Question at position 1 What precipitate forms when solutions of BaCl2 and (NH4)3PO4 are mixed?What precipitate forms when solutions of BaCl2 and (NH4)3PO4 are mixed?Barium phosphateAmmonium phosphateBarium chloride Ammonium chlorideClear my selection

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First, restating the question and options: What precipitate forms when solutions of BaCl2 and (NH4)3PO4 are mixed? Options: 1) Barium phosphate 2) Ammonium phosphate 3) Barium chloride 4) Ammonium chloride.

Now, analyze each option:

Option 1: Barium phosphate. This is the correct precipitate expected from mixing a soluble barium salt (BaCl2) with a soluble phosphate salt ((NH4)3PO4). The Ba2+ ions combine with the phosphate PO4^3− ions to form the sparingly soluble compound Ba3(PO4)2, which precipitates out of solution. The overall reaction produces Ba3(PO4)2(s) and soluble ammonium chloride (NH4Cl). Since Ba3(PO4)2 has low solubility in water, it will precipitate, making this option the product of the reaction.

Option 2: Ammonium phosphate. This would be a soluble salt if formed in solution, and it does not result as a precipitate in this particular reaction. The phosphate ion does not come isolated as a new ammonium phosphate solid; instead, it pairs with Ba2+ to form Ba3(PO4)2 precipitate. Thus, this option describes a species that remains in solution or is not produced as a solid phase.

Option 3: Barium chloride. Barium chloride is a soluble salt; when BaCl2 is mixed with another soluble salt, there is no reason for BaCl2 to precipitate unless a reaction produces Ba2+ in a form that is insoluble with another anion. In this system, Ba2+ is already present as a soluble salt and will not form an insoluble BaCl2 solid. Therefore, this option is incorrect as the precipitate.

Option 4: Ammonium chloride. Ammonium chloride is also a highly soluble salt. While NH4+ and Cl− ions are present, the formation of a solid ammonium chloride is not favored here. The driving precipitation product is Ba3(PO4)2, not NH4Cl, so this option does not describe the precipitate.

Putting it together, the only species that actually precipitates under these conditions is Ba3(PO4)2, i.e., barium phosphate. The other options describe soluble salts or species that do not form a solid phase in this reaction.

Question at position 1 What precipitate forms when solutions of BaCl2 and (NH4)3PO4 are mixed?What precipitate forms when solutions of BaCl2 and (NH4)3PO4 are mixed?Barium phosphateAmmonium phosphateBarium chloride Ammonium chlorideClear my selection

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