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Chapter 13: Problem 5

Give the formula of the conjugate acid of (a) \(\mathrm{OH}^{-}\) (b) \(\mathrm{HPO}_{4}{ }^{2-}\) (c) \(\mathrm{NH}_{3}\) (d) \(\mathrm{F}^{-}\) (e) \(\mathrm{Zn}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}(\mathrm{OH})_{2}\)

Short Answer

Expert verified
(a) OH- (b) HPO42- (c) NH3 (d) F- (e) Zn(H2O)2(OH)2 Answer: (a) H2O (b) H2PO4- (c) NH4+ (d) HF (e) Zn(H2O)2(OH)(H2O)+

Step by step solution

01

(a) Conjugate acid of OH-

To find the conjugate acid of \(\mathrm{OH}^{-}\), we add a proton (H+) to the species: \(\mathrm{OH}^{-} + \mathrm{H}^{+}\). This results in the formation of water (H2O): \(\mathrm{OH}^{-} + \mathrm{H}^{+} \rightarrow \mathrm{H}_{2}\mathrm{O}\).
02

(b) Conjugate acid of HPO42-

To find the conjugate acid of \(\mathrm{HPO}_{4}^{2-}\), we add a proton (H+) to the species: \(\mathrm{HPO}_{4}^{2-} + \mathrm{H}^{+}\). This results in the formation of dihydrogen phosphate: \(\mathrm{HPO}_{4}^{2-} + \mathrm{H}^{+} \rightarrow \mathrm{H}_{2}\mathrm{PO}_{4}^{-}\).
03

(c) Conjugate acid of NH3

To find the conjugate acid of \(\mathrm{NH}_{3}\), we add a proton (H+) to the species: \(\mathrm{NH}_{3} + \mathrm{H}^{+}\). This results in the formation of ammonium ion: \(\mathrm{NH}_{3} + \mathrm{H}^{+} \rightarrow \mathrm{NH}_{4}^{+}\).
04

(d) Conjugate acid of F-

To find the conjugate acid of \(\mathrm{F}^{-}\), we add a proton (H+) to the species: \(\mathrm{F}^{-} + \mathrm{H}^{+}\). This results in the formation of hydrogen fluoride: \(\mathrm{F}^{-} + \mathrm{H}^{+} \rightarrow \mathrm{HF}\).
05

(e) Conjugate acid of Zn(H2O)2(OH)2

To find the conjugate acid of \(\mathrm{Zn}(\mathrm{H}_{2}\mathrm{O})_{2}(\mathrm{OH})_{2}\), we add a proton (H+) to the species: \(\mathrm{Zn}(\mathrm{H}_{2}\mathrm{O})_{2}(\mathrm{OH})_{2} + \mathrm{H}^{+}\). This results in the formation of zinc hydroxide aqua complex: \(\mathrm{Zn}(\mathrm{H}_{2}\mathrm{O})_{2}(\mathrm{OH})_{2} + \mathrm{H}^{+} \rightarrow \mathrm{Zn}(\mathrm{H}_{2}\mathrm{O})_{2}(\mathrm{OH})(\mathrm{H}_{2}\mathrm{O})^{+}\).

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Most popular questions from this chapter

Rank the following solutions in order of increasing \(\left[\mathrm{H}^{+}\right]\). \(\begin{array}{llll}0.1 & M \mathrm{HBr}, & 0.1 \mathrm{M} \mathrm{HF}, & 0.1 \mathrm{MHCHO}_{2} & 0.1 \mathrm{MHCN}\end{array}\)

At \(25^{\circ} \mathrm{C}\), a \(0.20 \mathrm{M}\) solution of methylamine \(\left(\mathrm{CH}_{3} \mathrm{NH}_{2}\right)\) is \(5.0 \%\) ionized. What is \(K_{b}\) for methylamine?

WEB Give the formula of the conjugate base of (a) \(\mathrm{HCO}_{3}^{-}\) (b) \(\mathrm{Cu}\left(\mathrm{H}_{2} \mathrm{O}\right)(\mathrm{OH})_{3}^{-}\) (c) \(\mathrm{HNO}_{2}\) (d) \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NH}_{2}\) (e) \(\mathrm{H}_{2} \mathrm{SO}_{3}\)

Solution \(\mathrm{X}\) has \(\mathrm{pH}\) 11.7. Solution \(\mathrm{Y}\) has \(\left[\mathrm{OH}^{-}\right]=4.5 \times 10^{-2}\). Which solution is more basic? Which has the higher \(\mathrm{pOH}\) ?

Using the Brønsted-Lowry model, write equations to show why the following species behave as weak acids in water. (a) \(\mathrm{Ni}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{OH}^{+}\) (b) \(\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}\) (c) \(\mathrm{H}_{2} \mathrm{~S}\) (d) \(\mathrm{HPO}_{4}^{2-}\) (e) \(\mathrm{HClO}_{2}\) (f) \(\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5}(\mathrm{OH})^{+}\)
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