If an unknown sample contains 39.04% sulfuric acid by mass,then a 0.9368 g of that sample would require ________ mL of 0.2389 M NaOH for neutralization.
A)31.22
B)39.98
C)7.80
D)79.96
E)15.61

Question

Quizplus · Accepted Answer

The correct answer is A.To neutralize the sulfuric acid in the sample, we need to use an equivalent amount of NaOH. The balanced chemical equation for the neutralization reaction is:H2SO4 + 2NaOH -> Na2SO4 + 2H2OFrom the equation, we can see that 1 mole of H2SO4 reacts with 2 moles of NaOH. Therefore, the number of moles of NaOH required to neutralize the sulfuric acid in the sample is:moles of NaOH = moles of H2SO4 x 2The mass of H2SO4 in the sample is:mass of H2SO4 = 0.9368 g x 39.04% = 0.3648 gThe number of moles of H2SO4 in the sample is:moles of H2SO4 = 0.3648 g / 98.08 g/mol = 0.003718 molTherefore, the number of moles of NaOH required to neutralize the sulfuric acid in the sample is:moles of NaOH = 0.003718 mol x 2 = 0.007436 molThe volume of 0.2389 M NaOH required to neutralize the sulfuric acid in the sample is:volume of NaOH = moles of NaOH / molarity of NaOH = 0.007436 mol / 0.2389 M = 31.22 mLTherefore, the correct answer is A) 31.22 mL.

If an Unknown Sample Contains 39