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Chapter 17: Problem 3

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) \(\mathrm{HNO}_{3}+\mathrm{H}_{2} \mathrm{O} \rightarrow\) (b) \(\mathrm{HSO}_{4}^{-}+\mathrm{H}_{2} \mathrm{O} \rightarrow\) (c) \(\mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{F}^{-} \rightarrow\)

Short Answer

Expert verified
(a) Products: NO鈧冣伝, H鈧僌鈦�. (b) Products: SO鈧劼测伝, H鈧僌鈦�. (c) Products: H鈧侽, HF.

Step by step solution

01

Understand the Reaction Type

The given exercise involves identifying the products of acid-base reactions. In an acid-base reaction, an acid donates a proton ( H^+ ) to a base. The products are the conjugate base (from the acid) and the conjugate acid (from the base).
02

Solve Reaction (a)

For the reaction HNO_3 + H_2O \rightarrow: \(HNO_3\) (nitric acid) donates a proton to \(H_2O\). The conjugate base of \(HNO_3\) is \(NO_3^-\), and the conjugate acid formed is \(H_3O^+\). Therefore, the products are \(NO_3^-\) and \(H_3O^+\).
03

Solve Reaction (b)

For the reaction HSO_4^- + H_2O \rightarrow: \(HSO_4^-\) (bisulfate ion) can act as an acid and donate a proton to \(H_2O\). The conjugate base is \(SO_4^{2-}\), and the conjugate acid is \(H_3O^+\). Thus, the products are \(SO_4^{2-}\) and \(H_3O^+\).
04

Solve Reaction (c)

For the reaction H_3O^+ + F^- \rightarrow: \(H_3O^+\) (hydronium ion) acts as an acid and donates a proton to \(F^-\). The conjugate base of \(H_3O^+\) is \(H_2O\), and the conjugate acid formed is \(HF\). Therefore, the products are \(H_2O\) and \(HF\).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Conjugate Acid
When studying acid-base reactions, it is essential to understand the role of conjugate acids. A conjugate acid is formed when a base gains a proton (H鈦�). Think of it as a pair; wherever there is a base, if it accepts a proton, it transforms into its conjugate acid.
For example, in the reaction of the hydronium ion ( H_3O^+ ) with fluoride ion ( F^- ) , when ( F^- ) accepts a proton, it becomes hydrogen fluoride ( HF ) . Hence, ( HF ) serves as the conjugate acid to the base ( F^- ) .
In simpler terms:
  • A base gains a proton 鈫� Conjugate Acid is formed.
  • Example: ( F^- ) + ( H^+ ) 鈫� ( HF )
Conjugate Base
In an acid-base reaction, the conjugate base is what remains after an acid has donated a proton. This helps in understanding the idea of conjugate pairs, where acids and their conjugate bases balance each other in the chemical equation.
Let's delve into the example involving nitric acid ( HNO_3 ) reacting with water ( H_2O ) . When ( HNO_3 ) donates a proton, it becomes nitrate ion ( NO_3^- ) , acting as its conjugate base. Here鈥檚 a simple breakdown of the process:
  • An acid donates a proton 鈫� Results in a Conjugate Base.
  • Example: ( HNO_3 ) 鈫� ( NO_3^- ) + ( H^+ )
Understanding conjugate bases helps us track the flow of protons and predict the resulting products.
Proton Transfer
Proton transfer is the heart of acid-base reactions. It involves the movement of a proton (H鈦�) from the acid to the base. This key process is responsible for creating the products of such reactions: the conjugate bases and conjugate acids.
Consider the reaction between the bisulfate ion ( HSO_4^- ) and water ( H_2O ) . Here, ( HSO_4^- ) donates a proton to ( H_2O ) . This proton transfer transforms ( H_2O ) into hydronium ion ( H_3O^+ ) , and ( HSO_4^- ) into sulfate ion ( SO_4^{2-} ) .
  • Proton Transfer: The process of an acid donating and a base accepting a proton.
  • Key in determining reaction products: ( HSO_4^- ) + ( H_2O ) 鈫� ( SO_4^{2-} ) + ( H_3O^+ )
Understanding proton transfer is crucial for grasping how chemical reactions in this category operate.

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Most popular questions from this chapter

An aqueous solution has a pH of \(3.75 .\) What is the hydronium ion concentration of the solution? Is it acidic or basic?

If \(K_{\mathrm{a}}\) for a weak acid is \(2.4 \times 10^{-11},\) what is the value of \(\mathrm{p} K_{\mathrm{a}} ?\)

How can water be both a Bronsted base and a Lewis base? Can water be a Br枚nsted acid? A Lewis acid?

In each of the following acid-base reactions, identify the Bronsted acid and base on the left and their conjugate partners on the right. (a) \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{N}(\mathrm{aq})+\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}(\mathrm{aq}) \rightleftarrows\) \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NH}^{+}(\mathrm{aq})+\mathrm{CH}_{3} \mathrm{CO}_{2}^{-}(\mathrm{aq})\) (b) \(\mathrm{N}_{2} \mathrm{H}_{4}(\mathrm{aq})+\mathrm{HSO}_{4}^{-}(\mathrm{aq}) \rightleftarrows\) \(\mathrm{N}_{2} \mathrm{H}_{5}^{+}(\mathrm{aq})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})\) (c) \(\left[\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \rightleftarrows\) \(\left[\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{OH}\right]^{2+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)\)

The chromium(III) ion in water, \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+},\) is a weak acid with \(\mathrm{p} K_{\mathrm{a}}=3.95 .\) What is the value of \(K_{\mathrm{b}}\) for its conjugate base, \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{OH}\right]^{2+} ?\)
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