**Comparing Acidic Strength in Compound Pairs**In evaluating the stronger acid from each pair of compounds, consider both structural features and electronic effects that influence acidity.**Pair (a):**- **Compound I**: Ethyl ammonium ion, depicted as \(\text{C}_2\text{H}_5\text{NH}_3^+\).- **Compound II**: Ethyl ammonium ion with an additional methyl group, depicted as \(\text{C}_2\text{H}_5\text{NH}_2^+\).In pair (a), we compare the acidity of two ammonium ions. The presence of an additional alkyl group can influence the electron-donating effect and potentially decrease acidity.**Pair (b):**- **Compound I**: Nitroanilinium ion, depicted as \(\text{O}_2\text{N}-\text{C}_6\text{H}_4-\text{NH}_3^+\).- **Compound II**: Methyl anilinium ion, depicted as \(\text{CH}_3-\text{C}_6\text{H}_4-\text{NH}_3^+\).In pair (b), the nitro group in Compound I is a strong electron-withdrawing group, which can enhance acidity by stabilizing the negative charge in the conjugate base more effectively than the methyl group in Compound II. **Conclusion**Analyzing the electronic effects, substituents that withdraw electrons tend to increase acidity by stabilizing the conjugate base, while electron-donating groups may decrease acidity.

(a). Acidic strength of compound increase with increasing negative inductive effect while decreases…

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Which compound in each of the following pairs is the stronger acid? + + (a) NH N. H2 I or II (b) O2N -NH3" H3C- -NH

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

**Comparing Acidic Strength in Compound Pairs**

In evaluating the stronger acid from each pair of compounds, consider both structural features and electronic effects that influence acidity.

**Pair (a):**

- **Compound I**: Ethyl ammonium ion, depicted as \(\text{C}_2\text{H}_5\text{NH}_3^+\).
- **Compound II**: Ethyl ammonium ion with an additional methyl group, depicted as \(\text{C}_2\text{H}_5\text{NH}_2^+\).

In pair (a), we compare the acidity of two ammonium ions. The presence of an additional alkyl group can influence the electron-donating effect and potentially decrease acidity.

**Pair (b):**

- **Compound I**: Nitroanilinium ion, depicted as \(\text{O}_2\text{N}-\text{C}_6\text{H}_4-\text{NH}_3^+\).
- **Compound II**: Methyl anilinium ion, depicted as \(\text{CH}_3-\text{C}_6\text{H}_4-\text{NH}_3^+\).

In pair (b), the nitro group in Compound I is a strong electron-withdrawing group, which can enhance acidity by stabilizing the negative charge in the conjugate base more effectively than the methyl group in Compound II.

**Conclusion**

Analyzing the electronic effects, substituents that withdraw electrons tend to increase acidity by stabilizing the conjugate base, while electron-donating groups may decrease acidity.

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