No, not all carbonates are insoluble in water. While many carbonates, such as calcium carbonate and magnesium carbonate, have low solubility, some, like sodium carbonate and potassium carbonate, are soluble in water. The solubility of carbonates generally depends on the metal ion they contain and the pH of the solution.
Yes it is. All carbonates are insoluble, with the exception of 1st row elements.
Not all carbonates dissolve in water. Some carbonates, such as calcium carbonate (found in limestone and chalk) and sodium carbonate (commonly known as washing soda), are sparingly soluble in water and only dissolve to a small extent. Other carbonates, like potassium carbonate and lithium carbonate, are more soluble in water.
The solubility of carbonate salts varies depending on the specific salt and the conditions. Generally, carbonates of alkali metals like sodium and potassium are soluble in water, while carbonates of transition metals are not very soluble.
Carbonate salts are insoluble in water because of the strong ionic bond between the carbonate ion (CO3^2-) and the cation in the salt. This bond is difficult to break, preventing the salt from easily dissolving in water. Additionally, the carbonate ion tends to form insoluble precipitates with many cations, further reducing its solubility.
Carbonates of metals typically exhibit thermal stability, breaking down upon heating to release carbon dioxide and form metal oxides. They are often ionic compounds, with metal cations bonded to carbonate anions (CO3²⁻). Solubility varies widely among different metal carbonates; for instance, alkali metal carbonates are generally soluble in water, while many transition metal carbonates are insoluble. Additionally, metal carbonates can react with acids to produce carbon dioxide gas, water, and corresponding metal salts.
Yes it is. All carbonates are insoluble, with the exception of 1st row elements.
- All carbonates (except ammonium, sodium & potassium carbonates) are insoluble - Lead, barium & calcium sulphates are insoluble - Lead & silver chlorides are insoluble
Not all carbonates dissolve in water. Some carbonates, such as calcium carbonate (found in limestone and chalk) and sodium carbonate (commonly known as washing soda), are sparingly soluble in water and only dissolve to a small extent. Other carbonates, like potassium carbonate and lithium carbonate, are more soluble in water.
Common carbonates like calcium carbonate (CaCO3) and magnesium carbonate (MgCO3) are generally insoluble in water. However, some carbonates like sodium carbonate (Na2CO3) and potassium carbonate (K2CO3) are more soluble and will dissolve in water.
The solubility of carbonate salts varies depending on the specific salt and the conditions. Generally, carbonates of alkali metals like sodium and potassium are soluble in water, while carbonates of transition metals are not very soluble.
NaNO3 is highly soluble in room-temperature water.
Rule 6
Carbonate salts are insoluble in water because of the strong ionic bond between the carbonate ion (CO3^2-) and the cation in the salt. This bond is difficult to break, preventing the salt from easily dissolving in water. Additionally, the carbonate ion tends to form insoluble precipitates with many cations, further reducing its solubility.
Silicates generally do not react with acids like carbonates do. Silicates are generally insoluble in common acids due to their strong chemical bonds, whereas carbonates typically react with acids to form carbon dioxide gas, water, and a salt.
Carbonates of metals typically exhibit thermal stability, breaking down upon heating to release carbon dioxide and form metal oxides. They are often ionic compounds, with metal cations bonded to carbonate anions (CO3²⁻). Solubility varies widely among different metal carbonates; for instance, alkali metal carbonates are generally soluble in water, while many transition metal carbonates are insoluble. Additionally, metal carbonates can react with acids to produce carbon dioxide gas, water, and corresponding metal salts.
A precipitate is formed when two chemicals combine where one or more of which contains an "insoluble" element or compound. All Carbonates and Phosphates except Ammonium are insoluble. In addition, all Hydroxides except Strontium and Barium are insoluble. All Sulfides minus group II and Ammonium are also insoluble. Finally, all Oxides are also insoluble and will mandate the production of a precipitate in a reaction. It is important to remember that ALL group I elements, Ammonium, Strontium and Barium are soluble and should not be considered.
Fe2(CO3)3, iron(III) carbonate, is generally considered insoluble in water. While some carbonates are soluble, most metal carbonates, including iron(III) carbonate, have low solubility in water due to their ionic lattice structure. Therefore, in practical terms, Fe2(CO3)3 does not dissolve significantly in water.