Acid Base Titaration

Question

You carry out the titration of a weak diprotic solid acid. You take 0.178 g of the solid acid and dissolve it in about 50 mL of distilled water. You titrate with 0.1005 M NaOH and arrive at the second endpoint at 24.20 ml. You know that at the final pH both protons have been titrated. What is the molar mass of the acid?

Answer 1

(𝟎.𝟎𝟐𝟒𝟐𝟎 𝑳 𝑵𝒂𝑶𝑯) (𝟎.𝟏𝟎𝟎𝟓 𝒎𝒐𝒍 𝑵𝒂𝑶𝑯 / 𝟏 𝑳 𝑵𝒂𝑶𝑯) = 𝟎.𝟎𝟎𝟐𝟒𝟑𝟐𝟏 𝒎𝒐𝒍 𝑵𝒂𝑶𝑯

(𝟎.𝟎𝟎𝟐𝟒𝟑 𝒎𝒐𝒍 𝑵𝒂𝑶𝑯) (𝟏 𝒎𝒐𝒍 𝑨𝒄𝒊𝒅 / 𝟐 𝒎𝒐𝒍 𝑵𝒂𝑶𝑯) = 𝟎.𝟎𝟎𝟏𝟐𝟏𝟔 𝒎𝒐𝒍 𝑨𝒄𝒊𝒅

𝟎.𝟏𝟕𝟖 𝒈 𝑨𝒄𝒊𝒅 / 𝟎.𝟎𝟎𝟏𝟐𝟏𝟔 𝒎𝒐𝒍 𝑨𝒄𝒊𝒅 = 𝒎𝒐𝒍𝒂𝒓 𝒎𝒂𝒔𝒔

𝟏𝟒𝟔.𝟑𝟖 𝒈𝒎𝒐𝒍=𝒎𝒐𝒍𝒂𝒓 𝒎𝒂𝒔𝒔