How many mL of 0.100 M NaOH is required to react with 50.0 mL of 0.100 M H2SO4 a

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Explanation / Answer

first write a balanced equation H2SO4 + 2NaOH -----> Na2SO4 + 2H2O You can see that you need 2 moles of NaOH to neutralise 1 mole of H2SO4 moles H2SO4 used = molarity x Litres = 0.100 M x 0.0250 L = 0.00250 moles H2SO4 You need 2 moles NaOH for every 1 mole H2SO4 So moles NaOH needed = 2 x moles H2SO4 = 0.00500 moles NaOH needed Volume NaOH needed = moles / molarity = 0.00500 mol / 0.100 M = 0.0500 L = 50.0 ml

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