which of the following aqueous solutions should not form a precipitate with aqueous ba(no3)?
1. KOH
2. K2CO3
3. K2SO4
4. K3PO4
http://www.files.chem.vt.edu/RVGS/ACT/notes/solubility_rules.html
To determine which of the given aqueous solutions will not form a precipitate with aqueous Ba(NO3)2, we need to consider the solubility rules of common salts.
1. KOH (potassium hydroxide): According to the solubility rules, hydroxide compounds are generally insoluble, except for those of group 1 metals, such as potassium (K+). This means that KOH is soluble in water and will not form a precipitate with Ba(NO3)2.
2. K2CO3 (potassium carbonate): Carbonates are generally insoluble, except for those of group 1 metals, such as potassium (K+). Therefore, K2CO3 is soluble in water and will not form a precipitate with Ba(NO3)2.
3. K2SO4 (potassium sulfate): Sulfates are generally soluble, except for a few exceptions, including barium sulfate (BaSO4). Since Ba(NO3)2 reacts with sulfate ions (SO4^2-) to form an insoluble precipitate (BaSO4), K2SO4 will form a precipitate with Ba(NO3)2.
4. K3PO4 (potassium phosphate): Phosphates are generally insoluble, except for those of group 1 metals, such as potassium (K+). Therefore, K3PO4 is soluble in water and will not form a precipitate with Ba(NO3)2.
Based on the solubility rules, the aqueous solutions that should not form a precipitate with aqueous Ba(NO3)2 are: 1. KOH and 2. K2CO3.