""" Problem Statement You need to determine how many milliliters of 0.500 M sulfuric acid (H2SO4) will be necessary to neutralize 200 mL of 0.750 M sodium hydroxide (NaOH) solution. Steps to Solve the Problem 1. Write the Balanced Chemical Equation First, we write the chemical reaction that happens when sulfuric acid reacts with sodium hydroxide: H2SO4 (aq) + 2NaOH (aq) -> Na2SO4 (aq) + 2H2O (l) This equation shows that one mole of sulfuric acid reacts with two moles of sodium hydroxide to produce one mole of sodium sulfate and two moles of water. 2. Calculate the Moles of Sodium Hydroxide (NaOH) We use the formula for moles: Moles = Molarity * Volume (L) First, we need to convert the volume from milliliters (mL) to liters (L): 200 mL = 0.200 L Now, calculate the moles of NaOH: Moles of NaOH = 0.750 M * 0.200 L = 0.150 moles 3. Determine the Moles of Sulfuric Acid (H2SO4) Needed From the balanced equation, we see that 1 mole of H2SO4 reacts with 2 moles of NaOH. This means we need half as many moles of H2SO4 as we have moles of NaOH. Moles of H2SO4 = Moles of NaOH / 2 Moles of H2SO4 = 0.150 moles / 2 = 0.075 moles 4. Calculate the Volume of Sulfuric Acid (H2SO4) Needed We need to find out how many milliliters of 0.500 M H2SO4 solution contains 0.075 moles. Use the formula for volume: Volume (L) = Moles / Molarity Volume of H2SO4 (L) = 0.075 moles / 0.500 M = 0.150 L Convert the volume from liters to milliliters: 0.150 L = 150 mL Summary To neutralize 200 mL of 0.750 M NaOH solution, you will need 150 mL of 0.500 M H2SO4 solution. """