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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

Silver dissolves in sulfuric acid to form silver sulfate and \(\mathrm{H}_{2},\) but gold does not dissolve in sulfuric acid to form gold sulfate. Which of the two metals is the better reducing agent?

The water-soluble gas \(\mathrm{ClO}_{2}\) is known as an oxidative biocide. It destroys bacteria by oxidizing their cell walls and viruses by attacking their viral envelopes. \(\mathrm{ClO}_{2}\) may be prepared for use as a decontaminating agent from several different starting materials in slightly acidic solutions. Complete and balance the following chemical reactions for the synthesis of \(\mathrm{ClO}_{2}\) a. \(\mathrm{ClO}_{3}^{-}(a q)+\mathrm{SO}_{2}(g) \rightarrow \mathrm{ClO}_{2}(g)+\mathrm{SO}_{4}^{2-}(a q)\) b. \(\mathrm{ClO}_{3}^{-}(a q)+\mathrm{Cl}^{-}(a q) \rightarrow \mathrm{ClO}_{2}(g)+\mathrm{Cl}_{2}(g)\) c. \(\mathrm{ClO}_{3}^{-}(a q)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{ClO}_{2}(g)+\mathrm{O}_{2}(g)\)

Permanganate ion \(\left(\mathrm{MnO}_{4}^{-}\right)\) is used in water purification to remove oxidizable substances. Complete and balance the following reactions for the removal of sulfide, cyanide, and sulfite. Assume that reaction conditions are basic: a. \(\mathrm{MnO}_{4}^{-}(a q)+\mathrm{S}^{2-}(a q) \rightarrow \mathrm{MnS}(s)+\mathrm{S}_{8}(s)\) b. \(\mathrm{MnO}_{4}^{-}(a q)+\mathrm{CN}^{-}(a q) \rightarrow \mathrm{MnO}_{2}(s)+\mathrm{CNO}^{-}(a q)\) c. \(\operatorname{Mn} \mathrm{O}_{4}^{-}(a q)+\mathrm{SO}_{3}^{2-}(a q) \rightarrow \mathrm{MnO}_{2}(s)+\mathrm{SO}_{4}^{2-}(a q)\)

What is the difference between a strong base and a weak base?

Calcium nitrate is soluble, but calcium phosphate is not. Explain this difference in solubility
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