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Question

50 mL of 20.8% (w/v) BaCl2(aq) and 100 mL of 9.8% (w/v) H2SO4 solutions are mixed. Find the mass the BaSO4 formed.
(Molar mass of Ba = 137 g/mL)

A
23.32 g
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B
2.06 g
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C
0.126 g
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D
11.65 g
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Solution

The correct option is D 11.65 g
BaCl2+ H2SO4BaSO4+ 2HCl
Mass of BaCl2=20.8100×50 mL
=10.4 g
moles of BaCl2=10.4208=0.05 mol
Mass of H2SO4=9.8100×100=9.8 g
Moles of H2SO4=9.898=0.1 mol
Therefore, BaCl2 is the limiting reagent.
Moles of BaSO4​ formed is 0.05 mol
Mass of BaSO4​ formed = 0.05 x 233 g
= 11.65 g
Therefore, the mass of BaSO4​ formed is 11.65 g.

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