How many milliliters of 0.130 M H2SO4 are needed to neutralize 0.240 g of NaOH?
The balanced equation is
2 NaOH + H2SO4 ---------> Na2SO4 + 2 H2O
Number of moles of NaOH = mass/mol.wt. = 0.240 g/(40.00 g/mol) = 0.006 mol
According to balanced equation,
2 moles of NaOH neutralizes 1 mole of H2SO4
So, 0.006 mol of NaOH would neutralize 0.006 mol * ½ = 0.003 mol of H2SO4
Number of moles of H2SO4 = 0.003 mol
Molarity of H2SO4 = 0.130 M = 0.130 mol/L
Volume of H2SO4 = 0.003 mol/(0.130 mol/L) = 0.023077 L = 23.07692 mL = 23.1 mL
How many milliliters of 0.130 M H2SO4 are needed to neutralize 0.240 g of NaOH?
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