Chemistry
Solutes Solvents and Solutions
Solutes are substances that are dissolved in a solvent to form a solution. The solvent is the substance in which the solute dissolves. Solutions are homogeneous mixtures of solutes and solvents. The solute concentration in a solution can vary, and solutions can be liquid, solid, or gas.
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10 Key excerpts on "Solutes Solvents and Solutions"
- Morris Hein, Scott Pattison, Susan Arena, Leo R. Best(Authors)
- 2014(Publication Date)
- Wiley(Publisher)
The solute is the component that is dissolved or is the least abundant component in the solution. The solvent is the dissolving agent or the most abundant component in the solution. For example, when salt is dissolved in water to form a solution, salt is the solute and water is the solvent. Complex solutions containing more than one solute and/or more than one solvent are common. The three states of matter—solid, liquid, and gas—give us nine different types of solu- tions: solid dissolved in solid, solid dissolved in liquid, solid dissolved in gas, liquid dissolved in liquid, and so on. Of these, the most common solutions are solid dissolved in liquid, liquid dissolved in liquid, gas dissolved in liquid, and gas dissolved in gas. Some common types of solutions are listed in Table 14.1. A true solution is one in which the particles of dissolved solute are molecular or ionic in size, generally in the range of 0.1 to 1 nm (10 -8 to 10 -7 cm). The properties of a true solution are as follows: 1. A mixture of two or more components—solute and solvent—is homogeneous and has a variable composition; that is, the ratio of solute to solvent can be varied. 2. The dissolved solute is molecular or ionic in size. 3. It is either colored or colorless and is usually transparent. 4. The solute remains uniformly distributed throughout the solution and will not settle out with time. 5. The solute can generally be separated from the solvent by purely physical means (for example, by evaporation). Let’s illustrate these properties using water solutions of sugar and of potassium permanganate. KEY TERMS solution solute solvent P R A C T I C E 1 4 . 1 Identify the solute and the solvent in each of these solutions: (a) air (b) seawater (c) carbonated water E X A M P L E 1 4 . 1 Consider two sugar solutions: solution A containing 10 g of sugar added to 100 mL of water and solution B containing 20 g of sugar added to 100 mL of water.
eBook - PDF- Morris Hein, Susan Arena, Cary Willard(Authors)
- 2016(Publication Date)
- Wiley(Publisher)
The solute is the component that is dissolved or is the least abundant component in the solution. The solvent is the dissolving agent or the most abundant component in the solution. For example, when salt is dissolved in water to form a solution, salt is the solute and water is the solvent. Complex solutions containing more than one solute and/or more than one solvent are common. The three states of matter—solid, liquid, and gas—give us nine different types of solutions: solid dissolved in solid, solid dissolved in liquid, solid dissolved in gas, liquid dissolved in liquid, and so on. Of these, the most common solutions are solid dissolved in liquid, liquid dissolved in liquid, gas dissolved in liquid, and gas dissolved in gas. Some common types of solutions are listed in TABLE 14.1. KEY TERMS solution solute solvent LEARNING OBJECTIVE TABLE 14.1 Common Types of Solutions Phase of solution Solute Solvent Example Gas gas gas air Liquid gas liquid soft drinks Liquid liquid liquid antifreeze Liquid solid liquid salt water Solid gas solid H 2 in Pt Solid solid solid brass A true solution is one in which the particles of dissolved solute are molecular or ionic in size, generally in the range of 0.1 to 1 nm ( 10 −8 to 10 −7 cm ). The properties of a true solution are as follows: 1. A mixture of two or more components—solute and solvent—is homogeneous and has a variable composition; that is, the ratio of solute to solvent can be varied. 2. The dissolved solute is molecular or ionic in size. 3. It is either colored or colorless and is usually transparent. 4. The solute remains uniformly distributed throughout the solution and will not settle out with time. 5. The solute can generally be separated from the solvent by purely physical means (for example, by evaporation). Let’s illustrate these properties using water solutions of sugar and of potassium permanganate.
eBook - PDFChemistry
An Industry-Based Introduction with CD-ROM
- John Kenkel, Paul B. Kelter, David S. Hage(Authors)
- 2000(Publication Date)
- CRC Press(Publisher)
There is only one solvent, but there can be more that one solute. The solvent is the component that is present in the greatest amount, or the component that has dissolved the other component(s) in itself. The solute (s) is (are) the component(s) present in the lesser amount or the substance(s) that has (have) dissolved in the solvent. For example, if you had a large bowl of pure, distilled water and you added a few crystals of salt plus a few crystals of sugar, and stirred this with a spoon, you would have a solution with water as the solvent and salt and sugar as the solutes. Chemistry Professionals at Work CPW Box 10.1 W HY S TUDY T HIS T OPIC ? f there are two activities that all those working in the chemical process industries have in common, it is the preparation of laboratory solutions and the measurement of the qualitative and quantitative characteristics of unknown sample solutions. A quality assurance technician working in the pharmaceutical formulations industry may, for example, measure the concentration of the active ingredient in a cough syrup, which is a solution. A biotechnician may be assigned to measure the lead content in urine, which is a solution. An environmental laboratory technician may prepare a series of solutions of nitrate to obtain data crucial to the determination of the nitrate in a drinking water sample, which is also a solution. A working knowledge of solution terminology, solution concentration, solution preparation, and solution properties is essential to these tasks. For Class Discussion: Each class member identifies a material that he/she thinks is a solution. Discuss each as a class and tell why each is or is not a solution. I Solutions 255 Sugar and salt are examples of compounds that dissolve in water quite readily at ordinary room temperatures. There are, however, many substances that do not readily dissolve in water. Examples are sand and sawdust. There is some dependence on temperature for this ability to dissolve.
eBook - PDFChemistry for Today
General, Organic, and Biochemistry
- Spencer Seager, Michael Slabaugh, Maren Hansen, , Spencer Seager, Spencer Seager, Michael Slabaugh, Maren Hansen(Authors)
- 2021(Publication Date)
- Cengage Learning EMEA(Publisher)
In addition, some solutions are colored. The component particles are in constant motion (remember the kinetic theory, Section 6.2) and do not settle under the influence of gravity. In most solutions, a larger amount of one substance is present compared to the other components. This most abundant substance in a solution is called the solvent, and any other components are called solutes. Most people normally think of solutions as liquids, but solutions in solid (see Figure 7.1) and gaseous forms are known as well. The state of a solution is often the same as the state of the solvent. This is illustrated in Table 7.1, which lists examples of solutions in various states. The original states of the solvents and solutes are given in parentheses. Solution formation takes place when one or more solutes dissolve in a solvent. solution A homogeneous mixture of two or more substances in which the components are present as atoms, molecules, or ions. solvent The substance present in a solution in the largest amount. solute One or more substances present in a solution in amounts less than that of the solvent. dissolving A term used to describe the process of solution formation when one or more solutes are dispersed in a solvent to form a homogeneous mixture. 5 Describe how to prepare solutions of specific concentration using pure solutes and solvent, or solutions of greater con- centration than the one desired. (Section 7.5) 6 Do stoichiometric calculations based on solution concentra- tions. (Section 7.6) 7 Do calculations based on the colligative solution properties of boiling point, freezing point, and osmotic pressure. (Section 7.7) 8 Describe the characteristics of colloids. (Section 7.8) 9 Describe the process of dialysis, and compare it to the process of osmosis. (Section 7.9) FIGURE 7.1 Stainless steel is a solid solution of several metals.
- Frederick Bettelheim, William Brown, Mary Campbell, Shawn Farrell(Authors)
- 2019(Publication Date)
- Cengage Learning EMEA(Publisher)
These mixtures are classified as suspensions. We will deal with such systems in Section 6.7. Although mixtures can contain many components, we will generally re-strict our discussion to two-component systems, with the understanding that everything we say can be extended to multicomponent systems. © Sebastian Kaulitzki/Shutterstock.com Human blood cells in an isotonic solution. Copyright 2020 Cengage Learning. All Rights Reserved. May not be copied, scanned, or duplicated, in whole or in part. Due to electronic rights, some third party content may be suppressed from the eBook and/or eChapter(s). Editorial review has deemed that any suppressed content does not materially affect the overall learning experience. Cengage Learning reserves the right to remove additional content at any time if subsequent rights restrictions require it. When a solution consists of a solid or a gas dissolved in a liquid, the liq-uid is called the solvent and the solid or gas is called the solute. A solvent may have several solutes dissolved in it, even of different types. A common example is spring water, in which gases (carbon dioxide and oxygen) and solids (salts) are dissolved in the solvent, water. When one liquid is dissolved in another, a question may arise regarding which is the solvent and which is the solute. The one present in the greater amount is usually called the solvent. We normally do not use the terms “solute” and “solvent” when talking about solutions of gases in gases or solids in solids. 6.3 The Distinguishing Characteristics of Solutions The following are some properties of solutions: 1. The distribution of particles in a solution is uniform. Every part of the solution has exactly the same composition and prop-erties as every other part. A solution with these characteristics is called homogeneous. As a consequence, we cannot usually tell a solution from a pure solvent simply by looking at it.
eBook - PDF- Allan Blackman, Steven E. Bottle, Siegbert Schmid, Mauro Mocerino, Uta Wille(Authors)
- 2022(Publication Date)
- Wiley(Publisher)
In this chapter, we will focus on the energetics of formation of solutions and the quantification of physical properties of solutions. FIGURE 10.2 A saturated solution. In a saturated solution, a dynamic equilibrium exists between the undissolved solute and the dissolved solute in the solution. A solution can be defined as a homogeneous mixture of two or more pure substances (‘homogeneous’ means that all regions of the solution have exactly the same composition). Despite the fact that we often think of a solution as involving some type of liquid, we can have gaseous solutions com- prising two or more gases (e.g. air) and even solid solutions comprising two or more solids (e.g. alloys such as brass and solder) in addition to the ‘usual’ solutions containing a gas, liquid or solid dissolved in a liquid. In the case of liquid solutions, we call the liquid the solvent, while the dissolved substance is called the solute; the solute is present in smaller amounts than the solvent. A solute is said to be soluble in a particular solvent if it dissolves completely in that solvent at the specified temperature. We define the solubility of the solute in a particular solvent as the maximum amount of the solute that dissolves completely in a given mass or volume of the solvent at a particular temperature, T, and a particular pressure, p. A saturated solution is one in which no more solute will dissolve. The most common type of saturated solution we will encounter is that illustrated in figure 10.2, in which excess solid solute is in equilibrium with its dissolved form. The process of dissolving a solute in a solvent to give a homogeneous solution is called dissolution. We therefore talk of the dissolution of a solute in a particular solvent. 10.2 Gaseous solutions LEARNING OBJECTIVE 10.2 Describe why gases mix spontaneously. We will begin our investigation of solutions by looking at mixing two gases to form a gaseous solution.
eBook - PDF- David A. Ucko(Author)
- 2013(Publication Date)
- Academic Press(Publisher)
The solubility of most solids in water increases with increasing temperature. 13.4 A solution is saturated when it contains the maximum possible amount of dissolved solute under normal conditions at a particular temperature. At this point, the rate at which solute dissolves exactly equals the rate at which solute returns from the solution. 13.5 Liquids that mix completely in any proportion are said to be miscible. Immiscible liquids do not mix. All gases can mix to form solutions. The solubility of a gas in a liquid increases with increasing pressure but decreases with increasing temperature. 13.6 Solvents serve as a medium in which substances react and form products. Solvents are also used as cleaners, to deposit coatings, and in industrial processing. 13.7 The concentration of a solution describes the amount of solute present in any given quantity of solvent or solution. Concentration can be expressed as a percentage based on the ratios of solute and solution in terms of weight to volume, weight to weight, or volume to volume. 13.8 Molarity is defined as the number of moles of solute per liter of solution. Two solutions with the same molarity contain equal numbers of moles of solute per liter. However, they generally contain different masses of solute. 13.9 Solutions are often prepared by diluting a portion of an existing stock solution. Dilution calculations can be made using the relationship Mi x Vi = M 2 x V 2 , or by using the conversion factor method. 13.10 When a reaction takes place in aqueous solution, some of the reactants and products are often present as ions. The net ionic equation expresses the reaction in simplified form. Spectator ions, those that do not participate in the reaction, do not appear in a net ionic equation. 13.11 Colligative properties are properties that depend only on the number of solute particles in a solution. Colligative properties include 440
- Jan Rydberg(Author)
- 2004(Publication Date)
- CRC Press(Publisher)
The totality of these interactions is called the solvation of the solute in the particular solvent. When the solvent happens to be water, the term used is hydration. The solvation process has certain consequences pertaining to the energy, the volume, the fluidity, the electrical conductivity, and the spectroscopic properties of the solute-solvent system. The apparent molar properties of the solute ascribe to the solute itself the entire change in the properties of the system that occur when 1 mol of solute is added to an infinite amount of solution of specified composition. The solvent is treated in the calculation of the apparent molar quantities of the solute as if it had the properties of the pure solvent, present at its nominal amount in the solution. The magnitudes of quantities, such as the apparent molar volume or heat content, do convey some information on the system. However, it must be realized that both the solute and the solvent are affected by the solvation process, and more useful information is gained when the changes occurring in both are taken into account. 2.3.1 Interactions at the Molecular Scale The solvation process can be envisioned as occurring in several stages, although only the sum of the stage contributions to the overall process is measurable. First, a cavity must be created in the solvent to accommodate the solute. Then the solute is placed in the cavity and permitted to interact with its nearest neighbors, eventually forming coordinate bonds with some of them, forming a new entity, the solvated solute. Finally, this entity may interact further with its surroundings, by orienting solvent molecules, by the formation or disruption of hydrogen bonds, or by other interactions. If the solute is charged (i.e., if it is an ion), it will orient the dipoles of a polar solvent by its electrical field.
eBook - PDF- Young, William Vining, Roberta Day, Beatrice Botch(Authors)
- 2017(Publication Date)
- Cengage Learning EMEA(Publisher)
● For most solid–liquid solutions, temperature and solubility are directly related (14.3b). ● For most solids, solubility in water is related to the enthalpy of dissolution for the solid (14.3b). 14.4 Colligative Properties ● Changes in the properties of a solvent are directly related to the concentration of sol-ute particles in the solvent (14.4). ● Osmotic pressure, the result of an imbalance in the flow of solvent between a solu-tion with low solute concentration and a solution with a higher solute concentration, is directly related to the concentration of solute particles and the temperature of the solution (14.4a). ● Application of a pressure greater than osmotic pressure forces a solution with high solute concentration through a semipermeable membrane and can be used to produce pure solvent (14.4a). ● Adding a nonvolatile solute to a volatile solvent decreases the vapor pressure of the solvent, a relationship described mathematically by Raoult’s law (14.4b). ● The decrease in vapor pressure for a solvent is directly related to the concentration of solute particles in the solution (14.4b). ● Only ideal solutions follow Raoult’s law. When a solution contains a volatile solute or a solute that interacts with the solvent, deviations occur (14.4b). ● The boiling point of a solvent in a solution is always higher than that of the pure sol-vent (14.4c). ● The increase in boiling point for a solvent is directly related to the concentration of solute particles in the solution (14.4c). ● The freezing point of a solvent in a solution is always lower than that of the pure sol-vent (14.4d). ● The decrease in freezing point for a solvent is directly related to the concentration of solute particles in the solution (14.4d). 14.5 Other Types of Mixtures ● Some important alloys—mixtures of metals—are steel, brass, and bronze (14.5a). ● Colloids consist of uniform distributions of one substance in another. They are very common and include emulsions and aerosols (14.5b).
eBook - PDF- Stanley E. Manahan(Author)
- 2009(Publication Date)
- CRC Press(Publisher)
7. SOLUTIONS AND SOLVENTS 7. SOLUTIONS AND SOLVENTS 7.1. WHAT ARE SOLUTIONS? WHY ARE THEY IMPORTANT? 7.1. WHAT ARE SOLUTIONS? WHY ARE THEY IMPORTANT? To help understand solutions, consider a simple experiment. Run some water To help understand solutions, consider a simple experiment. Run some water from a faucet into a glass and examine it. Depending on the condition of the local from a faucet into a glass and examine it. Depending on the condition of the local water supply, it will probably appear clear. If tasted, it will probably not have any water supply, it will probably appear clear. If tasted, it will probably not have any particularly strong flavors. Now, add a teaspoon of sugar and stir the contents of the particularly strong flavors. Now, add a teaspoon of sugar and stir the contents of the glass; you will notice that the sugar will begin to disappear, and the water around the glass; you will notice that the sugar will begin to disappear, and the water around the sugar will start to appear cloudy or streaked. With continued stirring, the sugar will sugar will start to appear cloudy or streaked. With continued stirring, the sugar will seem to disappear completely, and the water will look as clear as it did when it came seem to disappear completely, and the water will look as clear as it did when it came out of the tap. However, it will have a sweet taste; some of its properties have there-out of the tap. However, it will have a sweet taste; some of its properties have there-fore been changed by the addition of sugar. fore been changed by the addition of sugar. This experiment illustrates several important characteristics of chemicals and This experiment illustrates several important characteristics of chemicals and how they are used. Sugar how they are used. Sugar dissolves dissolves in water; when this happens, a in water; when this happens, a solution solution is is formed. The sugar molecules were originally contained in hard, rigid sugar crystals.
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