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
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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