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Chapter 8: Problem 57

What is the difference between a saturated solution and a supersaturated solution?

Short Answer

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Question: Explain the difference between a saturated solution and a supersaturated solution, along with examples. Answer: A saturated solution is a solution containing the maximum amount of solute that can be dissolved in a solvent at a specific temperature, while a supersaturated solution contains more solute than typically dissolvable at that temperature. Saturated solutions are stable and in equilibrium with the solute, whereas supersaturated solutions are unstable and can easily precipitate. A saturated solution example is dissolving table salt in water until no more salt can be dissolved. A supersaturated solution example is dissolving more sodium acetate in hot water and cooling it slowly, where the excess solute doesn't immediately precipitate but may do so if disturbed or a seed crystal is added.

Step by step solution

01

Define Saturated Solution

A saturated solution is a solution that contains the maximum amount of solute that can be dissolved in a given solvent at a specific temperature. In a saturated solution, the solute and the solvent are in equilibrium, meaning that the rate of solvation (solute dissolving) is equal to the rate of precipitation (solute coming out of solution).
02

Define Supersaturated Solution

A supersaturated solution is a solution that contains more solute than what would normally be possible to dissolve in the solvent at a specific temperature. In a supersaturated solution, the solute is not in equilibrium with the solvent, meaning that the precipitation rate is higher than the solvation rate. This makes the supersaturated solution unstable, and the excess solute can precipitate out of the solution spontaneously, or if disturbed.
03

Differentiate between Saturated and Supersaturated Solutions

The main difference between a saturated and supersaturated solution lies in the amount of solute that is dissolved. In a saturated solution, the maximum amount of solute is dissolved, while in a supersaturated solution, more than the maximum amount of solute is dissolved. This makes supersaturated solutions unstable, as they can easily precipitate, whereas saturated solutions are stable and in equilibrium with the solute.
04

Provide Examples of Saturated and Supersaturated Solutions

For instance, when you dissolve table salt (sodium chloride) in water, a saturated solution is formed when no more salt can be dissolved and undissolved salt settles to the bottom of the container. On the other hand, a supersaturated solution of sodium acetate can be formed by dissolving more sodium acetate in hot water and then slowly cooling the solution. In this supersaturated solution, the excess sodium acetate does not immediately precipitate but can do so if the solution is disturbed or a seed crystal is added.

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Most popular questions from this chapter

Uranium is found in Earth's crust as UO, and in an assortment of compounds containing UO \(_{2}^{n+}\) cations. How many moles of electrons are transferred in the conversion of one mole of \(\mathrm{UO}_{2}\) to each of the following species? In which of the conversions is uranium oxidized? (a) \(\mathrm{UO}_{2}\left(\mathrm{CO}_{3}\right)_{3}^{4-}(a q) ;\) (b) \(\mathrm{UO}_{2}\left(\mathrm{HPO}_{4}\right)_{2}^{2-}(a q)\)

Sodium fluoride is added to drinking water in many municipalities to protect teeth against cavities. The target of the fluoridation is hydroxyapatite, \(\mathrm{Ca}_{10}\left(\mathrm{PO}_{4}\right)_{6}(\mathrm{OH})_{2},\) a compound in tooth enamel. There is concern, however, that fluoride ions in water may contribute to skeletal fluorosis, an arthritis-like disease. a. Write a net ionic equation for the reaction between hydroxyapatite and sodium fluoride that produces fluorapatite, \(\mathrm{Ca}_{10}\left(\mathrm{PO}_{4}\right)_{6} \mathrm{F}_{2}\) b. The U.S. EPA currently restricts the concentration of \(\mathrm{F}^{-}\) in drinking water to \(4 \mathrm{mg} / \mathrm{L}\). Express this concentration of \(F^{-}\) in molarity. c. One study of skeletal fluorosis suggests that drinking water with a fluoride concentration of \(4 \mathrm{mg} / \mathrm{L}\) for 20 years raises the fluoride content in bone to \(6 \mathrm{mg} / \mathrm{g}\), a level at which a patient may experience stiff joints and other symptoms. How much fluoride (in milligrams) is present in a 100 mg sample of bone with this fluoride concentration?

According to the label on a bottle of concentrated hydrochloric acid, the contents are \(36.0 \%\) HCl by mass and have a density of \(1.18 \mathrm{g} / \mathrm{mL}\) a. What is the molarity of this concentrated HCl? b. What volume of it would you need to prepare \(0.250 \mathrm{L}\) of \(2.00 \mathrm{MHCl} ?\) c. What mass of sodium hydrogen carbonate would be needed to neutralize the spill if a bottle containing 1.75 L of this concentrated HCl dropped on a lab floor and broke open?

Give the formulas of two strong acids and two weak acids.

Calculate the mass of \(\mathrm{Mg} \mathrm{CO}_{3}\) precipitated by mixing \(10.0 \mathrm{mL}\) of a \(0.200 M \mathrm{Na}_{2} \mathrm{CO}_{3}\) solution with \(5.00 \mathrm{mL}\) of \(0.0500 M \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\) solution.
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