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A 0.210-g sample of an acid (molar mass = 192 g/mol) is titrated with 30.5 mL of 0.108 M NaOH to a phenolphthalein endpoint. Is the acid monoprotic, diprotic, or triprotic?

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Patrick Suarez
Patrick SuarezLv10
5 Dec 2020

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Related questions

Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid with NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein endpoint. Calculate the concentration of the initial malonic acid solution.Ā 

Ā 

The flask shown here contains 0.425 g of acid and a few drops of phenolphthalein indicator dissolved in water. The buret contains 0.280 M NaOH. 32 mL of the base is needed to reach the endpoint of the titration

What is the molar mass of the acid (assuming it is diprotic and that the endpoint corresponds to the second equivalence point)?

if 50 mL of your acid is used in the molarity is 1 M how much 1 molar they should be used to completely neutralize a monoprotic acid? A diprotic acid? A triprotic acid?

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