# Problem: When barium hydroxide reacts with sulfuric acid, barium sulfate and water are produced. The balanced equation for this reaction is: Ba(OH)2(aq) + H2SO4(aq) → BaSO4(s) + 2H2O(l) Suppose 4.75 moles of barium hydroxide react. The reaction consumes  _____ moles of sulfuric acid The reaction produces _____ moles of barium sulfate and _____ moles of water.

###### FREE Expert Solution
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###### FREE Expert Solution

Ba(OH)2(aq) + H2SO4(aq) → BaSO4(s) + 2 H2O(l)

moles Ba(OH)2 = 4.75 moles

moles H2SO4 = 4.75 mol

The reaction consumes 4.75 moles of sulfuric acid

90% (254 ratings)
###### Problem Details

When barium hydroxide reacts with sulfuric acid, barium sulfate and water are produced. The balanced equation for this reaction is:

Ba(OH)2(aq) + H2SO4(aq) → BaSO4(s) + 2H2O(l)

Suppose 4.75 moles of barium hydroxide react.

The reaction consumes  _____ moles of sulfuric acid

The reaction produces _____ moles of barium sulfate and _____ moles of water.

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Our tutors have indicated that to solve this problem you will need to apply the Stoichiometry concept. You can view video lessons to learn Stoichiometry Or if you need more Stoichiometry practice, you can also practice Stoichiometry practice problems .

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Based on our data, we think this problem is relevant for Professor Fortenberry's class at OLE MISS.