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Chapter 16: Problem 15

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

Short Answer

Expert verified
To increase the solubility of a salt in water, one can: 1. Increase the temperature, as higher temperatures result in increased kinetic energy and more effective collisions between solute and solvent particles. 2. Stir the solution to disrupt the concentrated solute layer and increase the rate of dissolution. 3. Reduce particle size by grinding or crushing the salt to increase the surface area for solute-solvent interaction. 4. Use a high-pressure environment (mostly in industrial applications) to force solute particles closer together and improve solubility. 5. Utilize a cosolvent, like adding a small amount of alcohol to water, to enhance solubility by breaking down the lattice structure of the solute, but this method should be used with caution and appropriate knowledge.

Step by step solution

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1. Increase Temperature

Increasing the temperature of the water can increase the solubility of salts. Solubility is affected by temperature because the rate at which solute particles dissolve increases when the temperature is increased. This is because the kinetic energy of the particles increases, leading to more effective collisions between solute and solvent particles.
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2. Stirring the Solution

Stirring the solution can increase the solubility of a salt in water. When a solute is added to a solvent (water), a layer of highly concentrated solute forms around the solute particles. Stirring the solution disrupts this layer and brings fresh solvent into contact with the solute, increasing the rate of dissolution and thus improving solubility.
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3. Reducing Particle Size

The size of salt particles can also affect solubility. Smaller particles create a larger surface area for the solute-solvent interaction, which increases the rate at which the solute dissolves. Grinding or crushing the salt into smaller particles can increase the solubility of the salt in water.
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4. Using a High-Pressure Environment

Some salts have increased solubility in high-pressure environments. This is because the high pressure forces the solute particles closer together, making it easier for the solvent molecules to interact with the solute and dissolve it. This method might not be applicable in a typical home or classroom setting, it is used in some industrial applications.
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5. Utilizing a Cosolvent

Some salts have increased solubility when another solvent is added to the solution. For example, adding a small amount of alcohol to water can enhance the solubility of some salts. The cosolvent can help break down the lattice structure of the solute, allowing the water molecules to more effectively interact with and dissolve the salt. This method should be used with caution and should only be done with appropriate knowledge about the solvents and solutes being mixed.

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Most popular questions from this chapter

Calculate the solubility of \(\mathrm{Co}(\mathrm{OH})_{2}(s)\left(K_{\mathrm{sp}}=2.5 \times 10^{-16}\right)\) in a buffered solution with a pH of \(11.00\).

Aluminum ions react with the hydroxide ion to form the precipitate \(\mathrm{Al}(\mathrm{OH})_{3}(s)\), but can also react to form the soluble complex ion \(\mathrm{Al}(\mathrm{OH})_{4}^{-} .\) In terms of solubility, \(\mathrm{Al}(\mathrm{OH})_{3}(s)\) will be more soluble in very acidic solutions as well as more soluble in very basic solutions. a. Write equations for the reactions that occur to increase the solubility of \(\mathrm{Al}(\mathrm{OH})_{3}(s)\) in very acidic solutions and in very basic solutions. b. Let's study the \(\mathrm{pH}\) dependence of the solubility of \(\mathrm{Al}(\mathrm{OH})_{3}(s)\) in more detail. Show that the solubility of \(\mathrm{Al}(\mathrm{OH})_{3}\), as a function of \(\left[\mathrm{H}^{+}\right]\), obeys the equation $$S=\left[\mathrm{H}^{+}\right]^{3} K_{\mathrm{sp}} / K_{\mathrm{w}}^{3}+K K_{\mathrm{w}} /\left[\mathrm{H}^{+}\right]$$ where \(S=\) solubility \(=\left[\mathrm{Al}^{3+}\right]+\left[\mathrm{Al}(\mathrm{OH})_{4}^{-}\right]\) and \(K\) is the equilibrium constant for $$\mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{OH}^{-}(a q) \rightleftharpoons \mathrm{Al}(\mathrm{OH})_{4}^{-}(a q)$$ c. The value of \(K\) is \(40.0\) and \(K_{\mathrm{se}}\) for \(\mathrm{Al}(\mathrm{OH})_{3}\) is \(2 \times 10^{-32}\). Plot the solubility of \(\mathrm{Al}(\mathrm{OH})_{3}\) in the \(\mathrm{pH}\) range \(4-12\).

The concentration of \(\mathrm{Pb}^{2+}\) in a solution saturated with \(\mathrm{PbBr}_{2}(s)\) is \(2.14 \times 10^{-2} M .\) Calculate \(K_{\text {sp }}\) for \(\mathrm{PbBr}_{2}\).

The solubility of copper(II) hydroxide in water can be increased by adding either the base \(\mathrm{NH}_{3}\) or the acid \(\mathrm{HNO}_{3} .\) Explain. Would added \(\mathrm{NH}_{3}\) or \(\mathrm{HNO}_{3}\) have the same effect on the solubility of silver acetate or silver chloride? Explain.

When aqueous KI is added gradually to mercury(II) nitrate, an orange precipitate forms. Continued addition of KI causes the precipitate to dissolve. Write balanced equations to explain these observations. (Hint: \(\mathrm{Hg}^{2+}\) reacts with \(\mathrm{I}^{-}\) to form \(\mathrm{HgI}_{4}{ }^{2-}\).)
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