Concept explainers
(a)
Interpretation:
With reference to the stability of
Concept introduction:
A complex ion is formed when a metal ion reacts with a Lewis base in solution. This reaction is defined in relation to
The Metal ion which is positively charged functions as a Lewis acid and Lewis base or the ligand has one or more lone pairs of electrons. For example, Cu2+, which is a highly charged and small metal ion having a significant tendency to function as Lewis acids, consequently exhibiting the highest affinity to form complex ions.
The development of a complexion is a stepwise procedure, and every step has its equilibrium constant. When two of the equations are added together, the equilibrium constants multiply. The Equilibrium Constant reflects the concentration in a reaction, which is the molarity, written as moles per liter(M = mol/L).
The products of a reaction are present in the numerator, and the denominator has the reactants. The alphabets in upper-case are the molar concentrations of the reactants and products, and the alphabets in lower-case are the
(b)
Interpretation:
The value of
Concept introduction:
A complex ion is formed when a metal ion reacts with a Lewis base in solution. This reaction is defined concerning chemical equilibrium. A complexion comprises of a ligand and a metal ion as a result of an interaction of Lewis acid-base.
The Metal ion which is positively charged functions as a Lewis acid and Lewis base or the ligand has one or more lone pairs of electrons. For example, Cu2+, which is a highly charged and small metal ion having a significant tendency to function as Lewis acids, consequently exhibiting the highest affinity to form complex ions.
The development of a complexion is a stepwise procedure, and every step has its equilibrium constant. When two of the equations are added together, the equilibrium constants multiply. The Equilibrium Constant reflects the concentration in a reaction, which is the molarity, written as moles per liter(M = mol/L).
The products of a reaction are present in the numerator, and the denominator has the reactants. The alphabets in upper-case are the molar concentrations of the reactants and products, and the alphabets in lower-case are the stoichiometric coefficients which balance the equation.
(c)
Interpretation:
For the value of [Co3+] calculated in part (b), the reaction will occur or not should be determined.
Concept introduction:
A complex ion is formed when a metal ion reacts with a Lewis base in solution. This reaction is defined concerning chemical equilibrium. A complexion comprises of a ligand and a metal ion as a result of an interaction of Lewis acid-base.
The Metal ion which is positively charged functions as a Lewis acid and Lewis base or the ligand has one or more lone pairs of electrons. For example, Cu2+, which is a highly charged and small metal ion having a significant tendency to function as Lewis acids, consequently exhibiting the highest affinity to form complex ions.
The development of a complexion is a stepwise procedure, and every step has its equilibrium constant. When two of the equations are added together, the equilibrium constants multiply. The Equilibrium Constant reflects the concentration in a reaction, which is the molarity, written as moles per liter(M = mol/L).
The products of a reaction are present in the numerator, and the denominator has the reactants. The alphabets in upper-case are the molar concentrations of the reactants and products, and the alphabets in lower-case are the stoichiometric coefficients which balance the equation.
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Chapter 24 Solutions
GENERAL CHEMISTRY(LL)-W/MASTERINGCHEM.
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- 1. Answer the following questions: a) Why aqueous solutions of KMNO4 are not entirely stable? b) What factors affect the decomposition of KMNO4? c) How can you prepare 1L of 0.01M solution of KMnO4 (FW = 158.04g) in the laboratory? 2. Derive and Calculate the equilibrium constant of the reaction? 2 Fe3+ + 31 -→ 2 Fe* + P- 2 Fe3+ + 2 e - +2 e E = 0.771 V E = 0.536 V -> 2 Fe2+ -> 3. Compare between Galvanic cell and Electrolytic cell? 4. Explain how is K¿Cr,07 is applied in titration of Fe (II) solution? 5. Why reductants are seldom used for direct titration of oxidized analyte? 6. How is sodium thiosulfate solution is used to determine oxidizing agents (such as ClO) by indirect procedure that involves iodine as an intermediate?arrow_forwardThe correct statement is….Crystal field strength at [PtCl4]2- > [Pt(NH3)4]2+Crystal field strength at [NiCl4]2- > [PtCl4]2-Crystal field strength at [CoF6]3- > [CoI6]3-Crystal field strength at [Co(SCN)6]3- > [Co(NCS)6]3-arrow_forwardThe intermediate [Fe(SCN)(H2O)5]2+ is detected in the reaction of [Co(NCS)(NH3)5]2+ with [Fe(H2O)6]2+ in aqueous medium to produce [Co(H2O)6]2+ and [Fe(H2O)6]3+. This reaction occurs by a mechanism: Select one: a. Internal sphereb. Dissociativec. External sphered. Associativearrow_forward
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- Which of the following compounds can exhibit geometric isomerism? Select one: a. [Co(NH3)5Cl]2+ b. [Cu(CN)2]- c. [Zn(NH3)2Cl2] (tetrahedral) d. [Pt(NH3)2Cl2] (square plane) e. [Cu(NH3)4]2+ (square plane)arrow_forward20.60 Commercial silver-plating operations frequently use a solution containing the complex Ag(CN); ion. Be- cause the formation constant (K) is quite large, this procedure ensures that the free Ag" concentration in solution is low for uniform electrodeposition. In one process, a chemist added 9.0 L of 5.0 M NACN to 90.0 L of 0.20 M AGNO,. Calculate the concentration of free Ag" ions at equilibrium. See Table 17.4 for K, value.arrow_forward10) Indicate which species will be relatively easily reduced and which one will be easily oxidized. Explain your answer. Hint: It is related to 18-electron rule. 10 [Co(n³Cp)₂], [Fe(n³Cp)₂], [V(CO)], [Mn(CO)5]arrow_forward
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