Not true; as an example all the alkali carbonates are very soluble in water.
An example of a reaction:Na2SO4 + BaCl2 - BaSO4 + 2 NaClBarium sulfate is a white precipitate.
barium carbonate is a white crystals that it is an insoluble salts.
Some carbonates are soluble (carbonates of alkali metals) and some carbonates are practically insoluble in water (calcium and magnesium carbonate etc.).
Insoluble salts are the products of precipitation reactions.
Insoluble salts are not the products of electrolysis.
An example of a reaction:Na2SO4 + BaCl2 - BaSO4 + 2 NaClBarium sulfate is a white precipitate.
barium carbonate is a white crystals that it is an insoluble salts.
Examples are: silver chloride, cadmium sulfide, calcium carbonate, barium sulfate etc.
Some carbonates are soluble (carbonates of alkali metals) and some carbonates are practically insoluble in water (calcium and magnesium carbonate etc.).
Only some salts are insoluble.
All ammonium salts (containing NH4+ ions) are soluble.
Insoluble salts are the products of precipitation reactions.
Insoluble salts are not the products of electrolysis.
Insoluble salts are the products of precipitation reactions.
- All carbonates (except ammonium, sodium & potassium carbonates) are insoluble - Lead, barium & calcium sulphates are insoluble - Lead & silver chlorides are insoluble
There are several methods:1. Direct combination (for binary salts such as chlorides) 2.Acid plus metal 3. Acid plus base 4. Acid plus carbonate 5. Precipitation (for insoluble salts).
Salts are prepared by a reaction between an acid and a base; the insoluble salt is a precipitate.