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
79 exam-style questions on AQA A Level Chemistry Amount of substance, covering Relative atomic mass and relative molecular mass, The mole and the Avogadro constant, The ideal gas equation, Empirical and molecular formula, and Balanced equations and associated calculations. Each one has a worked solution and a mark scheme showing where the marks go.