A solution of a theoretical triprotic acid was prepared by dissolving 4.037 g of solid in enough DI water to make 500.0 mL of solution. 10.11 mL of a 0.592 M solution was required to titrate 20.00 mL of this acid's solution.
What is the concentration of the acid solution?
What is the molar mass of the acid?
Hint: You need to calculate the total moles in the 500.0 mL solution (the full 500.0 mL was NOT titrated).
How is the experiment "Molar Mass of a Known Acid" relevant to the "Molar Mass of an Unknown Acid"? More specifically, how do they complement each other?
Note: more than one of the following responses is true, but only one addresses this question.
|Both experiments will involve using the data collected in a titration experiment to calculate the molar mass of an acid.|
|The data we collect in the "Known Acid" experiment will enable us to compare the molar mass of the known acid to the acid studied in the "Unknown Acid" experiment.|
|Both experiments make use of primary and secondary standards.|
|The former experiment will make use of the same glassware that will be used in the latter.|
The results of the former experiment will be used to evaluate the accuracy of the titration technique that will be used in the latter experiment.
3- The procedure you will follow in this experiment will be very similar to the one you followed in the "Molar Mass of a Known Acid" experiment, but will differ in one significant respect. What is it?
A) concentration of acid solution = 0.592 M x 10.11 ml/3 x 20 ml = 0.099752 M
B) molar mas of acid = 0.437 g/0.099753 M x 0.02 L = 219.043 g/mol
3. For the molar mass determination of unknown acid,
we will perform part C once with known acid and second with unknown acid.
4. If the stoichiometry of acid to base is not known,
By calculating acid equivalent molar mass instead of true molar mass.
5. Equivalent point,
The point in a titration at which the number of moles of added titrant equals the number of moles of compound in the flask being titrated.
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