2.4 ### Determining the Molar Mass of an Unknown Acid through TitrationAn analytical chemist weighs out **0.074 g** of an unknown monoprotic acid into a **250 mL** volumetric flask and dilutes it to the mark with distilled water. She then titrates this solution with **0.0600 M NaOH** solution. When the titration reaches the equivalence point, the chemist finds she has added **13.1 mL** of NaOH solution.**Objective:** Calculate the molar mass of the unknown acid. Round your answer to 2 significant digits.#### Calculation Process:1. **Determine moles of NaOH added:** - Volume of NaOH solution used: 13.1 mL - Molarity of NaOH solution: 0.0600 M - Convert volume to liters: 13.1 mL = 0.0131 L - Moles of NaOH $ = \text{Molarity} \times \text{Volume} $ $ \text{Moles of NaOH} = 0.0600 \text{M} \times 0.0131 \text{L} = 0.000786 \text{ moles} $2. **Relate moles of NaOH to moles of the unknown acid:** Since the acid is monoprotic (one mole of acid reacts with one mole of NaOH), $ \text{Moles of unknown acid} = 0.000786 \text{ moles} $3. **Calculate molar mass:** - Mass of unknown acid: 0.074 g - Moles of unknown acid: 0.000786 moles - Molar mass $ = \frac{\text{Mass}}{\text{Moles}} $ $ \text{Molar mass} = \frac{0.074 \text{ g}}{0.000786 \text{ moles}} = 94.14 \text{ g/mol} $ Round to 2 significant digits: 94 g/mol#### Diagram and Graphical Explanation:The image contains results sections for entering numerical value:- A blank field for entering the molar mass with the unit "g/mol".- Interface buttons for submitting the answer, resetting the calculation, and accessing

Acid - Base titration In acid - base titration at equivalence point M1×V1 = M2×V2 Let, 1 for acid…

An analytical chemist weighs out 0.074 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0600M NaOH solution. Wwhen the titration reaches the equivalence point, the chemist finds she has added 13.1 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 2 significant digits.

An analytical chemist weighs out 0.074 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0600M NaOH solution. Wwhen the titration reaches the equivalence point, the chemist finds she has added 13.1 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 2 significant digits.

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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