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What mass of barium chloride, BaCL2, is required to completely precipitate the barium sulfate from 35.0 ml of 0.200 m h2so4? Bacl2 + H2SO4 to BaSO4 + HCL

What mass of barium chloride, BaCL2, is required to completely precipitate the barium sulfate from 35.0 ml of 0.200 m h2so4? Bacl2 + H2SO4 to BaSO4 + HCL
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What mass of barium chloride, BaCL2, is required to completely precipitate the barium sulfate from 35.0 ml of 0.200 m h2so4?

Bacl2 + H2SO4 to BaSO4 + HCL

asked
User Aerials
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1 Answer

1 vote
The balanced equation would be (1)BaCl2 + (1)H2SO4 --> (1)BaSO4 + (2)HCl2
Then you should know that the coefficients stand for moles.
The thing is I'm not sure if H2SO4 is 35 ml or .200 m.
Also, is this topic stoichiometry?
answered
User JSimonsen
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8.4k points
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