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Chapter 16: Problem 15

(a) Give the conjugate base of the following Bronsted-Lowry acids: (i) \(\mathrm{HIO}_{3},(\mathbf{i} \mathbf{i}) \mathrm{NH}_{4}^{+} .(\mathbf{b})\) Give the conjugate acid of the following Bronsted-Lowry bases: (i) \(\mathrm{O}^{2-},(\mathbf{i} \mathbf{i}) \mathrm{H}_{2} \mathrm{PO}_{4}^{-}\)

Short Answer

Expert verified
The conjugate bases and acids of the given Bronsted-Lowry acids and bases are: (a) Conjugate bases: (i) HIO₃ ➞ IO₃⁻ (ii) NH₄⁺ ➞ NH₃ (b) Conjugate acids: (i) O²⁻ ➞ OH⁻ (ii) H₂PO₄⁻ ➞ H₃PO₄

Step by step solution

01

Identify the acid as HIO₃

The given Bronsted-Lowry acid is HIO₃.
02

Remove a proton from the acid

To find the conjugate base, we need to remove a proton (H⁺) from the given acid, which means we are left with IO₃⁻.
03

Write down the conjugate base

The conjugate base of HIO₃ is IO₃⁻. (ii) NH₄⁺
04

Identify the acid as NH₄⁺

The given Bronsted-Lowry acid is NH₄⁺.
05

Remove a proton from the acid

To find the conjugate base, we need to remove a proton (H⁺) from the given acid, which means we are left with NH₃.
06

Write down the conjugate base

The conjugate base of NH₄⁺ is NH₃. (b) Give the conjugate acid of the following Bronsted-Lowry bases: (i) O²⁻
07

Identify the base as O²⁻

The given Bronsted-Lowry base is O²⁻.
08

Add a proton to the base

To find the conjugate acid, we need to add a proton (H⁺) to the given base, which means we end up with OH⁻.
09

Write down the conjugate acid

The conjugate acid of O²⁻ is OH⁻. (ii) H₂PO₄⁻
10

Identify the base as H₂PO₄⁻

The given Bronsted-Lowry base is H₂PO₄⁻.
11

Add a proton to the base

To find the conjugate acid, we need to add a proton (H⁺) to the given base, which means we end up with H₃PO₄.
12

Write down the conjugate acid

The conjugate acid of H₂PO₄⁻ is H₃PO₄.

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Most popular questions from this chapter

An unknown salt is either NaF, NaCl, or NaOCl. When 0.050 mol of the salt is dissolved in water to form 0.500 L of solution, the pH of the solution is 8.08. What is the identity of the salt?

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Identify the Lewis acid and Lewis base in each of the following reactions: (a) \(\mathrm{HNO}_{2}(a q)+\mathrm{OH}^{-}(a q) \rightleftharpoons \mathrm{NO}_{2}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) (b) \(\mathrm{FeBr}_{3}(s)+\mathrm{Br}^{-}(a q) \rightleftharpoons \mathrm{FeBr}_{4}^{-}(a q)\) (c) \(\mathrm{Zn}^{2+}(a q)+4 \mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}^{2+}(a q)\) (d) \(\mathrm{SO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{2} \mathrm{O}_{3}(a q)\)
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