Rule 4 states that bromides are usually soluble, but Rule 3 states that salts of silver are insoluble. Because Rule 3 precedes Rule 4, the compound is insoluble and will form a precipitate.
The products of the reaction must be examined; if either of the substances formed in the reaction is insoluble, a precipitate will form.
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. What factors affect solubility of ionic compounds? What factors affect the solubility of gases in liquids?
What factors affect the solubility of a solid? How can I calculate solubility of potassium nitrate? What does the solubility of KNO3 depend on? How can I calculate the solubility of solute in a solution? How is solubility affected by polymer chain structure?
Does solubility differ from molar solubility? See all questions in Factors Affecting Solubility. The solubility of gases displays the opposite relationship with temperature; that is, as temperature increases, gas solubility tends to decrease.
In a chart of solubility vs. Pressure has a negligible effect on the solubility of solid and liquid solutes, but it has a strong effect on solutions with gaseous solutes. This is apparent every time you open a soda can; the hissing sound from the can is due to the fact that its contents are under pressure, which ensures that the soda stays carbonated that is to say, that the carbon dioxide stays dissolved in solution.
The takeaway from this is that the solubility of gases tends to correlate with increasing pressure. For example, a polar solute such as sugar is very soluble in polar water, less soluble in moderately polar methanol, and practically insoluble in non-polar solvents such as benzene.
In contrast, a non-polar solute such as naphthalene is insoluble in water, moderately soluble in methanol, and highly soluble in benzene. The solubility chart shows the solubility of many salts. Salts of alkali metals and ammonium , as well as those of nitrate and acetate, are always soluble. Carbonates, hydroxides, sulfates, phosphates, and heavy metal salts are often insoluble.
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