in a titration, 0.0400 mol of solid NaOH is required to neutralize 10.0 mL of H2SO4(aq). From these data, the [H2SO4] is:
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To find the concentration of H2SO4, we can use the stoichiometry of the balanced equation and the given information.
First, let's write the balanced chemical equation for the reaction between NaOH and H2SO4:
2 NaOH + H2SO4 → Na2SO4 + 2 H2O
From the equation, we can see that 2 moles of NaOH react with 1 mole of H2SO4.
Given that 0.0400 mol of NaOH is required to neutralize 10.0 mL of H2SO4(aq), we can calculate the number of moles of H2SO4 used:
Moles of H2SO4 = (0.0400 mol NaOH) / (2 mol NaOH / 1 mol H2SO4) = 0.0200 mol H2SO4
Next, we need to find the concentration of H2SO4 in the given solution. Concentration is defined as the number of moles of solute per liter of solution.
Since 10.0 mL of H2SO4(aq) was used, we need to convert this volume to liters:
Volume of H2SO4 solution (in liters) = 10.0 mL * (1 L / 1000 mL) = 0.0100 L
Now we can calculate the concentration of H2SO4:
[H2SO4] = Moles of H2SO4 / Volume of H2SO4 solution
= 0.0200 mol / 0.0100 L
= 2.00 mol/L
Therefore, the concentration of H2SO4 in the solution is 2.00 mol/L.