Since Ag ClO3 is a silver chlorate, and rule 3 comes before rule 4, it supersedes it. This compound is soluble. None of the above silver is soluble. In rule 4, it states that silver salts Ag are insoluble, with silver nitrate, AgNO3, as one exception.
As we see from our solubility rules, some substances are very soluble, while some are insoluble or have low solubility. Let's take a look at how solubility works to better understand the solubility rules. Whether or not a substance is soluble, and to what degree, depends on a variety of factors.
Solutes typically will dissolve best in solvents that have the most molecular similarities. Polarity is a major factor in a substance's solubility. If a molecule does not have this ionic makeup, it is considered nonpolar. Generally, solutes are soluble in solvents that are most similar to them molecularly.
Polar solutes will dissolve better in polar solvents, and non-polar solutes will dissolve better in non-polar solvents. For example, sugar is a polar solute, and absorbs very well in water. However, sugar would have a low solubility in a nonpolar liquid like vegetable oil.
In general, solutes will also be more soluble if the molecules in the solute are smaller than the ones in the solvent. Other factors that affect solubility are pressure and temperature. In some solvents, when heated the molecules vibrate faster and are able to break apart the solute.
Pressure is mainly a factor when a gas substance is involved, and has little to no effect on liquid substances. The rate of solution refers to how quickly a substance dissolves, and is separate from solubility. Rate should not be factored into the solubility of a substance. This can often be confusing when first learning about solubility, since in a visual example, watching something dissolve quickly can feel like an affirmation of its ability to dissolve. However, the process of solubility is unique, and the rate at which it dissolves is not factored into the equation.
When a solute is mixed with a solvent, there are three possible outcomes: If the solution has less solute than the maximum amount it is able to dissolve the solubility , it is a dilute solution. If the amount of solute is exactly the same as the solubility it is saturated.
If there is more solute than is able to be dissolved, the excess separates from the solution and forms a precipitate. A solution is considered saturated when adding additional solute does not increase the concentration of the solution. Additionally, a solution is miscible when it can be mixed together at any ratio- this mainly applies to liquids, like ethanol, C2H5OH, and water, H2O.
Knowing and following the solubility rules is the best way to predict the outcome of any given solution. If we know that a substance is insoluble, it is likely that it would have excess solute, thus forming a precipitate. However, compounds that we know to be highly soluble, like salt, are likely to form solutions at various ratios; in this case, we will be able to determine how much solute and solvent is needed to form each solution, and if it's possible to form one at all. 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. Most hydroxide salts are only slightly soluble.
Hydroxide salts of Group I elements are soluble. Arsenic, antimony, bismuth, and lead sulfides are also insoluble. Carbonates are frequently insoluble. Carbonates, hydroxides, sulfates, phosphates, and heavy metal salts are often insoluble. Boundless vets and curates high-quality, openly licensed content from around the Internet.
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.
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