Advanced inorganic problems
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1. Identify the conjugate acids of the bases C5H5N (pyridine), HPO42-, O2-, CH3COOH, [Co(CO)4]-, CN-.
2. Use Pauling's rules to place the following acids in order of increasing acid strength: HNO2, H2SO4, HBrO3, and HClO4 in a nonlevelling solvent.
3. Which member of the following pairs is the stronger acid? Give reasons for the choice.
[Fe(OH2)6]3+ or [Fe(OH2)6]2+
4. Arrange the oxides Al2O3, B2O3, BaO, CO2, Cl2O7, SO3 in order from the most acidic through amphoteric to the most basic?
5. Which of the following reactions are predicated to have an equilibrium constant greater than 1? Unless otherwise stated, assume gas-phase or hydrocarbon solution and 25oC.
R3PBBr3 + R3NBF3 R3PRBF3 + R3NBBr3
6. Predict whether the equilibrium constants for the following reactions should be greater than 1 or less than 1
[CuI4]2-(aq) + [CuCl4]3-(aq) [CuCl4]2-(aq) + [CuI4]3-(aq)
7. Balance the following redox reaction in acid solution: MnO4- + H2SO3 Mn2+ + HSO4-. Predict the qualitative pH dependence on the net potential for this reaction (that is, increases, decreases, remains the same).
8. Use standard potentials as a quide to write equations for the main net reaction that you would predict in the following experiments
I2 is added to excess aqueous HClO3.
9. Characterize the condition of acidity or basicity that would most favour the following transformations in aqueous solution.
ClO4- ClO3-
10. Give an example of an acidic, a basic, and an amphoteric oxide from the same family in the Periodic Table.
11. Identify the following as Lewis acids or bases and rank them in order of increasing hardness. Explain the reasoning.
O(CH3)2 S(CH3)2 Se(CH3)2
12. The figure below is part of the modified Latimer diagram for nitrogen under conditions
of 1.0 M OH-(aq). Identify the species in the Latimer diagram provided that are unstable
with respect to disproportionation in 1.0 M hydroxide. State your reasoning. Calculate x.
13. Write and balance the equation for the disproportionation of sulfite (SO32-) into sulfate and sulfide ions in basic solution.
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Solution includes a number of advanced Inorganic problems with high qualtiy explanation along with working out to solve the problems.
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1. Identify the conjugate acids of the bases C5H5N (pyridine), HPO42-, O2-, CH3COOH, [Co(CO)4]-, CN-.
A conjugate acid is a species with one extra proton (H+) than the parent base.
Therefore, for pyridine, conjugate acid will be pyridinium ion C5H6N+ as shown below:
+
for HPO4^2-, conjugate acid will be H2PO4^-1
for O^2-, conjugate acid will be OH^-1.
For CH3COOH, conjugate acid will be CH3C(OH)2^+
For Co(CO)4^-1, conjugate acid will be HCo(CO)4
For CN^-1, conjugate acid will be HCN.
2. Use Pauling's rules to place the following acids in order of increasing acid strength: HNO2, H2SO4, HBrO3, and HClO4 in a nonlevelling solvent.
Pauling stated two empirical rules of oxo-acid strength:
1. For OpE(OH)q, pKa ~ 8 - 5p
2. The successive pKa values of polyprotic acids (i.e. q >1) increase by 5 units for each successive proton transfer.
This suggests that the dominant factor in determining the strength of oxoacids is the number of terminal oxygen atoms attached to the central element E.
On the basis of these rules, we can arrange the given acids in increasing acidic strength as:
HNO2 < HBrO3 < H2SO4< HClO4
3. Which member of the following pairs is the stronger acid? Give reasons for the choice.
[Fe(OH2)6]3+ or [Fe(OH2)6]2+
The Fe(III) complex, [Fe(OH2)6]^3+, is the stronger acid on of thethe basis of its higher charge as well as smaller ionic radius as compared to Fe(II). The electrostatic parameter will be considerably higher for z = 3 than for z = 2. The decrease in the radius on going from the Fe(II) to the Fe(III) species will enhance the differences in for the two species and increasing the polarization power of Fe(III) as compared to Fe(II), making Fe(III) aqua complex more acidic than Fe(II).
4. Arrange the oxides Al2O3, B2O3, BaO, CO2, Cl2O7, SO3 in order from the most acidic through amphoteric to the most basic?
Out of the given options, the compounds B2O3, CO2, Cl2O7, and SO3 are acidic, since the central element for each of them is found in the acidic region of the ...
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