What volume in mL of 0.05 M NaOH(aq)would have to be added to 50.0 mL of 0.10 M H₂SO₄(aq)in order to affect complete neutralization of the acid? A)50 mL B)20 mL C)100 mL D)150 mL E)200 mL

Question

Quizplus · Accepted Answer

To find the volume of NaOH needed for neutralization, we must first determine the moles of acid present in the solution: moles H₂SO₄ = Molarity x Volume (in liters) = 0.10 mol/L x 0.050 L = 0.005 mol Since the acid is diprotic, it will react with 2 moles of NaOH for complete neutralization. Therefore, the number of moles of NaOH needed is: moles NaOH = 2 x 0.005 mol = 0.010 mol Now we can use the concentration and stoichiometry to determine the volume of NaOH needed: 0.05 mol/L = moles NaOH / Volume NaOH (in liters) Volume NaOH = moles NaOH / 0.05 mol/L Volume NaOH = 0.010 mol / 0.05 mol/L Volume NaOH = 0.200 L = 200 mL Therefore, the answer is (E) 200 mL.

What Volume in ML of 0