In order to determine how many milliliters of a 1.28 M H2SO4 solution are needed to neutralize 60.2 mL of a 0.427 M KOH solution, we need to use the stoichiometry of the reaction and the concept of molarity. The balanced chemical equation for the reaction between sulfuric acid (H2SO4) and potassium hydroxide (KOH) is: H2SO4 + 2KOH → K2SO4 + 2H2O From the equation, we can see that each mole of sulfuric acid (H2SO4) reacts with 2 moles of potassium hydroxide (KOH). Therefore, we need to calculate the number of moles of KOH in the 60.2 mL of 0.427 M KOH solution: moles of KOH = concentration × volume = 0.427 M × 0.0602 L = 0.0258 mol According to stoichiometry, we need the same number of moles of H2SO4 to completely neutralize the KOH. Since we know the concentration of the H2SO4 solution, we can use the following equation to calculate the volume of the H2SO4 solution required: moles of H2SO4 = concentration × volume volume of H2SO4 = moles of H2SO4 / concentration volume of H2SO4 = 0.0258 mol / 1.28 M = 0.0202 L Finally, we need to convert this volume to milliliters: volume of H2SO4 = 0.0202 L × 1000 mL/L = 20.2 mL Therefore, 20.2 mL of a 1.28 M H2SO4 solution are needed to neutralize 60.2 mL of a 0.427 M KOH solution. In conclusion, the calculation of the volume of H2SO4 required to neutralize a given volume of KOH solution involves the use of the stoichiometry of the reaction and the concept of molarity. It is important to pay attention to the balanced chemical equation and the units of the concentration and volume used in the calculations. This type of calculation is commonly used in analytical chemistry and is an essential skill for any laboratory scientist.