What is the precipitate of K2CrO4 +
Al2(SO4)3 ?
Al2(CrO4)3(s)
To determine the precipitate formed in a chemical reaction, we need to examine the solubility rules of the compounds involved. In this case, we have K2CrO4 (potassium chromate) and Al2(SO4)3 (aluminum sulfate).
Let's first look at the solubility rules for potassium chromate (K2CrO4):
1. All compounds containing alkali metal cations (such as K+; potassium) are soluble and generally do not form precipitates, except when combined with certain anions.
2. Chromates (CrO4^2-) are generally insoluble, except when combined with alkali metals such as potassium (K+).
Now let's examine the solubility rules for aluminum sulfate (Al2(SO4)3):
1. All compounds containing alkali metal cations (such as K+; potassium) are soluble and generally do not form precipitates.
2. Sulfates (SO4^2-) are generally soluble, except when combined with certain cations, including silver (Ag+), lead (Pb2+), and barium (Ba2+).
Based on these solubility rules, we can determine that potassium chromate (K2CrO4) is soluble, as it contains an alkali metal cation (K+). On the other hand, aluminum sulfate (Al2(SO4)3) is also soluble, as sulfates are generally soluble except when combined with certain cations, which is not the case here.
Therefore, the reaction between K2CrO4 and Al2(SO4)3 does not result in a precipitate.