This particular resource used the following sources:. Skip to main content. Aqueous Reactions. Search for:. Key Points Solubility is the relative ability of a solute to dissolve into a solvent. Several factors affect the solubility of a given solute in a given solvent. Temperature often plays the largest role, although pressure can have a significant effect for gases.
Show Sources Boundless vets and curates high-quality, openly licensed content from around the Internet. Licenses and Attributions. CC licensed content, Shared previously. Considering NaNO 3 , Rule 3 states that nitrates tend to be soluble.
A precipitate of this compound will not form. Next, consider Ag 2 S. According to Rule 5, that sulfides tend to be insoluble. Therefore, because of this compound, a precipitate will form in the course of this reaction. The first product, KOH, is an example of two rules contradicting each other.
Although Rule 5 says that hydroxides tend to be insoluble, Rule 1 states that salts of alkali metal cations tend to be soluble, and Rule 1 precedes Rule 5. Therefore, this compound will not contribute to any precipitation being formed. The second product, Na 2 CrO 4 , also adheres to Rule 1, which states that salts of alkali metals tend to be soluble. Solubility Effects on Reactions Depending on the solubility of a solute, there are three possible results: 1 if the solution has less solute than the maximum amount that it is able to dissolve its solubility , it is a dilute solution; 2 if the amount of solute is exactly the same amount as its solubility, it is saturated; 3 if there is more solute than is able to be dissolved, the excess solute separates from the solution.
Solubility Rules The following are the solubility rules for common ionic solids. There are few exceptions to this rule. Salts containing nitrate ion NO 3 - are generally soluble.
Salts containing Cl - , Br - , or I - are generally soluble. Most silver salts are insoluble. Most sulfate salts are soluble. Steps 1 and 2 are endothermic processes because energy is required to break up molecular interactions these interactions could be hydrogen bonds, dipole-dipole interactions, dispersion forces, etc.
The enthalpy change, and thus, the outcome of the solution process depends on the attraction of solute to solvent. There are no polar C-H or O-H bonds on acetone; therefore, it cannot form hydrogen bonds with other acetone molecules. The intramolecular forces consist of dispersion forces. Water, on the other hand, has two polar O-H bonds.
The slightly positive charge on each hydrogen can attract slightly negative oxygen atoms on other water molecules, forming hydrogen bonds. If acetone is added to water, acetone would completely dissolve. There would be no change in the type or amount of hydrogen bonding that would take place from the perspective of water. This results in a more favourable solute-solvent interaction, so acetone goes into solution. Solubility by reaction takes advantage of the presence of a functional group and the properties associated with it.
Organic acids and bases may reaction to form water soluble salts, thus forcing the compound into solution.
0コメント