We’re being asked tocalculate the mass of barium sulfate (BaSO4)formed in the reaction of100.0 mL of 0.100 M BaCl2 solution and 100.0 mL of 0.100 M Fe2(SO4)3.

You are watching: How many moles of barium sulfate are produced from 0.100 mole of barium chloride?

For this problem, we need to do the following steps:

Step 1:Determine the products of the reaction.

Step 2:Write and balance a chemical equation for the given reaction.

Step 3:Determine the limiting reactant and calculate the mass of BaSO4 produced.

Step 1:Since BaCl2 and Fe2(SO4)3 areionic compounds, they form ions when dissociating in water.The dissociation of the two compounds is as follows:

For BaCl2:

The chloride ion, Cl–, has a charge of–1. Barium is from Group 2 so it has a charge of+2:

BaCl2(aq)⇌Ba2+(aq) + 2Cl–(aq)

For Fe2(SO4)3:

The sulfate ion, SO42–, has a charge of–2. Iron then has a charge of+3:

Fe2(SO4)3(aq)⇌2 Fe3+(aq) + 3SO42–(aq)

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Problem Details

What mass of barium sulfate can be produced when 100.0 mL of a 0.100-M solution of barium chloride is mixed with 100.0 mL of a 0.100-M solution of iron(III) sulfate?

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.

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