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The acidic character of alcohols is due ...

 The acidic character of alcohols is due the polar nature of O-H bond. An e releasing group `(- CH_(3) -C_(2)H_(5))` increases e density on oxygen thus decreasing the acidity while e withdrawing group increases the acidity.
Which among the following is a better proton acceptor

A

`CH_(3)O^(-)`

B

`OH^(-)`

C

`SO_(4)^(2-)`

D

`NO_(3)^(-)`

Text Solution

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The correct Answer is:
To determine which among the given compounds is a better proton acceptor, we need to analyze the acidic and basic properties of each compound based on the information provided. ### Step-by-Step Solution: 1. **Understanding the Concept of Proton Acceptors**: - A proton acceptor is a species that can accept a proton (H⁺). This is often associated with the basicity of the species. The stronger the base, the better it is at accepting protons. 2. **Identifying the Compounds**: - The compounds mentioned are CH₃OH (methanol), OH⁻ (hydroxide ion), SO₄²⁻ (sulfate ion), and NO₃⁻ (nitrate ion). 3. **Analyzing the Acidity and Basicity**: - **CH₃OH (Methanol)**: It is a weak acid and can donate a proton to form CH₃O⁻ (methoxide ion). - **OH⁻ (Hydroxide Ion)**: This is a strong base and readily accepts protons to form water (H₂O). - **SO₄²⁻ (Sulfate Ion)**: This is a conjugate base of a strong acid (H₂SO₄) and is relatively stable, making it less likely to accept protons. - **NO₃⁻ (Nitrate Ion)**: This is also a conjugate base of a strong acid (HNO₃) and is similarly stable, thus less likely to accept protons. 4. **Comparing the Basicity**: - Between CH₃OH and OH⁻, OH⁻ is a stronger base than CH₃OH because it is more willing to accept protons. - Between SO₄²⁻ and NO₃⁻, both are stable conjugate bases of strong acids, making them less likely to accept protons. 5. **Conclusion**: - The best proton acceptor among the given options is **OH⁻ (hydroxide ion)** because it is a strong base and readily accepts protons to form water. ### Final Answer: **OH⁻ (hydroxide ion) is the better proton acceptor.** ---
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