/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 16 The stepwise formation constants... [FREE SOLUTION] | 91影视

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Chapter 15: Problem 16

The stepwise formation constants for a complex ion usually have values much greater than \(1 .\) What is the significance of this?

Short Answer

Expert verified
The significance of stepwise formation constants for a complex ion having values much greater than 1 indicates that the complex ion formation is favored, implying that the reaction is more likely to proceed in the forward direction. This results in increased stability of the complex ion, making the metal ion more likely to combine with the ligands easily and increasing its solubility. Hence, understanding stepwise formation constants is essential in coordination chemistry for determining the stability and solubility of metal ions in solution.

Step by step solution

01

Define stepwise formation constants

Stepwise formation constants are equilibrium constants that represent the successive addition of ligands to a metal ion, forming a complex ion. In other words, they describe the stability of the intermediate complexes formed during the step-by-step process of the complex ion formation.
02

Explain the significance of formation constants values greater than 1

The significance of stepwise formation constants having values much greater than 1 indicates that the formation of the complex ion is favored, meaning that the reaction is more likely to proceed in the forward direction, leading to the formation of the complex ion. Basically, a stepwise formation constant with a value much greater than 1 indicates that the equilibrium position of the reaction lies far to the right, which means that the complex ion is very stable, and the metal ion tends to combine with the ligands easily, making it highly soluble.
03

Relate the significance to the solubility of metal ions

The formation of complex ions can have an impact on the solubility of some metal ions in solution. When a metal ion forms a coordinative bond with a ligand (e.g., a counter ion or a neutral molecule) to create a complex ion, equilibria are established. If the complex ion is significantly more stable than the free metal ion in solution, the equilibrium will shift towards the formation of the complex ion. This effectively increases the solubility of the metal ion by reducing its concentration in solution. Having stepwise formation constants much greater than 1 helps us understand which metal ions will be more likely to form stable complex ions, and thus increase the solubility of these metals, making it an essential concept in coordination chemistry. In conclusion, the significance of the stepwise formation constants for a complex ion having values much greater than 1 indicates that the complex ion formation is favored and leads to increased solubility and stability of metal ions in solution.

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Most popular questions from this chapter

a. Calculate the molar solubility of \(\operatorname{Sr} \mathrm{F}_{2}\) in water, ignoring the basic properties of \(\left.\mathrm{F}^{-} . \text {(For } \operatorname{Sr} \mathrm{F}_{2}, K_{\mathrm{sp}}=7.9 \times 10^{-10} .\right)\). b. Would the measured molar solubility of \(\operatorname{Sr} \mathrm{F}_{2}\) be greater than or less than the value calculated in part a? Explain. c. Calculate the molar solubility of \(\operatorname{Sr} \mathrm{F}_{2}\) in a solution buffered at \(\mathrm{pH}=2.00 .\left(K_{\mathrm{a}} \text { for } \mathrm{HF} \text { is } 7.2 \times 10^{-4} .\right)\).

The overall formation constant for \(\mathrm{HgI}_{4}^{2-}\) is \(1.0 \times 10^{30}\) That is, $$ 1.0 \times 10^{30}=\frac{\left[\mathrm{HgI}_{4}^{2-}\right]}{\left[\mathrm{Hg}^{2+}\right]\left[\mathrm{I}^{-}\right]^{4}} $$ What is the concentration of \(\mathrm{Hg}^{2+}\) in \(500.0 \mathrm{mL}\) of a solution that was originally \(0.010\) \(M\) \(\mathrm{Hg}^{2+}\) and \(0.78\) \(M\) \(\mathrm{I}^{-} ?\) The reaction is $$\mathrm{Hg}^{2+}(a q)+4 \mathrm{I}^{-}(a q) \rightleftharpoons \mathrm{HgI}_{4}^{2-}(a q)$$

A solution is prepared by mixing \(75.0 \mathrm{mL}\) of \(0.020\) \(M\) \(\mathrm{BaCl}_{2}\) and \(125 \mathrm{mL}\) of \(0.040\) \(M\) \(\mathrm{K}_{2} \mathrm{SO}_{4}\). What are the concentrations of barium and sulfate ions in this solution? Assume only \(\mathrm{SO}_{4}^{2-}\) ions \(\left(\text { no } \mathrm{HSO}_{4}^{-}\right)\) are present.

List some ways one can increase the solubility of a salt in water.

A solution contains \(1.0 \times 10^{-5} M \mathrm{Na}_{3} \mathrm{PO}_{4} .\) What is the minimum concentration of \(\mathrm{AgNO}_{3}\) that would cause precipitation of solid \(\mathrm{Ag}_{3} \mathrm{PO}_{4}\left(K_{\mathrm{sp}}=1.8 \times 10^{-18}\right) ?\)
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