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Chapter 11: Problem 24

In order for sodium chloride to dissolve in water, a small amount of energy must be added during solution formation. This is not energetically favorable. Why is \(\mathrm{NaCl}\) so soluble in water?

Short Answer

Expert verified
NaCl is soluble in water primarily due to its strong hydration energy. When NaCl dissolves, the ionic bonds in the crystal lattice are broken, and the ions are surrounded by water molecules. The dissolution process involves two energy changes: the endothermic lattice energy and the exothermic hydration energy. In the case of NaCl, the strong hydration energy, which results from the attractions between the ions and water molecules, compensates for the energy required to break the ionic bonds in the crystal lattice. This makes the dissolution process energetically favorable, allowing NaCl to dissolve in water.

Step by step solution

01

Understand the dissolution process

When a salt dissolves in water, the crystal lattice of the salt is broken apart and the ions are surrounded by water molecules. This process involves overcoming the attraction between the ions in the crystal lattice and the formation of new attractions between the ions and the water molecules.
02

Consider the energy changes during dissolution

Dissolving a salt in water involves two main energy changes: 1. The energy required to break the ionic bonds in the crystal lattice (lattice energy) - an endothermic process that consumes energy. 2. The energy released when ions form new attractions with water molecules (hydration energy) - an exothermic process that releases energy.
03

Factors affecting the solubility of NaCl in water

The solubility of NaCl in water is affected by the balance between the lattice energy and the hydration energy. When the hydration energy is greater than or equal to the lattice energy, the process becomes energetically favorable, and NaCl will dissolve in water.
04

Discuss the specific interactions that make NaCl soluble in water

NaCl is soluble in water primarily because of the strong hydration energy. When NaCl dissolves in water, the positively charged Na+ ions are attracted to the partially negative oxygen atoms of the water molecules, while the negatively charged Cl- ions are attracted to the partially positive hydrogen atoms of the water molecules. These attractions result in the formation of a hydration shell around the ions, which stabilizes them in the solution. This strong hydration energy compensates for the energy required to break the ionic bonds in the crystal lattice, making the dissolution process energetically favorable.

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Most popular questions from this chapter

Creatinine, \(\mathrm{C}_{4} \mathrm{H}_{7} \mathrm{~N}_{3} \mathrm{O}\), is a by-product of muscle metabolism, and creatinine levels in the body are known to be a fairly reliable indicator of kidney function. The normal level of creatinine in the blood for adults is approximately \(1.0 \mathrm{mg}\) per deciliter (dL) of blood. If the density of blood is \(1.025 \mathrm{~g} / \mathrm{mL}\), calculate the molality of a normal creatinine level in a \(10.0-\mathrm{mL}\) blood sample. What is the osmotic pressure of this solution at \(25.0^{\circ} \mathrm{C} ?\)

A solution of phosphoric acid was made by dissolving \(10.0 \mathrm{~g}\) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) in \(100.0 \mathrm{~mL}\) water. The resulting volume was \(104 \mathrm{~mL}\) Calculate the density, mole fraction, molarity, and molality of the solution. Assume water has a density of \(1.00 \mathrm{~g} / \mathrm{cm}^{3}\).

What mass of glycerin \(\left(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}_{3}\right)\), a nonelectrolyte, must be dissolved in \(200.0 \mathrm{~g}\) water to give a solution with a freezing point of \(-1.50^{\circ} \mathrm{C} ?\)

A \(0.500-\mathrm{g}\) sample of a compound is dissolved in enough water to form \(100.0 \mathrm{~mL}\) of solution. This solution has an osmotic pressure of \(2.50\) atm at \(25^{\circ} \mathrm{C}\). If each molecule of the solute disso- ciates into two particles (in this solvent), what is the molar mass of this solute?

Using the phase diagram for water and Raoult's law, explain why salt is spread on the roads in winter (even when it is below freezing).
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