton. In this article, we will examine a specific chemical reaction and identify the Bronsted-Lowry base.

The Chemical Reaction

The given chemical reaction is:

HCO3−+H2S→H2CO3+HS−HCO _3^{-} + H _2 S \rightarrow H _2 CO _3 + HS ^{-}

In this reaction, we have two substances: HCO3−HCO _3^{-} (bicarbonate ion) and H2SH _2 S (hydrogen sulfide). The reaction produces two new substances: H2CO3H _2 CO _3 (carbonic acid) and HS−HS ^{-} (hydrogen sulfide ion).

Bronsted-Lowry Theory

According to the Bronsted-Lowry theory, a base is a substance that accepts a proton (H+ ion). In the given reaction, we need to identify which substance accepts a proton.

Analyzing the Reaction

Let's analyze the reaction step by step:

  1. HCO3−HCO _3^{-} (bicarbonate ion) donates a proton to form H2CO3H _2 CO _3 (carbonic acid).
  2. H2SH _2 S (hydrogen sulfide) accepts a proton to form HS−HS ^{-} (hydrogen sulfide ion).

From the above analysis, we can see that H2SH _2 S (hydrogen sulfide) accepts a proton to form HS−HS ^{-} (hydrogen sulfide ion). Therefore, H2SH _2 S is the Bronsted-Lowry base.

Conclusion

In conclusion, the Bronsted-Lowry base in the given chemical reaction is H2SH _2 S (hydrogen sulfide). This substance accepts a proton to form HS−HS ^{-} (hydrogen sulfide ion).

Key Takeaways

  • The Bronsted-Lowry theory defines a base as a substance that accepts a proton (H+ ion).
  • In the given chemical reaction, H2SH _2 S (hydrogen sulfide) accepts a proton to form HS−HS ^{-} (hydrogen sulfide ion).
  • Therefore, H2SH _2 S is the Bronsted-Lowry base in the given reaction.

Frequently Asked Questions

Q: What is the Bronsted-Lowry theory?

A: The Bronsted-Lowry theory is a fundamental concept in chemistry that defines an acid as a substance that donates a proton (H+ ion) and a base as a substance that accepts a proton.

Q: What is the Bronsted-Lowry base in the given chemical reaction?

A: The Bronsted-Lowry base in the given chemical reaction is H2SH _2 S (hydrogen sulfide).

Q: Why is H2SH _2 S the Bronsted-Lowry base?

A: H2SH _2 S is the Bronsted-Lowry base because it accepts a proton to form HS−HS ^{-} (hydrogen sulfide ion).

References

  • Bronsted, J.N. (1923). "The Theory of Acids and Bases". Journal of the American Chemical Society, 45(10), 2598-2611.
  • Lowry, T.M. (1923). "The Proton-Donor Theory of Acids and Bases". Journal of the American Chemical Society, 45(10), 2611-2624.

Additional Resources

  • Khan Academy: Bronsted-Lowry Theory
  • Chemistry LibreTexts: Bronsted-Lowry Theory
  • Wikipedia: Bronsted-Lowry Theory
    Bronsted-Lowry Theory Q&A =============================

Frequently Asked Questions

Q: What is the Bronsted-Lowry theory?

A: The Bronsted-Lowry theory is a fundamental concept in chemistry that defines an acid as a substance that donates a proton (H+ ion) and a base as a substance that accepts a proton.

Q: What is the difference between the Bronsted-Lowry theory and the Arrhenius theory?

A: The Arrhenius theory defines an acid as a substance that donates a hydrogen ion (H+) and a base as a substance that accepts a hydrogen ion. The Bronsted-Lowry theory is more comprehensive and defines an acid as a substance that donates a proton (H+ ion) and a base as a substance that accepts a proton.

Q: What is the Bronsted-Lowry base in the given chemical reaction?

A: The Bronsted-Lowry base in the given chemical reaction is H2SH _2 S (hydrogen sulfide).

Q: Why is H2SH _2 S the Bronsted-Lowry base?

A: H2SH _2 S is the Bronsted-Lowry base because it accepts a proton to form HS−HS ^{-} (hydrogen sulfide ion).

Q: What is the Bronsted-Lowry acid in the given chemical reaction?

A: The Bronsted-Lowry acid in the given chemical reaction is HCO3−HCO _3^{-} (bicarbonate ion).

Q: Why is HCO3−HCO _3^{-} the Bronsted-Lowry acid?

A: HCO3−HCO _3^{-} is the Bronsted-Lowry acid because it donates a proton to form H2CO3H _2 CO _3 (carbonic acid).

Q: What is the relationship between the Bronsted-Lowry theory and the Lewis theory?

A: The Lewis theory defines an acid as a substance that accepts a pair of electrons and a base as a substance that donates a pair of electrons. The Bronsted-Lowry theory is a subset of the Lewis theory, where the acid donates a proton (H+ ion) and the base accepts a proton.

Q: What are some common examples of Bronsted-Lowry acids and bases?

A: Some common examples of Bronsted-Lowry acids include:

  • Hydrochloric acid (HCl)
  • Sulfuric acid (H2SO4)
  • Nitric acid (HNO3)

Some common examples of Bronsted-Lowry bases include:

  • Sodium hydroxide (NaOH)
  • Potassium hydroxide (KOH)
  • Ammonia (NH3)

Q: How is the Bronsted-Lowry theory used in real-world applications?

A: The Bronsted-Lowry theory is used in a variety of real-world applications, including:

  • Water treatment: The Bronsted-Lowry theory is used to understand the behavior of acids and bases in water treatment processes.
  • Pharmaceutical industry: The Bronsted-Lowry theory is used to understand the behavior of acids and bases in pharmaceutical formulations.
  • Environmental science: The Bronsted-Lowry theory is used to understand the behavior of acids and bases in environmental systems.

Additional Resources

  • Khan Academy: Bronsted-Lowry Theory
  • Chemistry LibreTexts: Bronsted-Lowry Theory
  • Wikipedia: Bronsted-Lowry Theory

Glossary

  • Acid: A substance that donates a proton (H+ ion).
  • Base: A substance that accepts a proton (H+ ion).
  • Bronsted-Lowry theory: A fundamental concept in chemistry that defines an acid as a substance that donates a proton (H+ ion) and a base as a substance that accepts a proton.
  • Proton: A positively charged particle that is a component of an atom's nucleus.
  • Lewis theory: A fundamental concept in chemistry that defines an acid as a substance that accepts a pair of electrons and a base as a substance that donates a pair of electrons.