does BaCl2+Pb(NO3)2 form a percipitate
Yes, PbCl2.
Here is a simplified table that gives the solubility of salts.
http://www.files.chem.vt.edu/RVGS/ACT/notes/solubility_rules.html
See rule 3.
To determine if a precipitate forms when BaCl2 reacts with Pb(NO3)2, we need to consider the solubility rules for these compounds.
According to the solubility rules:
1. All nitrates (NO3-) are soluble.
2. Most chlorides (Cl-) are soluble, except for those of silver (Ag+), lead (Pb2+), and mercury (Hg2+).
3. Most sulfates (SO4^2-) are soluble, except for those of calcium (Ca2+), strontium (Sr2+), barium (Ba2+), lead (Pb2+), and silver (Ag+).
Based on these rules, BaCl2 and Pb(NO3)2 are both soluble compounds. Therefore, when they react together, no precipitate will form. The products of the reaction would be Ba(NO3)2 and PbCl2, both of which remain dissolved in the solution.
To determine if a precipitate will form when BaCl2 and Pb(NO3)2 are mixed, we can use a process called a precipitation reaction.
In a precipitation reaction, two aqueous solutions are combined, resulting in the formation of an insoluble solid called a precipitate.
To determine if a precipitate forms, we need to check if the ions from the reactants can form an insoluble compound.
BaCl2 dissociates into Ba2+ and 2 Cl- ions in solution, while Pb(NO3)2 dissociates into Pb2+ and 2 NO3- ions.
To determine if a precipitate will form, we need to check if the cation (Ba2+) from one reactant can combine with the anion (Cl-) from the other reactant to form an insoluble compound.
We can use a solubility table to check the solubility of the product formed (BaCl2).
According to most solubility tables, all chlorides are soluble except for those of silver, lead, and mercury (I).
Since PbCl2 is insoluble, a precipitate will indeed form when BaCl2 and Pb(NO3)2 are mixed.