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During a titration a student neutralizes 50.0 ml of sulfuric acid with 75.0 ml of 0.25 m sodium hydroxide, as shown below. H2SO4(aq) + 2naoh (aq) → Na2SO4 (aq) + 2h2o (l), What is the molarity of the Na2SO4 solution that results from the titration?

Accepted Answer

The molarity of the Na2SO4 solution can be calculated using the following steps:

1. Calculate the number of moles of NaOH used in the titration:

Moles of NaOH = Molarity of NaOH × Volume of NaOH
= 0.25 M × 0.075 L
= 0.01875 mol

2. Since the reaction is 1:2 (1 mole of H2SO4 reacts with 2 moles of NaOH), the number of moles of H2SO4 neutralized is:

Moles of H2SO4 = 0.01875 mol NaOH × (1 mol H2SO4 / 2 mol NaOH)
= 0.009375 mol

3. Calculate the molarity of the H2SO4 solution:

Molarity of H2SO4 = Moles of H2SO4 / Volume of H2SO4
= 0.009375 mol / 0.050 L
= 0.1875 M

4. Calculate the total volume of the solution after titration:

Total volume = Volume of H2SO4 + Volume of NaOH
= 0.050 L + 0.075 L
= 0.125 L

5. Calculate the molarity of the Na2SO4 solution:

Molarity of Na2SO4 = Moles of Na2SO4 / Total volume
= 0.009375 mol / 0.125 L
= 0.075 M

Therefore, the molarity of the Na2SO4 solution that results from the titration is 0.075 M.

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