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Ch.16 - Acid-Base Equilibria
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
All textbooksBrown 14th EditionCh.16 - Acid-Base EquilibriaProblem 15
Chapter 16, Problem 15

Give the conjugate base of the following Brønsted–Lowry acids: (i) HIO3, (ii) NH4+.

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1. A Brønsted-Lowry acid is a substance that donates a proton (H+) in a chemical reaction. The conjugate base of an acid is formed when the acid donates a proton. Therefore, to find the conjugate base of a Brønsted-Lowry acid, we simply need to remove a proton (H+) from the acid.
2. For HIO3, remove one H+ to get the conjugate base. The conjugate base of HIO3 is IO3-.
3. For NH4+, remove one H+ to get the conjugate base. The conjugate base of NH4+ is NH3.
4. Remember, the charge of the conjugate base will be one unit less than the charge of the acid, since a positively charged proton has been removed.
5. So, the conjugate bases of HIO3 and NH4+ are IO3- and NH3 respectively.

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Key Concepts

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

Brønsted–Lowry Acid-Base Theory

The Brønsted–Lowry theory defines acids as proton donors and bases as proton acceptors. This framework emphasizes the transfer of protons (H+) in chemical reactions, allowing for a broader understanding of acid-base behavior beyond just the presence of hydroxide ions. This theory is essential for identifying conjugate acid-base pairs.
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Bronsted-Lowry Acid-Base Theory

Conjugate Acid-Base Pairs

A conjugate base is formed when an acid donates a proton. In a conjugate acid-base pair, the acid and its conjugate base differ by one proton. Understanding this relationship is crucial for predicting the products of acid-base reactions and for identifying the conjugate base of a given acid.
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Conjugate Acid-Base Pairs

Dissociation of Acids

The dissociation of acids involves the release of protons into solution, which is a key step in determining their conjugate bases. For example, when HIO3 dissociates, it loses a proton to form IO3-, while NH4+ dissociates to form NH3. Recognizing how acids dissociate helps in identifying their corresponding conjugate bases.
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Acid-Base Dissociation Example
Related Practice
Textbook Question

Which of the following statements is false? (a) An Arrhenius base increases the concentration of OH- in water. (b) A Brønsted-Lowry base is a proton acceptor. (c) Water can act as a Brønsted–Lowry acid. (d) Water can act as a Brønsted–Lowry base. (e) Any compound that contains an –OH group acts as a Brønsted-Lowry base.

Textbook Question

Give the conjugate base of the following Brønsted–Lowry acids: (i) HCOOH, (ii) HPO42-.

Textbook Question

Identify the Brønsted–Lowry acid and the Brønsted–Lowry base on the left side of each of the following equations, and also identify the conjugate acid and conjugate base of each on the right side:

(a) NH4+(aq) + CN-(aq) ⇌ HCN(aq) + NH3(aq)

(b) (CH3)3N(aq) + H2O(l) ⇌ (CH3)3NH+(aq) + OH-(aq)

(c) HCOOH(aq) + PO43-(aq) ⇌ HCOO-(aq)+ HPO42-(aq)

Textbook Question

NH31g2 and HCl(g) react to form the ionic solid NH4Cl1s2. Which substance is the Brønsted–Lowry acid in this reaction? Which is the Brønsted–Lowry base?

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Textbook Question

Give the conjugate acid of the following Brønsted–Lowry bases: (i) SO42-, (ii) CH3NH2.