Ch.17 - Acids and Bases

Problem 36c

Chapter 17, Problem 36c

Write the formula for the conjugate base of each acid. c. HI

Verified step by step guidance

Identify the acid in the problem: HI (hydroiodic acid).

Recall that a conjugate base is formed by removing a proton (H⁺) from the acid.

Remove one hydrogen ion (H⁺) from HI, which leaves you with the iodide ion (I⁻).

Write the formula for the conjugate base: I⁻.

Understand that the conjugate base of an acid is the species that remains after the acid has donated a proton.

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Key Concepts

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

Conjugate Acid-Base Pairs

In acid-base chemistry, a conjugate acid-base pair consists of two species that differ by the presence of a proton (H+). When an acid donates a proton, it forms its conjugate base, while the base that accepts the proton becomes its conjugate acid. Understanding this relationship is crucial for identifying the conjugate base of any given acid.

Strong Acids and Their Conjugate Bases

Strong acids, such as hydroiodic acid (HI), completely dissociate in water, meaning they release all their protons. The conjugate base of a strong acid is typically a weak base, which does not readily accept protons. Recognizing the strength of the acid helps predict the properties of its conjugate base.

Chemical Formulas and Ion Representation

Chemical formulas represent the composition of substances, including ions. The conjugate base of an acid can be represented by removing a hydrogen ion (H+) from the acid's formula. For HI, the removal of H+ results in the iodide ion (I-), which is the conjugate base of hydroiodic acid.

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