Final answer:
To find the volume of 0.270 M H2SO4 needed to react with 46.0 mL of 0.104 M NaOH, we can use the balanced chemical equation and stoichiometry of the reaction. The volume of 0.270 M H2SO4 needed is approximately 8.855 mL.
Step-by-step explanation:
To find the volume of 0.270 M H2SO4 needed to react with 46.0 mL of 0.104 M NaOH, we need to use the balanced chemical equation and the stoichiometry of the reaction.
The balanced equation is H2SO4 (aq) + 2NaOH(aq) → Na2SO4 (aq) + 2H2O(1). From the equation, we can see that for every 1 mole of H2SO4, 2 moles of NaOH are required.
First, we calculate the moles of NaOH: 0.104 M NaOH x 0.0460 L = 0.004784 moles NaOH.
Since the ratio of moles of H2SO4 to NaOH is 1:2, we can multiply the moles of NaOH by 1/2 to find the moles of H2SO4: 0.004784 moles NaOH x (1/2) = 0.002392 moles H2SO4.
Finally, we can calculate the volume of 0.270 M H2SO4 needed using the molarity formula: Volume = moles/molarity = 0.002392 moles / 0.270 M = 0.008855 L = 8.855 mL.