A saturated solution is one that contains the maximum amount of solute capable of being dissolved, whereas unsaturated solutions contain less than the maximum amount of solute capable of being dissolved. Because carbonated water is saturated with carbon, it emits carbon through bubbles. Sand in water is an example of an unsaturated. Show
Saturated Solutions
The saturation point of any liquid is determined by the type of the material and the temperature. A saturated solution is one in which the quantity of dissolved solute equals the saturation point of the solvent. A solvent can dissolve some particular types of solutes in it. The maximum amount of solute that can be dissolved in a solvent at a specified temperature can be termed as a saturated solution. A solution cannot dissolve any more solute further upon reaching saturation. The undissolved substances remain at the bottom. The point at which the solute stops dissolving in the solvent is termed the saturation point. Following are the examples of Saturated Solutions:
Unsaturated SolutionsA solute must be added to a solvent in order for a solution to form. At first, the solute dissolves in a solvent and forms a homogeneous solution. A solution in which solutes dissolve is referred to as an unsaturated solution. A solution is made up of two types of particles: solutes and solvents. Water is commonly used as a solvent (which is one of the reasons why water is also called the universal solvent).
As a result, all solutions are considered to be largely unsaturated in nature before being transformed into saturated solutions by adding solute to them. The amount of solute that is contained in lesser amounts than the maximum value, that is before the solution reaches the saturation level is called an unsaturated solution. No remaining substances leave at the bottom, that is, all the solute is dissolved in the solvent. An unsaturated solution is basically a chemical solution that has a solute concentration lesser than its corresponding equilibrium solubility. Following are the examples of Unsaturated Solutions:
Interconversion of Saturated and Unsaturated SolutionSaturated solution on heating becomes unsaturated whereas an unsaturated solution becomes saturated upon cooling. On heating the saturated solution, the solubility of that particular solute increases in the given solvent. As a result of this, more solute can be dissolved into the solvent. However, in the case of cooling a solution, the solute particles which were initially dissolved in the solvent separate out as crystals. Solubility
The maximum amount of a solute that can be dissolved in 100 gm of a solvent. Different solutes possess varying different solubilities. Solubility increases with an increase in temperature. In the case of saturated solutions, the solute concentration is equivalent to the equilibrium solubility. The solubility of a substance depends on the solvent. It is observed that sugar dissolves in water but not in oil. Effect of Temperature and Pressure on Solubility
Concentration of SolutionThe quantity of solute present in a specified quantity of the solvent can be termed as the concentration of the solution. It is measured as a fraction of the amount of solute dissolved in a given mass or volume of a solvent.
Mathematically,
Also,
Sample ProblemsProblem 1: A solution is formed by dissolving 20g of sodium chloride in 180 g of water as solvent. Compute the concentration of the solution. Solution:
Problem 2: How to identify whether the solution is saturated or not? Solution:
Problem 3: How can you create a saturated solution? Solution:
Problem 4: Give some outdoor examples of saturated solutions. Solution:
Problem 5: Give one example to show a solution that can be unsaturated, saturated, and supersaturated at different intervals of time. Solution:
In order to continue enjoying our site, we ask that you confirm your identity as a human. Thank you very much for your cooperation. There are many ways to measure the amount of solute present in a solution. Each method is useful for a different purpose in chemistry, so we're unfortunately stuck with the task of learning all of them. Without further ado, here they are: Qualitative ConcentrationsThe amount of solute present in a solution can be described without numbers by one of the following terms:
It's easy to tell if a solution is unsaturated, saturated, or supersaturated by adding a very small amount of solute. If the solution is unsaturated, the solute will dissolve. If the solution is saturated, it won't. If the solution is supersaturated, crystals will very quickly form around the solute you've added. Molarity (M)
When reading the definitions of the following methods of determining concentration, pay close attention to whether the volume component asks for the weight or volume "of solution" or weight or volume "of solvent." When the weight or volume of the solution is specified, it means that you're interested in the amount of solution present after the solute has been added. If the weight or volume of the solvent is specified, this means that you're interested in the amount of solvent before the solute has been added. Molarity is probably the most commonly used way of measuring concentration and is defined as the number of moles of solute per liters of solution.
Problem 1: What is the molarity of a solution with a volume of 3.0 liters that contains 120 grams of acetic acid (C2H3O2H)? Let's say that we have made a solution by adding water to 40 grams (1.0 mole) of sodium hydroxide until the final volume of the solution is one liter (to review mole calculations, head back to The Mole). Because we have one mole of solute in one liter of solution, the molarity is equal to (1 mole)/(1 liter) = 1 M. We refer to a solution with a molarity of one as being a "one molar" solution. Molality (m)Molality is defined as the number of moles of solute per kilogram of solvent. For example, if we were to add two kilograms of water to 4 moles of sugar, the molality would be equal to 4 moles/2 kilograms = 2 m ("two molal"). When doing calculations with molality, note that because the density of water is 1.0 g/mL under standard conditions, the number of kilograms of water is equal to the number of liters of water. Normality (N)The normality of a solution is defined as the number of moles of a reactive species, usually referred to as "equivalents" per liter of solution. The use of "equivalents" will depend on the reaction being performed, so some knowledge of the specific chemical process in a reaction is necessary before computing normality. At least, that's the "normal" way of solving this problem. (I couldn't resist.) Mole Fraction ()
Problem 2: What is the mole fraction of water in a solution made by mixing 4.5 moles of isopropanol with 15.0 moles of water? The mole fraction is defined as the number of moles of one component in a solution divided by the total number of moles of all components in the mixture. In equation form, we can express the mole fraction of one component in a solution as being:
where A refers to the first component, B refers to the second component, and C refers to the third component. As the "…" indicates, this calculation can be extended to include any number of components in the mixture. Parts Per Million (ppm) and Parts Per Billion (ppb)Both parts per million and parts per billion are units of concentration most frequently used in environmental analysis. Because the solvent used is most frequently water, the concentration of a solution in ppm can be found by dividing the number of mg (0.001 g) of solute by the number of liters of water. Parts per billion can be determined by dividing the number of g (10-6 g) of solute by the number of liters of water. A Quick Summary of Units of ConcentrationThe following table includes all of the units of concentration we've mentioned in this section, as well as how to find them.
Excerpted from The Complete Idiot's Guide to Chemistry © 2003 by Ian Guch. All rights reserved including the right of reproduction in whole or in part in any form. Used by arrangement with Alpha Books, a member of Penguin Group (USA) Inc. To order this book direct from the publisher, visit the Penguin USA website or call 1-800-253-6476. You can also purchase this book at Amazon.com and Barnes & Noble. |