How many mL of a 0.10 M NaOH solution are needed to neutralize 25.0 mL of 0.200 M H3PO4 solution?

Answer 1

Balanced chemical equation:

3NaOH + H₃PO₄ = Na₃PO₄ + 3H₂O

Calculate moles of Phosphoric acid neutralized:

Convert 25.0 ml to liters = .025 liters

Use Molarity equation:

Moles of H3PO4 = .025 lit ( .200 moles/ liter) = .005 moles of H3PO4

Use balanced chemical equation to calculate the mole ratio:

Moles of NaOH required to neutralize H3PO4: .005 moles H3PO4 ( 3 mole NaOH / 1 Mole H3PO4) = .015 mole of NaOH required to neutralize H3PO4

Use Molarity equation:

Liters of NaOH required = .015 moles NaOH / .10 M = .15 liter of NaOH : Convert to ml = 150 ml of .10 M NaOH required to neu=tralize H3PO4.

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