When performing titrations with hydrochloric acid (HCl) and sulfuric acid (H₂SO₄), the student must consider the differences in stoichiometry between the two acids and the sodium hydroxide (NaOH) reactant. For HCl, the reaction produces one mole of water for each mole of HCl reacted with NaOH, allowing for a straightforward 1:1 molar ratio. In contrast, sulfuric acid can donate two protons (H⁺) per molecule, leading to a 1:2 stoichiometry with NaOH; therefore, it will require twice the amount of NaOH to completely neutralize a given amount of H₂SO₄. Consequently, when calculating the concentration of the acids, the student must account for these stoichiometric differences, applying the correct molar ratios in their calculations to ensure accurate determination of concentration.
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.
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