Question

a student fills a buret to the 3.50-ml mark with 1.10 m NaOH. she puts a 10.00 ml of an unknown monoprotic acid solution in an erlenmeyer flask with a few drops of phenolphthalein. she titrate the acid to a pink endpoint. the final buret reading is 12.33 ml. what is the concentration of the acid?

Answer 1

The concentration of the acid is found by using the titration formula M1V1 = M2V2, considering the volume of NaOH solution used and its concentration to solve for the molarity of the acid.

Step-by-step explanation:

The student is asking to find the concentration of an unknown monoprotic acid using titration data. To calculate the concentration of the acid, we use the formula M1V1 = M2V2, where M1 and M2 are the molarities of the acid and base respectively, and V1 and V2 are the volumes of acid and base used in the titration. Given the initial volume of NaOH in the buret (3.50 ml), the final volume (12.33 ml), and the NaOH molarity (1.10 M), we can calculate the volume of NaOH used in the reaction (12.33 ml - 3.50 ml = 8.83 ml). The volume of the acid is 10.00 ml.

Using the titration equation: M1V1 = M2V2, where M1 is the molarity of the unknown acid, V1 is 10.00 ml, M2 is 1.10 M (molarity of NaOH), and V2 is 8.83 ml (volume of NaOH used), we can solve for M1, the molarity of the acid. The calculation would be as follows: M1 * 10.00 ml = 1.10 M * 8.83 ml. Therefore, M1 = (1.10 M * 8.83 ml) / 10.00 ml, which gives us the concentration of the unknown acid.