Pick the stronger base from each pair. a. F – or Cl – b. NO 2 – or NO 3 –

Hey everyone, we're asked to identify the acid with the stronger conjugate base from the following pair, nitrous acid versus nitric acid. Now looking at nitrous acid, we know that this is a weak acid. Now, in comparison to nitric acid, we know that this is one of our strong acids. So thinking about their conjugate bases, all we need to do is go ahead and remove a proton. So removing a proton from our nitrous acid, we end up with our nitrite ion and removing a proton from our nitric acid. We end up with our nitrate ion. Now comparing the two, the stronger conjugate base is going to come from our nitrous acid. So that would be our nitrite. And the reason why is because since nitrous acid is a weaker acid in comparison to nitric acid, this must mean its conjugate base must be stronger than that of our nitric acid. Now, I hope that made sense. And let us know if you have any questions

Ch.16 - Acids and Bases

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Tro 4th Edition

Ch.16 - Acids and Bases

Problem 45a,b

Chapter 16, Problem 45a,b

Pick the stronger base from each pair. a. F^– or Cl^– b. NO₂^– or NO₃^–

Verified step by step guidance

Identify the periodic trend for halides: Fluoride (F^–) and Chloride (Cl^–) are both halide ions. In general, the basicity of halide ions decreases as you move down the group in the periodic table.

Compare the electronegativity: Fluoride is more electronegative than Chloride, which means it holds onto its electrons more tightly and is less willing to donate them, making it a weaker base.

Determine the conjugate acid strength: The strength of a base is inversely related to the strength of its conjugate acid. HF is a weaker acid than HCl, so F^– is a stronger base than Cl^–.

Analyze the resonance stabilization: For NO₂^– and NO₃^–, consider the resonance structures. NO₃^– has more resonance structures, which stabilizes the ion and makes it a weaker base.

Evaluate the conjugate acid strength for nitrites and nitrates: HNO₃ is a stronger acid than HNO₂, indicating that NO₂^– is a stronger base than NO₃^–.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Acid-Base Theory

Acid-base theory explains the behavior of acids and bases in chemical reactions. According to the Brønsted-Lowry theory, an acid is a proton donor, while a base is a proton acceptor. The strength of a base is determined by its ability to accept protons, which is influenced by the stability of the resulting conjugate acid.

Conjugate Acid-Base Pairs

Conjugate acid-base pairs consist of two species that differ by the presence of a proton. When a base accepts a proton, it forms its conjugate acid, and the strength of the base can be inferred from the stability of its conjugate acid. A weaker conjugate acid indicates a stronger base, as it is less likely to donate a proton back.

Electronegativity and Basicity

Electronegativity is the tendency of an atom to attract electrons in a bond. In the context of basicity, a more electronegative atom will hold onto its electrons more tightly, making it less likely to accept protons. Therefore, when comparing bases, the one with the less electronegative atom is typically the stronger base, as it can more readily accept protons.