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Chapter 13: Problem 13

In general, the attractive intermolecular forces between solvent and solute particles must be comparable or greater than solute-solute interactions for significant solubility to occur. Explain this statement in terms of the overall energetics of solution formation.

Short Answer

Expert verified
In summary, for significant solubility to occur, the attractive intermolecular forces between solvent and solute particles must be comparable or greater than solute-solute interactions. This is because the overall energetics of solution formation depend on a balance between breaking solute-solute and solvent-solvent interactions, and forming solvent-solute interactions. If the energy released from solvent-solute interactions is insufficient to break solute-solute interactions, the solubility will be low. Therefore, stronger attractive forces between solvent and solute particles are needed for efficient dissolution and higher solubility.

Step by step solution

01

Understand the meaning of the statement

The statement says that for significant solubility to occur, the intermolecular forces between solvent and solute particles must be comparable or greater than the solute-solute interactions. This means that the attractive forces between the solute and solvent particles should be strong enough to break the interactions between the solute particles and dissolve them in the solvent.
02

Analyze the energetics of solution formation

When a solute is dissolved in a solvent, there are three main processes that occur: 1. Breaking solute-solute interactions: Energy is required to break the attractive forces between solute particles. 2. Breaking solvent-solvent interactions: Energy is required to break the attractive forces between solvent particles. 3. Forming solvent-solute interactions: Energy is released when new attractive forces are formed between solute and solvent particles. The overall energetics of solution formation is determined by the balance between these three energy changes.
03

Relate energetics to solubility

For significant solubility to occur, the energy released by forming solvent-solute interactions should be comparable or greater than the energy required to break solute-solute interactions. Mathematically, this can be represented as: \( \Delta H_{solute-solvent} \geq \Delta H_{solute-solute} \), where \(\Delta H_{solute-solvent} \) is the energy change associated with forming solvent-solute interactions and \(\Delta H_{solute-solute} \) is the energy change associated with breaking solute-solute interactions. If the energy released from the formation of solvent-solute interactions is small, that means it might not be enough to break the solute-solute interactions and dissolve the solute, resulting in low solubility.
04

Conclusion

In conclusion, the attractive intermolecular forces between solvent and solute particles should be comparable or greater than solute-solute interactions for significant solubility to occur. This is because the overall energetics of solution formation depend on the balance between the energy changes associated with breaking solute-solute and solvent-solvent interactions, and the energy released by forming solvent-solute interactions. If the attractive forces between the solvent and solute particles are not strong enough, there will be insufficient energy to break the solute-solute interactions, resulting in low solubility.

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Most popular questions from this chapter

Which of the following in each pair is likely to be more soluble in water: (a) cyclohexane \(\left(\mathrm{C}_{6} \mathrm{H}_{12}\right)\) or glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) (Figure 13.12); (b) propionic acid \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COOH}\right)\) or sodium propionate \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COONa}\right) ;\) (c) \(\mathrm{HCl}\) or ethyl chloride \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{Cl}\right) ?\) Explain in each case.

Calculate the number of moles of solute present in each of the following aqueous solutions: (a) \(600 \mathrm{~mL}\) of \(0.250 \mathrm{M} \mathrm{SrBr}_{2}\), (b) \(86.4 \mathrm{~g}\) of \(0.180 \mathrm{~m} \mathrm{KCl}\), (c) \(124.0 \mathrm{~g}\) of a solution that is \(6.45 \%\) glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) by mass.

The osmotic pressure of a \(0.010 \mathrm{M}\) aqueous solution of \(\mathrm{CaCl}_{2}\) is found to be \(0.674 \mathrm{~atm}\) at \(25^{\circ} \mathrm{C}\). (a) Calculate the van't Hoff factor, \(i\), for the solution. (b) How would you expect the value of \(i\) to change as the solution becomes more concentrated? Explain.

(a) Many proteins that remain homogeneously distributed in water have molecular masses in the range of 30,000 amu and larger. In what sense is it appropriate to consider such suspensions to be colloids rather than solutions? Explain. (b) What general name is given to a colloidal dispersion of oneliquid in another? What is an emulsifying agent?

Indicate the type of solute-solvent interaction (Section 11.2) that should be most important in each of the following solutions: (a) \(\mathrm{CCl}_{4}\) in benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\),(b) methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\) in water, (c) \(\mathrm{KBr}\) in water, (d) \(\mathrm{HCl}\) in acetonitrile \(\left(\mathrm{CH}_{3} \mathrm{CN}\right)\).
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