All compounds that contain a nitrate ion (NO3-) or acetate ion (C2H3O2-) are soluble.
This is a rule for solubility. Why aren't they soluable. what does charge density for acetate ion have to do with it?
Here is an article I found on the Internet that addresses your question.
http://www.pubmedcentral.nih.gov/articlerender.fcgi?artid=1184297
By the way, not the correct spelling of soluble.
The statement you mentioned is actually a rule stating that most compounds containing nitrate ion (NO3-) or acetate ion (C2H3O2-) are soluble in water. However, there are some exceptions to this rule, especially when we consider the charge density of the ions.
Charge density refers to the ratio of the charge of an ion to its volume. In the case of acetate ion (C2H3O2-), the charge is spread over a larger volume due to the presence of the two carbon atoms and three oxygen atoms. This results in a lower charge density compared to other ions with similar charge, such as chloride ion (Cl-).
When an ion with high charge density dissolves in water, it tends to interact more strongly with the water molecules, forming strong hydration shells around it. This hydration helps to stabilize and solvate the ion, making it more soluble in water.
On the other hand, an ion with low charge density, like the acetate ion, can experience weaker interactions with water molecules during the process of dissolution. This results in a lower solubility as compared to ions with higher charge density.
Additionally, factors like the presence of other ions in a compound, the nature of the solvent, and temperature can also influence the solubility of a compound.
So, while most compounds containing nitrate or acetate ions are soluble, there are exceptions due to the charge density of the ions and other factors affecting solubility.