When performing titrations with hydrochloric acid (HCl) and sulfuric acid (H2SO4), the student needs to consider the stoichiometry of the reactions. The titration of HCl with NaOH has a 1:1 molar ratio, meaning that one mole of HCl reacts with one mole of NaOH. In contrast, the titration of H2SO4 with NaOH involves a 1:2 molar ratio because sulfuric acid can donate two protons, requiring two moles of NaOH for each mole of H2SO4. Therefore, when calculating the concentration of H2SO4, the student must account for this difference by adjusting the volume of NaOH used in their calculations to reflect that two moles of NaOH are needed for every mole of H2SO4 to determine the correct concentration of the diprotic acid.
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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