Barium chloride and sodium phosphate react in aqueous solution to form a precipitate of barium phosphate according to the following balanced equation:
3BaCl2(aq)+2Na3PO4(aq)→Ba3(PO4)2(s)+6NaCl(aq) 3\text{BaCl}_2(\text{aq}) + 2\text{Na}_3\text{PO}_4(\text{aq}) \rightarrow \text{Ba}_3(\text{PO}_4)_2(\text{s}) + 6\text{NaCl}(\text{aq}) 3BaCl2(aq)+2Na3PO4(aq)→Ba3(PO4)2(s)+6NaCl(aq)In an experiment, 50.0 cm3 of a 0.150 mol dm-3 solution of each compound are mixed together.
Which amount, in mol, of barium phosphate precipitate is formed?
3.75×10−33.75 \times 10^{-3}3.75×10−3
2.50×10−32.50 \times 10^{-3}2.50×10−3
5.00×10−35.00 \times 10^{-3}5.00×10−3
7.50×10−37.50 \times 10^{-3}7.50×10−3