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A student runs the reaction below with 169 mL of 0.471 M sulfuric acid (H2SO4). If the sodium hydroxide is 0.280 M, how many milliliters will be needed for the reaction?
H2SO4 + 2 NaOH → Na2SO4 + 2 H2O
Expert Answer
Answer
First, let us identify the ratio of moles:
1 mol of H2SO4 = 2 mol of NaOH
so…
mol of H2SO4 = Macid*Vacid = 0.471 * 169 = 79.599 mmol of H2SO4
then, we need –> 1/2*79.599 = 39.7995 mmol of NaOH
if we have
M = 0.28 M of NaOH
find volume, in mL:
M = mmol/mL
mL = mmol/M
mL of base = 39.7995 / 0.28
mL of base = 142.141 mL required
