Solubility Rules

Fluorides refer to compounds containing the fluoride ion. Therefore, the correct answer is 'All' because any substance that contains fluoride ions can be categorized as fluorides.

Iodides are generally soluble except those of silver, mercury, and lead due to the nature of their respective compounds. On the other hand, chlorides, sulfates, and carbonates have varying solubility properties which may not necessarily follow the same exceptions as iodides.

Chlorides are typically soluble in water, except for silver, mercury, and lead chlorides. Lead (II) chloride is an exception as it is soluble in hot water.

Bromides are generally soluble except for those of silver, mercury, and lead due to their low solubility constants.

Chlorates are typically soluble in water due to their highly polar nature, which allows them to dissociate into ions and form a solution. This property makes them useful in various industrial and laboratory applications.

Acetates are generally soluble in water due to their nature as salts of acetic acid.

Nitrates are highly soluble in water due to their ionic nature, making them easily dissolve and form solutions.

Nitrites are salts that are generally soluble in water, meaning they can dissolve in water to form a clear solution.

Perchlorates are typically considered soluble in water due to their highly ionic nature, allowing them to dissociate into ions and interact with water molecules.

Phosphates are generally insoluble except for those of ammonium and group 1 compounds due to their unique chemical properties.

Carbonates are generally insoluble except for those of ammonium and group 1 compounds due to the nature of their chemical structures and bonding.

Borates are typically insoluble in water, except for those of ammonium and group 1 compounds which are exceptions to the general rule of insolubility.

Silicates are typically insoluble except in the case of compounds involving ammonium and group 1 elements. This is due to the strong bonding within silicates that makes them difficult to dissolve in most types of compounds.

Metallic oxides are generally insoluble in water and other common solvents due to their low reactivity, with exceptions being the oxides of ammonium and group 1 compounds which are soluble.

Metallic hydroxides are typically insoluble in water except for ammonium and group one compounds, as well as group two compounds below calcium. This is due to the low solubility of most metallic hydroxides in water.

Sulfides are generally insoluble except when combined with ammonium, group one compounds, and group two compounds, where they exhibit solubility.

The correct answer states that most silver salts are insoluble except for silver nitrate and silver acetate, which are exceptions to this rule.

Chromates are generally insoluble except in the case of ammonium and group 1 compounds where they show solubility.