/*! 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 39 A concentrated aqueous copper(II... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 20: Problem 39

A concentrated aqueous copper(II) chloride solution is bright green in color. When diluted with water, the solution becomes light blue. Explain.

Short Answer

Expert verified
The color difference in the copper(II) chloride solution before and after dilution is due to changes in the electronic environment of the copper ion. A concentrated solution results in green colour due to lesser d-d transitions, while dilution causes an increase in the d-d transitions and results in a light blue colour.

Step by step solution

01

Identify the Compound

Firstly, recognize that copper(II) chloride is a transition metal complex. In aqueous solution, it exists as the complex ion [Cu(H2O)6]2+.
02

Determining the Cause of the Color Change

The color of transition metal complexes is based on the d-d transition of electrons. In a concentrated solution, the water molecules are able to move less freely and hence are less able to contribute to the d-d transitions resulting in the green color. As the number of water molecules increases in relation to copper ions (dilution), the water molecules are more able to contribute to the d-d transitions. This results in greater d-d transitions and the observed colour change to light blue.
03

Conclusion

Thus, it can be concluded that the color difference in the copper(II) chloride solution before and after dilution is due to changes in the electronic environment of copper ions in solution. When more water is added, the increased number of water molecules relative to copper ions effects the observed colour change.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

The formation constant for the reaction \(\mathrm{Ag}^{+}+\) \(2 \mathrm{NH}_{3} \rightleftharpoons\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+}\) is \(1.5 \times 10^{7}\) and that for the reaction \(\mathrm{Ag}^{+}+2 \mathrm{CN}^{-} \rightleftharpoons\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}\) is 1.0 \(\times 10^{21}\) at \(25^{\circ} \mathrm{C}\) (see Table 17.4 ). Calculate the equilibrium constant at \(25^{\circ} \mathrm{C}\) for the reaction $$\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+}+2 \mathrm{CN}^{-} \rightleftharpoons\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}+2 \mathrm{NH}_{3}$$

Aqueous copper(II) sulfate solution is blue in color. When aqueous potassium fluoride is added, a green precipitate is formed. When aqueous potassium chloride is added instead, a bright-green solution is formed. Explain what is happening in these two cases.

A student prepared a cobalt complex that has one of the following structures: \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{3}\), \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}\right] \mathrm{Cl}_{2},\) or \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right] \mathrm{Cl} .\) Explain how the student would distinguish among these possibilities by an electrical conductance experiment. At the student's disposal are three strong electrolytes: \(\mathrm{NaCl}, \mathrm{MgCl}_{2},\) and \(\mathrm{FeCl}_{3},\) which may be used for comparison purposes.

Write the electron configurations of these ions: \(\mathrm{V}^{5+}\) \(\mathrm{Cr}^{3+}, \mathrm{Mn}^{2+}, \mathrm{Fe}^{3+}, \mathrm{Cu}^{2+}, \mathrm{Sc}^{3+}, \mathrm{T}_{1}^{4+}\)

In a dilute nitric acid solution, \(\mathrm{Fe}^{3+}\) reacts with thiocyanate ion \(\left(\mathrm{SCN}^{-}\right)\) to form a dark-red complex: $$\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}+\mathrm{SCN}^{-} \rightleftharpoons \mathrm{H}_{2} \mathrm{O}+\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{NCS}\right]^{2+}$$ The equilibrium concentration of \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{NCS}\right]^{2+}\) may be determined by how darkly colored the solution is (measured by a spectrometer). In one such experiment, \(1.0 \mathrm{~mL}\) of \(0.20 \mathrm{M} \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}\) was mixed with \(1.0 \mathrm{~mL}\) of \(1.0 \times 10^{-3} M \mathrm{KSCN}\) and \(8.0 \mathrm{~mL}\) of dilute \(\mathrm{HNO}_{3}\). The color of the solution quantitatively indicated that the \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{NCS}\right]^{2+}\) concentration was \(7.3 \times 10^{-5} M\). Calculate the formation constant for \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{NCS}\right]^{2+}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Chemical Reactions

Read Explanation

Organic Chemistry

Read Explanation

Making Measurements

Read Explanation

Chemistry Branches

Read Explanation

The Earths Atmosphere

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.