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Chapter 18: Problem 9

Identify the conjugate acid-base pairs in the following equation. \(\mathrm{HNO}_{2}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{NO}_{2}^{-}+\mathrm{H}_{3} 0^{+}\)

Short Answer

Expert verified
The conjugate acid-base pairs in the given equation are: 1. HNO鈧� (acid) and NO鈧傗伝 (conjugate base) 2. H鈧侽 (base) and H鈧僌鈦� (conjugate acid)

Step by step solution

01

Identify the Initial Acid and Base

The equation given is: \(\mathrm{HNO}_{2}+\mathrm{H}_{2}\mathrm{O} \rightleftharpoons \mathrm{NO}_{2}^{-}+\mathrm{H}_{3}\mathrm{O}^{+}\) Here, the HNO鈧� is donating an H+ to H鈧侽 (which accepts it). So, the initial acid is HNO鈧� and the initial base is H鈧侽.
02

Identify the Conjugate Acid and Base

After donating a proton, HNO鈧� now becomes a base (conjugate base). It forms NO鈧傗伝, which is without the H+ it initially had. So, the conjugate base to HNO鈧� is NO鈧傗伝. After accepting a proton from HNO鈧�, H鈧侽 becomes an acid (conjugate acid) and is now called H鈧僌鈦� (the extra proton added a positive charge). So, the conjugate acid to H鈧侽 is H鈧僌鈦�.
03

Write Down the Conjugate Acid-Base Pairs

We have found both the conjugate acid-base pairs, and they are as follows: 1. The conjugate acid-base pair of HNO鈧� (acid) is HNO鈧�/NO鈧傗伝 (conjugate base). 2. The conjugate acid-base pair of H鈧侽 (base) is H鈧侽/H鈧僌鈦� (conjugate acid).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Bronsted-Lowry Theory
The Bronsted-Lowry Theory is a fundamental part of understanding acid-base chemistry. According to this theory, an acid is a substance that donates a proton (H^+), and a base is a substance that accepts a proton. This is a broader definition compared to other theories, which offers more flexibility in classifying substances.

For example, in the reaction provided:
  • \(\text{HNO}_2\) is the acid because it donates a proton to \(\text{H}_2O\).
  • Water (\(\text{H}_2O\)) acts as a base because it accepts the proton from \(\text{HNO}_2\).
This exchange of protons is what defines their roles in the reaction. Understanding this principle helps to predict the behavior of different substances in aqueous solutions.
Acid-Base Reactions
Acid-base reactions are essential chemical reactions occurring all around us. These reactions involve the transfer of protons from acids to bases, forming conjugate acid-base pairs.

Let's break down the given equation:
  • The initial acid, \(\text{HNO}_2\), donates a proton, becoming \(\text{NO}_2^-\), its conjugate base.
  • The initial base, \(\text{H}_2O\), accepts a proton, transforming into \(\text{H}_3O^+\), its conjugate acid.
This interplay of donating and accepting protons leads to simultaneous formation of new acids and bases, highlighting the reversible nature of acid-base reactions. Knowing how to identify these pairs is crucial for understanding reaction dynamics and predicting outcomes.
Chemistry Education
Chemistry education focuses on making complex concepts like acid-base reactions accessible to students. By exploring real-world examples and interactive exercises, students deepen their understanding of underlying principles.

To engage with the topic better:
  • Visual aids, like molecular diagrams, can illustrate how acids and bases interact.
  • Practice problems enhance problem-solving skills by applying theoretical knowledge to practical scenarios.
  • Group discussions encourage diverse perspectives and collaborative learning.
Incorporating these methods ensures that students not only learn the mechanics of reactions but also appreciate their significance in chemical processes. This approach nurtures curiosity and paves the way for further exploration in chemistry.

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Most popular questions from this chapter

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Calculate the \(K_{\mathrm{a}}\) for the following acids using the given information. a. 0.220 \(\mathrm{M}\) solution of \(\mathrm{H}_{3} \mathrm{AsO}_{4}, \mathrm{pH}=1.50 \quad\) b. 0.0400 \(\mathrm{M}\) solution of \(\mathrm{HClO}_{2}, \mathrm{pH}=1.80\)

Solution A has a pH of 2.0. Solution B has a pH of 5.0. Which solution is more acidic? Based on the H't ion concentrations in the two solutions, how many times more acidic?
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