Textbook Question
Predict the stronger acid in each pair: (c) HBrO3 or HBrO2
Ch.16 - Acid-Base Equilibria
Chapter 16, Problem 89b
Based on their compositions and structures and on conjugate acid–base relationships, select the stronger base in each of the following pairs: (b) BrO- or BrO2-
Verified step by step guidance1
Identify the conjugate acids for each base: BrO^- and BrO_2^-.
Recall that the strength of a base is inversely related to the strength of its conjugate acid.
Determine the conjugate acids: HBrO for BrO^- and HBrO_2 for BrO_2^-.
Compare the acid strengths: HBrO is a weaker acid than HBrO_2 because it has fewer oxygen atoms, which means less electron-withdrawing effect.
Conclude that BrO^- is the stronger base because its conjugate acid (HBrO) is weaker than the conjugate acid of BrO_2^- (HBrO_2).
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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+). The strength of a base is often determined by its ability to accept protons, while the strength of an acid is determined by its ability to donate protons. Understanding these relationships helps in predicting which species will act as a stronger base in a given context.
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Conjugate Acid-Base Pairs
Oxidation States and Stability
The oxidation state of an element in a compound can influence its chemical behavior, including its acidity or basicity. In the case of bromine oxoanions like BrO- and BrO2-, the oxidation state of bromine affects the stability of the anions. Generally, higher oxidation states can lead to greater acidity, which inversely affects the basicity of the conjugate base.
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Electronegativity and Basicity
Electronegativity refers to the tendency of an atom to attract electrons in a bond. In the context of basicity, a more electronegative atom can stabilize negative charge better, which can influence the strength of a base. For the bromine oxoanions, the presence of additional oxygen atoms in BrO2- increases the electronegativity effect, making BrO- a stronger base due to less stabilization of the negative charge.
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Related Practice
Textbook Question
Predict the stronger acid in each pair: (e) benzoic acid (C6H5COOH) or phenol (C6H5OH).
Textbook Question
Based on their compositions and structures and on conjugate acid–base relationships, select the stronger base in each of the following pairs: (b) PO43- or AsO43-
Textbook Question
Indicate whether each of the following statements is true or false. For each statement that is false, correct the statement to make it true. (a) In general, the acidity of binary acids increases from left to right in a given row of the periodic table. (b) In a series of acids that have the same central atom, acid strength increases with the number of hydrogen atoms bonded to the central atom. (c) Hydrotelluric acid 1H2Te2 is a stronger acid than H2S because Te is more electronegative than S.
Textbook Question
Indicate whether each of the following statements is true or false. For each statement that is false, correct the statement to make it true. (a) Acid strength in a series of H¬A molecules increases with increasing size of A. (b) For acids of the same general structure but differing electronegativities of the central atoms, acid strength decreases with increasing electronegativity of the central atom. (c) The strongest acid known is HF because fluorine is the most electronegative element.