The solubility of barium is somewhat mixed---it can be soluble with notoriously insoluble things like hydroxide, and it can be insoluble with other somewhat insoluble anions like sulfate. However, chromate is one anion that is almost always insoluble unless it is paired with an alkali metal. So mixing these two compounds will give you a BaCrO4 precipitate.
If both are in solutions, barium sulfate would precipitate out of the solution - unless if the barium chloride solution is dilute enough that only a small amount of barium sulfate will form, thus remaining soluble in the solution. The remaining sulfate will remain in the solution as wellas sodium and chloride.
Ba(NO3)2(aq) +K2CO3(aq)-->BaCO3 (s)(aq) +2KNO3(aq)
2K3PO4 + 3Ba(NO3)2 -----> 6KNO3 + Ba3(PO4)2
no reaction.
The formula unit for the formation of potassium chloride and barium sulfate is one mole. One unit of potassium sulfate and barium chloride are required for the reaction.
bubbling
It may produce an explosive mixture on standing .
BaCl2- and KCl-solutions have no color, and also none when mixed.
Pb(NO3)2 + 2KI -----> PbI2 + 2KNO3
2K 3 PO 4 + 3Ba(NO 3 ) 2 -----> 6KNO 3 + Ba 3 (PO 4 ) 2
It's Barium Carbonate. Due to the solubilty rules, nitrates and chlorates are soluble.
The formula unit for the formation of potassium chloride and barium sulfate is one mole. One unit of potassium sulfate and barium chloride are required for the reaction.
bubbling
No
jj
3KBrO3 + AlPO4 ------> K3PO4 + Al(BrO3)3
I am not sure
yellow
silver nitrate and potassium iodide can be used.
It may produce an explosive mixture on standing .
Ag+(aq) + PO4-(aq) -------> Ag3PO4(s)