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Chapter 16: Problem 61

Write equations for the stepwise formation of each of the following complex ions. a. \(\mathrm{Ni}(\mathrm{CN})_{4}^{2-}\) $$ \text { b. } \mathrm{V}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}{ }^{3-} $$

Short Answer

Expert verified
Short Answer: The stepwise formation equations for the complex ions are as follows: a. Ni(CN)₄²⁻ : 1. Ni²⁺ + CN⁻ → NiCN²⁻ 2. NiCN²⁻ + CN⁻ → Ni(CN)₂³⁻ 3. Ni(CN)₂³⁻ + CN⁻ → Ni(CN)₃⁴⁻ 4. Ni(CN)₃⁴⁻ + CN⁻ → Ni(CN)₄²⁻ b. V(C₂O₄)₃³⁻ : 1. V³⁺ + C₂O₄²⁻ → VC₂O₄⁺ 2. VC₂O₄⁺ + C₂O₄²⁻ → V(C₂O₄)₂⁻ 3. V(C₂O₄)₂⁻ + C₂O₄²⁻ → V(C₂O₄)₃³⁻

Step by step solution

01

Identify the central metal ion and ligands

In this complex ion, the central metal ion is Ni²⁺ (nickel ion) and the ligand is the CN⁻ ion (cyanide ion). There are 4 CN⁻ ions surrounding the Ni²⁺ ion.
02

Write the stepwise formation equations for the complex ion

Now we will write the equations for the formation of the Ni(CN)₄²⁻ complex ion as the CN⁻ ions progressively bind to the Ni²⁺ ion. 1. Ni²⁺ + CN⁻ → NiCN²⁻ 2. NiCN²⁻ + CN⁻ → Ni(CN)₂³⁻ 3. Ni(CN)₂³⁻ + CN⁻ → Ni(CN)₃⁴⁻ 4. Ni(CN)₃⁴⁻ + CN⁻ → Ni(CN)₄²⁻ b. V(C₂O₄)₃³⁻
03

Identify the central metal ion and ligands

In this complex ion, the central metal ion is V³⁺ (vanadium ion) and the ligand is the C₂O₄²⁻ ion (oxalate ion). There are 3 C₂O₄²⁻ ions surrounding the V³⁺ ion.
04

Write the stepwise formation equations for the complex ion

Now we will write the equations for the formation of the V(C₂O₄)₃³⁻ complex ion as the C₂O₄²⁻ ions progressively bind to the V³⁺ ion. 1. V³⁺ + C₂O₄²⁻ → VC₂O₄⁺ 2. VC₂O₄⁺ + C₂O₄²⁻ → V(C₂O₄)₂⁻ 3. V(C₂O₄)₂⁻ + C₂O₄²⁻ → V(C₂O₄)₃³⁻ These are the stepwise formation equations for the given complex ions.

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Most popular questions from this chapter

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

Calculate the final concentrations of \(\mathrm{K}^{+}(a q), \mathrm{C}_{2} \mathrm{O}_{4}{ }^{2-}(a q)\), \(\mathrm{Ba}^{2+}(a q)\), and \(\mathrm{Br}^{-}(a q)\) in a solution prepared by adding \(0.100 \mathrm{~L}\) of \(0.200 \mathrm{M} \mathrm{K}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) to \(0.150 \mathrm{~L}\) of \(0.250 \mathrm{M} \mathrm{BaBr}_{2}\). (For \(\left.\mathrm{BaC}_{2} \mathrm{O}_{4}, K_{\mathrm{sp}}=2.3 \times 10^{-\mathrm{s}} .\right)\)

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

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 \(\mathrm{Ce}\left(\mathrm{IO}_{3}\right)_{3} .\)

Write balanced equations for the dissolution reactions and the corresponding solubility product expressions for each of the following solids. a. \(\mathrm{Ag}_{2} \mathrm{CO}_{3}\) b. \(\mathrm{Ce}\left(\mathrm{IO}_{3}\right)_{3}\) c. \(\mathrm{BaF}_{2}\)
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