3BaCl + 2Na3PO4 --> Ba3(Po4)2 +^NaCl
is Ba3(PO4)2 the ppt. because Cl salts are soluble so it will dissolve?
yes.
A couple of additional notes here. First, barium chloride is BaCl2.
Also, not all chlorides are soluble. All chlorides are soluble except the chlorides of silver, mercury(I) and lead.
To determine if Ba3(PO4)2 is the precipitate (ppt) in the reaction 3BaCl + 2Na3PO4 -> Ba3(PO4)2 + 6NaCl, we need to consider the solubility of the compounds involved.
Solubility rules state that most chloride (Cl-) salts are soluble, including sodium chloride (NaCl). However, not all phosphates (PO4-), including barium phosphate (Ba3(PO4)2), are soluble.
To determine if Ba3(PO4)2 will form a solid precipitate, we need to compare the solubility rules for chloride and phosphate compounds.
1. Chloride salts (such as NaCl) are generally soluble, meaning they will dissolve in water.
2. Phosphate salts (such as Ba3(PO4)2) have limited solubility. According to solubility rules, most phosphates are insoluble except for a few exceptions like those of Group 1A cations (such as Na+) and ammonium (NH4+).
Based on these solubility rules, it is likely that Ba3(PO4)2 will form as a solid precipitate during the reaction, while NaCl will remain dissolved in the solution.