I performed a titration using 0.01 M NaOH to estimate the H+ concentration in a mixture containing approximately 20 mL of 50 µM H₂SO₄ and 50 µM FeCl₂ under inert atmosphere. However, I observed two endpoints during the titration, and I'm not sure why that happened. Which endpoint should I use to determine the H+ concentration?
To estimate the H⁺ concentration in a titration of H₂SO₄ and FeCl₂ with NaOH, use the first endpoint observed, which corresponds to the neutralization of H⁺ ions from sulfuric acid. The second endpoint might be influenced by other reactions or impurities and is generally not used for calculating H⁺ concentration from H₂SO₄.
FeCl2 acts as weak acid, and therefore you have two "endpoints". The second endpoint neutralizes all acidity in the mixture. In general, it is wrongly to search H+ concentration because you still have some H+ at the end of titration, even at pH 10..... You need to search H2SO4 , or total H2SO4 + FECL2. Message me for more details.
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