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

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


moles Ba(OH)2 = 4.75 moles


moles H2SO4=4.75 mol Ba(OH)2×1 mol H2SO41 mol Ba(OH)2

moles H2SO4 = 4.75 mol


The reaction consumes 4.75 moles of sulfuric acid 

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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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