How many milliliters of 0.130 m h2so4 are needed to neutralize 0.220 g of naoh? express the volume in milliliters to three significant digits?

The reaction between H2SO4 and NaOH can be illustrated using the following balanced chemical equation:
2 NaOH + H2So4 > Na2So4 + 2 H2O

From the periodic table:
mass of Na = 22.9 grams
mass of O = 16 grams
mass of H = 1 gram
molar mass of NaOH = 22.9+16+1 = 39.9 grams
number of moles reacting = mass / molar mass
number of moles of NaOH = 0.22 / 39.9 = 0.0055 moles

From the balanced equation above:
2 moles of NaOH react with 1 mole of H2SO4, therefore, number of H2SO4 moles that react with 0.0055 moles of NaOH can be calculated as:
number of moles of H2SO4 = (0.0055*1) / 2 = 0.00275 moles

molarity = number of moles of solvent / liters of solution
liters of solution = number of moles / molarity
liters of solution = 0.00275 / 0.13 =0.02115 liters = 21.15 ml

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