Solubility The maximum amount of solute that

Solubility The maximum amount of solute that dissolves in 100 g of water at a certain temperature. 

Single bond. Two atoms are held together by one electron pair. (9.4) Solubility. The maximum amount of solute that can be dissolved in a given quantity of solvent at a specific temperature. (16.6)... 

A solution is saturated if it contains the maximum amount of solute that can possibly be dissolved in a solvent at the existing temperature and pressure conditions. If a solution is saturated, it need not be concentrated. Concentrated refers to the ratio of solute to solvent. A solution is concentrated if it contains a high ratio of solute to solvent. A solution is dilute if it contains a low ratio of solute to solvent. A solution of ammonia gas dissolved in water can be highly concentrated but not saturated. Ammonia gas dissolves easily in water. Barium hydroxide is slightly soluble. A saturated solution of barium hydroxide is very dilute. 

If you have ever added so much sugar to a sweetened beverage that sugar crystals accumulated on the container s bottom, then you know that only a limited amount of solute can dissolve in a solvent at a given set of conditions. In fact, every solute has a characteristic solubility. Solubility refers to the maximum amount of solute that will dissolve in a given amount of solvent at a specified temperature and pressure. As you can see from Table 15-2, solubility is usually expressed in grams of solute per 100 g of solvent. 

How can we predict whether a precipitate will form when a compound is added to a solntion or when two solutions are mixed It depends on the solubility of the solute, which is defined as the maximum amount of solute that will dissolve in a given quantity of solvent at a specific temperature. Chemists refer to substances as soluble, slightly soluble, or insoluble in a qualitative sense. A substance is said to be soluble if a fair amount of it visibly dissolves when added to water. If not, the substance is described as slightly soluble or insoluble. All ionic compounds are strong electrolytes, but they are not equally soluble. 

Solubility is defined as the maximum amount of solute that dissolves in a given amount of solvent at a specified temperature. Polar molecules are most soluble in polar solvents, whereas nonpolar molecules are most soluble in nonpolar solvents. This is the rule of "like dissolves like." Substances of similar polarity are mutually soluble, and large differences in polarity lead to insolubility. 

Solubility is a measure of the maximum amount of solute that can be dissolved in a given amount of solvent to form a stable solution. The composition of many solutions cannot be varied continuously because there are certain fixed limits imposed by the nature of the substances involved. Solid salt and sugar can be mixed in any desired proportions, but unlimited quantities of sugar (or salt) cannot be dissolved in a given amount of water however, up to the solubility limit, solutions can be produced in any desired proportion. 

The maximum amount of solute that will dissolve in a standard quantity of solvent is termed the solubility of the solute. Exceeding the solubility of the solute wiU not resnlt in any additional amount of solute dissolved. The solubility of various solutes is affected both by tanperature and pressure. Most solid solutes increase their solubilities as temperature increases (Fignre 3.7.3), whereas the solubilities of gases decrease as tanperature increases There is less oxygen in warm water than in cool water, so aquatic species may sometimes asphyxiate in warm water. 

A saturated solution contains the maximum amount of solute that can dissolve at a given temperature. Any excess undissolved solute is in equilibrium with dissolved solute. Because of the equilibrium nature of solubility, most solids are more soluble in water at higher temperatures, all gases are less soluble in water at higher temperatures, and the solubility of a gas is directly proportional to its pressure (Henry s law). Section 13.3)... 

Most liquid/solid solutions do not make solutions in infinite ratios. Typically, there is a limit to how much solid can be dissolved in a given amount of liquid. At this limit, the solution is said to be saturated. The solubility represents the amount of solid that is dissolved in order to make a saturated solution, and is given in a wide variety of units. [A common unit for solubility is (grams of solute)/(100 mL of solvent).] Most of the solutions we work with are unsaturated, having less than the maximum amount of solute that can dissolve. Occasionally, it is possible to dissolve more than the maximum. This is typically done by heating the solvent, dissolving more solute, then cooling the solution carefully so that the excess solute does not precipitate. These are supersaturated solutions. However, they are not thermodynamically stable. 

The term solubility describes the amount of a solute that can dissolve in a given amount of solvent. Many factors, such as type of solute, type of solvent, and temperature, affect the solubility of a solute. Solubility, usually expressed in grams of solute in 100 g of solvent, is the maximum amount of solute that dissolves at a certain temperature. If a solute readily dissolves when added to the solvent, the solution does not contain the maximum amount of solute. We call this solution an unsaturated solution. 

Solubility is the maximum amount of solute that will dissolve in a given cimount of a solvent at a specified temperature. You know from your own experiences, I m sure, that there s a limit to how much solute you can dissolve in a given amount of solvent. Most people have been guilty of putting far too much sugar in iced tea. No matter how much you stir, some undissolved sugar stays at the bottom of the glass. 

Solubility is defined as the maximum amount of solute that will dissolve in a given quantity of solvent at a specific temperature. Not all ionic compounds dissolve in water. Whether or not an ionic compound is water soluble depends on the relative magnitudes of the water molecules attraction to the ions, and the ions attraction for each other. We will learn more about the magnitudes of attractive forces in ionic compounds in Chapter 8, but for now it is useful to learn some guidelines that enable us to predict the solubility of ionic compounds. Table 4.2 lists groups of compounds that are soluble and shows the insoluble exceptions. Table 4.3 lists groups of compounds that are insoluble and shows the soluble exceptions. 

The concentration of solute that remains in the liquid solution is dependent on solid-liquid equilibrium. Phase diagrams can be of many types, depending on the system. The maximum amount of solute that can be dissolved in a given volume of solvent at equilibrium and at a given temperature is called solubility. While it is typical for solubility to increase with increasing temperature, that is not always the case for example, see Ce CSO jj, as seen in Figure 7.10. 

There are limits as to how much solute may be dispersed or dissolved in a given amount of solvent. This limit is the solubility and is defined as the maximum weight of solute that dissolves in 100 g of a given solvent at a given temperature. For example, sucrose (or table sugar) is soluble to the extent of 203.9 g per 100 g of water at 20°C. This means that if you have 100 g of water, you can dissolve up to 203.9 g of table sugar, but no more, in that quantity of water at 20°C. If more is added, the extra amount sinks to the bottom undissolved. A solution in this state is referred to as saturated. A solution with less than the maximum at the same temperature is called unsaturated. Solubility also varies with temperature (Fig. 17.1). 

The solubilities of ionic salts have wide range. For instance, in contrast to silver perchlorate (AgC104), which has a solubility of 55.7 g per 100 g of water, only 0.00018 g of silver chloride (AgCl) can dissolve in 100 g of water. If the maximum amount of solute dissolved in 100 g of water is less than 0.1 g, this solute is said to be insoluble. The solute that has a solubility range from 0.1 g to 1 g is called slightly soluble. If the amount of solute is more than 1 g, then it is soluble. Silver perchlorate is a soluble compound but silver chloride is an insoluble compound in water. It is not necessary to memorize the solubilities of substances. Solubility tables (e.g.,Table 2) help you determine whether a substance is soluble, insoluble, or slightly soluble in water. 

Protein solubility is a thermodynamic characteristic of the protein/solvent system dehned as the concentration of soluble protein in equilibrium with the solid phase at a given pH, temperature, and solvent composition (Flynn, 1984 Arakawa and Timashelf, 1985 Middaugh and Volkin, 1992). For practical purposes, solubility of proteins can be dehned as the maximum amount of protein that remains in a visibly clear solution (i.e. does not show protein precipitates, crystals, gels, or hazy soluble aggregates), or does not sediment at 30,000 g centrifugation for 30 min (Schein, 1990 Ducruix and Reis-Kautt, 1990). 

When we say that one substance is soluble in another, we mean that they can be mixed to a significant degree. More specifically, chemists describe the solubility of a substance as the maximum amount of it that can be dissolved in a given amount of solvent at a particular temperature. This property is often described in terms of the maximum number of grams of solute that will dissolve in 100 milliliters (or 100 grams) of solvent. For example, the water solubility of calcium nitrate is 121.2 g Ca(N03)2 per 100 mL water at 25 °C. This means that when calcium nitrate is added steadily to 100 mL of water at 25 °C, it will dissolve until 121.2 g Ca(N03)2 have been added. If more Ca(N03)2 is added to the solution, it will remain in the solid form. 

Tabulated values of solubilities of ionic salts refer to the maximum amount of solid that will dissolve in a given mass of water to give a saturated solution. 

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