For the bases shown, draw the conjugate acid and identify a pK_a value from Table 4.5 that would help you accurately estimate its stability.
(e)

Verified step by step guidance

1. Identify the base in the problem. A base is a species that can accept a proton (H⁺). Look for lone pairs of electrons or negative charges that can act as proton acceptors.
2. Draw the conjugate acid of the base by adding a proton (H⁺) to the atom in the base that has the lone pair or negative charge. Ensure proper placement of the hydrogen atom and adjust the formal charges accordingly.
3. Refer to Table 4.5 (or a similar pKₐ table) to find the pKₐ value of the conjugate acid. The pKₐ value provides insight into the strength of the conjugate acid and, by extension, the stability of the base.
4. Use the pKₐ value to estimate the stability of the base. A higher pKₐ value for the conjugate acid indicates a weaker acid, which corresponds to a more stable base. Conversely, a lower pKₐ value indicates a stronger acid and a less stable base.
5. Compare the stability of the base with other bases if needed, using the pKₐ values of their conjugate acids as a reference. This will help you rank the bases in terms of stability or reactivity.

Key Concepts

Conjugate Acids and Bases

In acid-base chemistry, a conjugate acid is formed when a base accepts a proton (H⁺). Understanding this concept is crucial for predicting the behavior of substances in reactions. For example, when ammonia (NH₃) acts as a base, it can accept a proton to form its conjugate acid, ammonium (NH₄⁺). This relationship helps in determining the strength of acids and bases.

pKₐ and Acid Strength

The pKₐ value is a quantitative measure of the strength of an acid in solution; it is the negative logarithm of the acid dissociation constant (Kₐ). A lower pKₐ value indicates a stronger acid, which dissociates more completely in solution. This concept is essential for comparing the stability of conjugate acids and understanding their reactivity in chemical reactions.

Stability of Conjugate Acids

The stability of a conjugate acid is influenced by factors such as electronegativity, resonance, and inductive effects. A more stable conjugate acid will have a lower tendency to donate a proton, thus correlating with a stronger base. Evaluating the stability of conjugate acids helps in predicting the direction of acid-base reactions and the relative strengths of the corresponding bases.