The flask shown here contains 0.275 g of acid and a few drops of phenolphthalein

Question

The flask shown here contains 0.275 g of acid and a few drops of phenolphthalein indicator dissolved in water. The buret contains 0.130 M NaOH. What volume of base is needed to reach the end point of the titration? __________mL base Assuming the acid is monoprotic, what is its molar mass? __________g/mol

Explanation / Answer

m (acid) = 0.275 g c (NaOH) = 0.130 M V (NaOH) = 20.2 ml = 0.0202 l NaOH + HX ---> NaX + H2O, as the acid is monoprotic. Using the equation, we know that NaOH reacts with HX in a 1 : 1 ratio, therefore, n (NaOH) = n (HX) = cV = 0.0202 l * 0.130 M = 0.002626 mol. M (acid) = m (acid) / n (NaOH) = m (acid) / m (acid) = 0.275 g / 0.002626 mol = 104.72 g/mol

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