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Chapter 15: Problem 4

Write the formulas of the conjugate bases of the following acids: (a) \(\mathrm{HNO}_{2}\), (b) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (c) \(\mathrm{H}_{2} \mathrm{~S}\) (d) \(\mathrm{HCN}\), (e) HCOOH (formic acid).

Short Answer

Expert verified
The conjugate bases of the given acids are (a) \(NO_2^-\) (b) \(HSO_4^-\) (c) \(HS^-\) (d) \(CN^-\) (e) \(HCOO^-\).

Step by step solution

01

Conjugate base of \(HNO_2\)

Remove one hydrogen (H+) atom from the acid \(HNO_2\). The remaining molecule is the conjugate base of \(HNO_2\), thus it is \(NO_2^-\).
02

Conjugate base of \(H_2SO_4\)

Remove one hydrogen (H+) atom from the acid \(H_2SO_4\). The remaining molecule is the conjugate base of \(H_2SO_4\), thus it is \(HSO_4^-\). Remember, sulfuric acid is a diprotic acid and can lose two protons. The first loss results in the \(HSO_4^-\) ion.
03

Conjugate base of \(H_2S\)

Remove one hydrogen (H+) atom from the acid \(H_2S\). The remaining molecule is the conjugate base of \(H_2S\), thus it is \(HS^-\).
04

Conjugate base of \(HCN\)

Remove one hydrogen (H+) atom from the acid \(HCN\). The remaining molecule is the conjugate base of \(HCN\), thus it is \(CN^-\).
05

Conjugate base of \(HCOOH\)

Remove one hydrogen (H+) atom from the acid \(HCOOH\). The remaining molecule is the conjugate base of formic acid, thus it is \(HCOO^-\).

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Most popular questions from this chapter

Write the equation relating \(K_{\mathrm{a}}\) for a weak acid and \(K_{\mathrm{b}}\) for its conjugate base. Use \(\mathrm{NH}_{3}\) and its conjugate acid \(\mathrm{NH}_{4}^{+}\) to derive the relationship between \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\).

The three common chromium oxides are \(\mathrm{CrO}\), \(\mathrm{Cr}_{2} \mathrm{O}_{3},\) and \(\mathrm{CrO}_{3} .\) If \(\mathrm{Cr}_{2} \mathrm{O}_{3}\) is amphoteric, what can you say about the acid-base properties of \(\mathrm{CrO}\) and \(\mathrm{CrO}_{3} ?\)

HA and \(\mathrm{HB}\) are both weak acids although \(\mathrm{HB}\) is the stronger of the two. Will it take a larger volume of a \(\begin{array}{llll}0.10 & M & \text { NaOH } & \text { solution to } & \text { neutralize } & 50.0 & \text { mL }\end{array}\) of \(0.10 M\) HB than would be needed to neutralize \(50.0 \mathrm{~mL}\) of \(0.10 \mathrm{M}\) HA?

\(\mathrm{H}_{2} \mathrm{SO}_{4}\) is a strong acid, but \(\mathrm{HSO}_{4}^{-}\) is a weak acid. Account for the difference in strength of these two related species.

Calculate the \(\mathrm{pH}\) of a \(0.42 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}\) solution.
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