If 25.0 mL of 0.100 M HCl is titrated with 0.150 M Ba(OH)2,what volume of barium hydroxide is required to neutralize the acid? 2 HCl(aq)+ Ba(OH)2(aq)→ BaCl₂(aq)+ 2 H₂O(l)

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The balanced equation shows that 2 moles of HCl react with 1 mole of Ba(OH)2. Calculate moles of HCl: 0.025 L * 0.100 M = 0.0025 moles. Moles of Ba(OH)2 needed: 0.0025 moles / 2 = 0.00125 moles. Volume of Ba(OH)2: 0.00125 moles / 0.150 M = 0.00833 L = 8.33 mL.

If 250 ML of 0