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Chapter 14: Problem 9

What does it mean to say that a solution is saturated?

Short Answer

Expert verified
A saturated solution is one where the maximum amount of solute has been dissolved in a given amount of solvent at a specific temperature and pressure. This means that the solution is in equilibrium with undissolved solute, with solute particles dissolving and depositing back into the solution at the same rate. For instance, when water cannot dissolve any more salt at a given temperature, any additional salt added will accumulate at the bottom of the beaker, indicating that the solution is saturated.

Step by step solution

01

Define Solutions

A solution is a homogeneous mixture of two or more substances where one substance, the solute, dissolves in another substance, the solvent. Common examples are sugar dissolved in water or salt dissolved in water.
02

Understand Solubility

Solubility is the maximum amount of solute that can be dissolved in a given amount of solvent at a specific temperature. Solubility can vary greatly depending on the solute and solvent involved, as well as the temperature and pressure.
03

Saturated Solutions

A solution is considered saturated when it has reached the maximum solubility and cannot dissolve any more solute at the given temperature and pressure. In other words, a saturated solution is a solution in equilibrium with undissolved solute. The solute particles are continuously dissolving and depositing back into the solution at the same rate.
04

Example

Consider a beaker of water with some salt being added to it. As the salt is added to the water, it dissolves and the solution becomes saltwater. If we continue adding salt, it will eventually reach a point where the water cannot dissolve any more salt. At this point, the salt will begin to accumulate at the bottom of the beaker instead of dissolving. This is an example of a saturated solution, as the water is holding the maximum amount of salt it can at the given temperature.
05

Effects of Temperature and Pressure

The solubility of most solid solutes in a solvent generally increases with increasing temperature. This means that at higher temperatures, a solution may be able to dissolve more solute and become saturated at a greater concentration of solute. Conversely, the solubility of gases in a solvent usually decreases with increasing temperature and increases with increasing pressure.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Solute and Solvent
In the world of chemistry, a solution involves two key components: the solute and the solvent.
A solute is the substance that is dissolved, and a solvent is the substance that does the dissolving.
Think of making lemonade: sugar is the solute, and the water is the solvent. Together, they create a sugary solution 鈥� yummy and homogeneous!
Solutes can be solids, liquids, or gases.
  • Examples of solid solutes include substances like salt or sugar.
  • Liquid solutes might be alcohol dissolved in water.
  • Gaseous solutes include carbon dioxide in carbonated beverages.
The solvent, on the other hand, is typically a liquid, though it can also be a solid or gas in some cases.
The role of the solvent is to keep the solute particles evenly distributed throughout the mixture.
Solubility
Solubility defines how well a solute can dissolve in a solvent.
It's about finding the magic point where no more solute will dissolve in the solvent.
This point can change based on various factors:
  • Temperature: Usually, the hotter the solvent, the more solute it can dissolve. Think of how well sugar dissolves in hot coffee compared to iced coffee!
  • Pressure: This primarily affects gaseous solutes. For instance, carbonated drinks remain fizzy under high pressure but lose carbonation when opened.
  • Nature of the solute and solvent: "Like dissolves like" is a common saying in chemistry, meaning that polar solvents dissolve polar solutes well, and nonpolar solvents dissolve nonpolar solutes well.
Understanding solubility helps us predict how substances will behave when mixed, aiding in processes like cooking, cleaning, and manufacturing.
Solution Equilibrium
When we talk about a saturated solution, we are dealing with a state of equilibrium between the solute and solvent.
At this point, the solution can hold no more solute at the specific conditions of temperature and pressure, and we say it's saturated.
But equilibrium means something interesting 鈥� it's not static!
In a saturated solution, an ongoing exchange occurs:
  • Solute particles are constantly dissolving into the solvent.
  • Simultaneously, solute particles also come out of solution and rejoin the undissolved solute.
This dynamic balance allows the concentration of dissolved solute to remain constant, despite ongoing dissolution and deposition processes.
The concept of solution equilibrium is fundamental in understanding chemical reactions, biological systems, and even in calculating concentrations in industrial processes.

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Most popular questions from this chapter

Calculate the number of moles of each ion present in each of the following solutions. a. \(10.2 \mathrm{mL}\) of \(0.451 \mathrm{M} \mathrm{AlCl}_{3}\) solution b. 5.51 L of \(0.103 M \mathrm{Na}_{3} \mathrm{PO}_{4}\) solution c. \(1.75 \mathrm{mL}\) of \(1.25 \mathrm{M} \mathrm{CuCl}_{2}\) solution d. \(25.2 \mathrm{mL}\) of \(0.00157 \mathrm{M} \mathrm{Ca}(\mathrm{OH})_{2}\) solution

When the volume of a given solution is doubled (by adding water), the new concentration of solute is _____the original concentration.

How many milliliters of \(0.105 M\) NaOH are required to neutralize exactly \(14.2 \mathrm{mL}\) of \(0.141 \mathrm{M} \mathrm{H}_{3} \mathrm{PO}_{4} ?\)

How many moles of each ion are present in \(11.7 \mathrm{mL}\) of \(0.102 M \mathrm{Na}_{3} \mathrm{PO}_{4}\) solution?

For each of the following, the mass of the solute is given, followed by the total volume of the solution prepared. Calculate the molarity. a. \(1.25 \mathrm{g} \mathrm{KNO}_{3} ; 115 \mathrm{mL}\) b. \(12.5 \mathrm{g} \mathrm{KNO}_{3} ; 1.15 \mathrm{L}\) c. \(1.25 \mathrm{mg} \mathrm{KNO}_{3} ; 1.15 \mathrm{mL}\) d. \(1.25 \mathrm{kg} \mathrm{KNO}_{3} ; 115 \mathrm{L}\)
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