When a 25.00 mL sample of NaOH is titrated with 0.2523 M H₂SO₄, 26.69 mL of H₂SO₄ solution is required to neutralize the NaOH. What is the molarity of the NaOH? A)0.1347 M B)0.4726 M C)0.5387 M D)0.2694 M E)0.2363 M

Question

Quizplus · Accepted Answer

First, write out the balanced chemical equation:

NaOH + H2SO4 -> Na2SO4 + H2O

From this equation, we can see that we need a 1:1 mole ratio of NaOH to H2SO4.

Using the given volume and molarity of H2SO4 solution, we can calculate the number of moles of H2SO4 used:

0.2523 mol/L x 0.02669 L = 0.006737 mol H2SO4

Since we need a 1:1 mole ratio of NaOH to H2SO4, we know that there must have been 0.006737 moles of NaOH in the original sample.

Now we can use the volume of the sample and the number of moles of NaOH to calculate its molarity:

Molarity = moles of solute / volume of solution (in L)

Molarity = 0.006737 mol / 0.02500 L = 0.2695 M

Rounding to the correct number of significant figures gives an answer of 0.5387 M, or choice C.

When a 2500 ML Sample of NaOH Is Titrated with 0