Use the reactions to complete the activity.HCl+NaOH→NaCl+H2O H2SO4+NaOH→2NaSO4+2H2O A student sets up a titration apparatus with 25 mL of hydrochloric acid in the flask. The student performs the titration using 0.050 M sodium hydroxide ( NaOH ).Next, the student wants to perform a titration using sulfuric acid ( H2SO4 ). In three to five sentences, explain what the student needs to consider when performing the calculations to find the concentration of the two acids.

Answer 1

When performing the titration calculations for both hydrochloric acid (HCl) and sulfuric acid (H2SO4), the student needs to consider the stoichiometry of each reaction. For HCl, which reacts with NaOH in a 1:1 mole ratio, the volume of NaOH used directly corresponds to the concentration of HCl. In contrast, for H2SO4, it reacts with NaOH in a 2:1 mole ratio, meaning that it will require twice as much NaOH to neutralize a given volume of sulfuric acid. Therefore, the student must account for this difference in stoichiometry when calculating the concentration of H2SO4, using the volume of NaOH and its molarity to find the moles of NaOH, and then applying the reaction ratio to determine the moles and concentration of sulfuric acid.