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Chapter 17: Problem 51

Write the formation constant expressions for these complex ions: (a) \(\mathrm{Zn}(\mathrm{OH})_{4}^{2-},\) (b) \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}^{3+}\) (c) \(\mathrm{HgI}_{4}^{2-}\).

Short Answer

Expert verified
The formation constant expressions for the complex ions are: \n(a) Kf = [Zn(OH)4^(2-)] / ([Zn^2+][OH^-]^4) \n(b) Kf = [Co(NH3)6^(3+)] / ([Co^3+][NH3]^6) \n(c) Kf = [HgI4^(2-)] / ([Hg^2+][I^-]^4)

Step by step solution

01

Identify the central ion and ligands in Zn(OH)4^(2-)

In the complex ion Zn(OH)4^(2-), the central metal ion is Zn^2+ and the ligand is hydroxide ion (OH^-). The complex ion is formed from the reaction of one zinc ion with four hydroxide ions.
02

Write the formation constant expression for Zn(OH)4^(2-)

The formation reaction can be written as: \nZn^2+ + 4OH^- \<\> Zn(OH)4^(2-) \nThe equilibrium expression for this reaction is: \nKf = [Zn(OH)4^(2-)] / ([Zn^2+][OH^-]^4)
03

Identify the central ion and ligands in Co(NH3)6^(3+)

In the complex ion Co(NH3)6^(3+), the central metal ion is Co^3+ and the ligand is ammonia (NH3). The complex ion is formed from reaction of one cobalt ion with six ammonia molecules.
04

Write the formation constant expression for Co(NH3)6^(3+)

The formation reaction can be written as: \nCo^3+ + 6NH3 \<\> Co(NH3)6^(3+) \nThe equilibrium expression for this reaction is: \nKf = [Co(NH3)6^(3+)] / ([Co^3+][NH3]^6)
05

Identify the central ion and ligands in HgI4^(2-)

In the complex ion HgI4^(2-), the central metal ion is Hg^2+ and the ligand is iodide ion (I^-). The complex ion is formed from reaction of one mercury ion with four iodide ions.
06

Write the formation constant expression for HgI4^(2-)

The formation reaction can be written as: \nHg^2+ + 4I^- \<\> HgI4^(2-) \nThe equilibrium expression for this reaction is: \nKf = [HgI4^(2-)] / ([Hg^2+][I^-]^4)

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Most popular questions from this chapter

A volume of \(25.0 \mathrm{~mL}\) of \(0.100 \mathrm{M} \mathrm{HCl}\) is titrated against a \(0.100 \mathrm{M} \mathrm{NH}_{3}\) solution added to it from a buret. Calculate the \(\mathrm{pH}\) values of the solution (a) after \(10.0 \mathrm{~mL}\) of \(\mathrm{NH}_{3}\) solution have been added, \((\mathrm{b})\) after \(25.0 \mathrm{~mL}\) of \(\mathrm{NH}_{3}\) solution have been added, (c) after \(35.0 \mathrm{~mL}\) of \(\mathrm{NH}_{3}\) solution have been added.

The \(\mathrm{p} K_{\mathrm{a}} \mathrm{s}\) of two monoprotic acids \(\mathrm{HA}\) and \(\mathrm{HB}\) are 5.9 and \(8.1,\) respectively. Which of the two is the stronger acid?

Calculate the concentration of ions in these saturated solutions: (a) \(\left[\mathrm{I}^{-}\right]\) in AgI solution with \(\left[\mathrm{Ag}^{+}\right]=9.1 \times 10^{-9} \mathrm{M}\) (b) \(\left[\mathrm{Al}^{3+}\right]\) in \(\mathrm{Al}(\mathrm{OH})_{3}\) with \(\left[\mathrm{OH}^{-}\right]=2.9 \times 10^{-9} \mathrm{M}\)

The molar solubility of \(\mathrm{Pb}\left(\mathrm{IO}_{3}\right)_{2}\) in a \(0.10 \mathrm{M} \mathrm{NaIO}_{3}\) solution is \(2.4 \times 10^{-11} \mathrm{~mol} / \mathrm{L}\). What is \(K_{\mathrm{sp}}\) for \(\mathrm{Pb}\left(\mathrm{IO}_{3}\right)_{2} ?\)

Write the solubility product expression for the ionic compound \(\mathrm{A}_{x} \mathrm{~B}_{y}\).
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