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Chapter 16: Problem 60

Write equations for the stepwise formation of each of the following complex ions. a. \(\mathrm{CoF}_{6}^{3-}\) b. \(\mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}^{2+}\)

Short Answer

Expert verified
The stepwise formation equations for the complex ion \(\mathrm{CoF}_{6}^{3-}\) are as follows: 1. Co鲁鈦 + F鈦 鈫 CoF虏鈦 2. CoF虏鈦 + F鈦 鈫 CoF鈧傗伜 3. CoF鈧傗伜 + F鈦 鈫 CoF鈧 4. CoF鈧 + F鈦 鈫 CoF鈧勨伝 5. CoF鈧勨伝 + F鈦 鈫 CoF鈧吢测伝 6. CoF鈧吢测伝 + F鈦 鈫 CoF鈧喡斥伝 The stepwise formation equations for the complex ion \(\mathrm{Zn}(\mathrm{NH}_{3})_{4}^{2+}\) are as follows: 1. Zn虏鈦 + NH鈧 鈫 Zn(NH鈧)虏鈦 2. Zn(NH鈧)虏鈦 + NH鈧 鈫 Zn(NH鈧)鈧偮测伜 3. Zn(NH鈧)鈧偮测伜 + NH鈧 鈫 Zn(NH鈧)鈧兟测伜 4. Zn(NH鈧)鈧兟测伜 + NH鈧 鈫 Zn(NH鈧)鈧劼测伜

Step by step solution

01

Identify components of the complex ions

In order to write stepwise formation equations for the complex ions, we first need to identify the components involved in the formation of each ion. For complex ion a: \(\mathrm{CoF}_{6}^{3-}\) - Central metal ion: Co (Cobalt) - Ligand: F鈦 (Fluoride ion) - Charge: 3- For complex ion b: \(\mathrm{Zn}(\mathrm{NH}_{3})_{4}^{2+}\) - Central metal ion: Zn (Zinc) - Ligand: NH鈧 (Ammonia) - Charge: 2+
02

Write the stepwise formation equations for \(\mathrm{CoF}_{6}^{3-}\)

Now we will write the stepwise formation equations for the cobalt fluoride complex ion \(\mathrm{CoF}_{6}^{3-}\): 1. Co鲁鈦 + F鈦 鈫 CoF虏鈦 2. CoF虏鈦 + F鈦 鈫 CoF鈧傗伜 3. CoF鈧傗伜 + F鈦 鈫 CoF鈧 4. CoF鈧 + F鈦 鈫 CoF鈧勨伝 5. CoF鈧勨伝 + F鈦 鈫 CoF鈧吢测伝 6. CoF鈧吢测伝 + F鈦 鈫 CoF鈧喡斥伝 The stepwise formation of \(\mathrm{CoF}_{6}^{3-}\) is completed.
03

Write the stepwise formation equations for \(\mathrm{Zn}(\mathrm{NH}_{3})_{4}^{2+}\)

Now we will write the stepwise formation equations for the zinc ammonia complex ion \(\mathrm{Zn}(\mathrm{NH}_{3})_{4}^{2+}\): 1. Zn虏鈦 + NH鈧 鈫 Zn(NH鈧)虏鈦 2. Zn(NH鈧)虏鈦 + NH鈧 鈫 Zn(NH鈧)鈧偮测伜 3. Zn(NH鈧)鈧偮测伜 + NH鈧 鈫 Zn(NH鈧)鈧兟测伜 4. Zn(NH鈧)鈧兟测伜 + NH鈧 鈫 Zn(NH鈧)鈧劼测伜 The stepwise formation of \(\mathrm{Zn}(\mathrm{NH}_{3})_{4}^{2+}\) is completed.

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Most popular questions from this chapter

The solubility of \(\mathrm{Ce}\left(\mathrm{IO}_{3}\right)_{3}\) in a \(0.20 \mathrm{M} \mathrm{KIO}_{3}\) solution is \(4.4 \times\) \(10^{-8} \mathrm{~mol} / \mathrm{L}\). Calculate \(K_{\mathrm{sp}}\) for \(\mathrm{Ce}\left(\mathrm{IO}_{3}\right)_{3}\).

A \(50.0-\mathrm{mL}\) sample of \(0.00200 \mathrm{M} \mathrm{AgNO}_{3}\) is added to \(50.0 \mathrm{~mL}\) of \(0.0100 M \mathrm{NaIO}_{3-}\) What is the equilibrium concentration of \(\mathrm{Ag}^{+}\) in solution? \(\left(K_{\mathrm{sp}}\right.\) for \(\mathrm{AgIO}_{3}\) is \(3.0 \times 10^{-8}\).)

A solution is prepared by mixing \(100.0 \mathrm{~mL}\) of \(1.0 \times 10^{-2} M\) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) and \(100.0 \mathrm{~mL}\) of \(1.0 \times 10^{-3} \mathrm{M} \mathrm{NaF}\). Will \(\mathrm{PbF}_{2}(s)\) \(\left(K_{\mathrm{sp}}=4 \times 10^{-8}\right)\) precipitate?

a. Calculate the molar solubility of AgBr in pure water. \(K_{\text {sp }}\) for \(\mathrm{AgBr}\) is \(5.0 \times 10^{-13}\) b. Calculate the molar solubility of AgBr in \(3.0 M \mathrm{NH}_{3}\). The overall formation constant for \(\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}\) is \(1.7 \times 10^{7}\), that is, \(\mathrm{Ag}^{+}(a q)+2 \mathrm{NH}_{3}(a q) \longrightarrow \mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}(a q) \quad K=1.7 \times 10^{7}\) c. Compare the calculated solubilities from parts a and b. Explain any differences. d. What mass of AgBr will dissolve in \(250.0 \mathrm{~mL}\) of \(3.0 \mathrm{M} \mathrm{NH}_{3}\) ? e. What effect does adding \(\mathrm{HNO}_{3}\) have on the solubilities calculated in parts a and b?

Solutions of sodium thiosulfate are used to dissolve unexposed \(\mathrm{AgBr}\left(K_{\mathrm{sp}}=5.0 \times 10^{-13}\right)\) in the developing process for blackand-white film. What mass of AgBr can dissolve in \(1.00 \mathrm{~L}\) of \(0.500 \mathrm{M} \mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3} ? \mathrm{Ag}^{+}\) reacts with \(\mathrm{S}_{2} \mathrm{O}_{3}{ }^{2-}\) to form a complex ion:
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