2.4 **Scenario:** An analytical chemist weighs out 0.125 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1400 M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 11.9 mL of NaOH solution.**Objective:** Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits.To solve this task, follow these steps:1. **Understanding the Titration Reaction:** For a diprotic acid, the reaction with NaOH can be represented as: \[ H_2A + 2\ NaOH \rightarrow Na_2A + 2\ H_2O \] Here, $ H_2A $ is the diprotic acid, and $ NaOH $ is the sodium hydroxide.2. **Calculate Moles of NaOH Added:** Given the volume of NaOH solution used is 11.9 mL (0.0119 L) and its molarity is 0.1400 M: \[ \text{Moles of NaOH} = 0.1400\ \text{M} \times 0.0119\ \text{L} = 0.001666\ \text{mol} \]3. **Determine Moles of Diprotic Acid:** From the balanced chemical equation, 1 mole of $ H_2A $ reacts with 2 moles of NaOH. Therefore, the moles of diprotic acid ( $ H_2A $ ) would be: \[ \text{Moles of } H_2A = \frac{0.001666\ \text{mol NaOH}}{2} = 0.000833\ \text{mol} \]4. **Molar Mass of Acid:** Molar mass is calculated using the formula: \[ \text{Molar mass} = \frac{\text{Mass of Acid}}{\text{Moles of Acid}} \] Given the mass of the acid is 0.125 g: \[ \text{Molar mass} = \frac{0

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An analytical chemist weighs out 0.125 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1400M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 11.9 mL of NAOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. Ox10 mol

An analytical chemist weighs out 0.125 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1400M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 11.9 mL of NAOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. Ox10 mol

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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