Question

What are the products of each of the following acid-base reactions? Indicate the acid and its conjugate base and the base and its conjugate acid. (a) $\mathrm{HClO}_{4}+\mathrm{H}_{2} \mathrm{O} \rightarrow$ (b) $\mathrm{NH}_{4}^{+}+\mathrm{H}_{2} \mathrm{O} \rightarrow$ (c) $\mathrm{HCO}_{3}^{-}+\mathrm{OH}^{-} \rightarrow$

Name: Problem 4, Chapter 17: Chemistry and Chemical Reactivity
Uploaded: 2020-06-23T03:07:53-08:00
Duration: 3 min 39 s
Channel: Mina Mozafari
Description: What are the products of each of the following acid-base reactions? Indicate the acid and its conjugate base and the base and its conjugate acid. (a) HClO4+H2 O →(b) NH4^++H2 O →(c) HCO3^-+OH^- →

   What are the products of each of the following acid-base reactions? Indicate the acid and its conjugate base and the base and its conjugate acid.
(a) $\mathrm{HClO}_{4}+\mathrm{H}_{2} \mathrm{O} \rightarrow$
(b) $\mathrm{NH}_{4}^{+}+\mathrm{H}_{2} \mathrm{O} \rightarrow$
(c) $\mathrm{HCO}_{3}^{-}+\mathrm{OH}^{-} \rightarrow$

Chemistry and Chemical Reactivity

John C. Kotz, Paul… 8th Edition

Chapter 17, Problem 4

Instant Answer

Solved by Expert Mina Mozafari

06/23/2020

Step 1

The acid donates a proton (H+) to the base, forming their conjugate pairs. HClO4 (acid) → ClO4- (conjugate base) H2O (base) → H3O+ (conjugate acid) So the products are: ClO4- + H3O+ Show more…

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What are the products of each of the following acid-base reactions? Indicate the acid and its conjugate base and the base and its conjugate acid. (a) $\mathrm{HClO}_{4}+\mathrm{H}_{2} \mathrm{O} \rightarrow$ (b) $\mathrm{NH}_{4}^{+}+\mathrm{H}_{2} \mathrm{O} \rightarrow$ (c) $\mathrm{HCO}_{3}^{-}+\mathrm{OH}^{-} \rightarrow$

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Key Concepts

Brønsted–Lowry Acid-Base Theory

This theory defines acids as proton donors and bases as proton acceptors. It is fundamental in understanding acid–base reactions by focusing on the transfer of protons between reactants, thereby forming conjugate acid–base pairs.

Conjugate Acid-Base Pairs

In any acid–base reaction, when an acid donates a proton, it becomes its conjugate base, and when a base accepts a proton, it becomes its conjugate acid. This pairing is essential for balancing acid–base reactions and predicting the behavior and strength of the involved species.

Role of Water in Acid-Base Chemistry

Water is amphiprotic, meaning it can act as both an acid and a base. In acid–base reactions, water typically functions as a proton acceptor (base) or donor (acid), leading to the formation of hydronium (H3O+) or hydroxide (OH–) ions, respectively. This dual nature of water underlines its central role in many chemical reactions.

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