### Problem:An analytical chemist is titrating 64.7 mL of a 0.8500 M solution of acetic acid (HCH₃CO₂) with a 0.2700 M solution of KOH. The $ pK_a $ of acetic acid is 4.70.Calculate the pH of the acid solution after the chemist has added 56.9 mL of the KOH solution to it.**Note for advanced students:** you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added.**Round your answer to 2 decimal places.**### Input Fields:- $ \text{pH} = \_\_\_ $### Additional Information:The image shows input boxes for entering and calculating the pH value. The functionality includes options for confirming the input (X), resetting (↺), and getting help or information (?) symbol. ### Key Formulas and Approach:1. **Determine the initial moles of acetic acid (HCH₃CO₂)**: \[ \text{Moles of } HCH_3CO_2 = \text{Concentration} \times \text{Volume} \] \[ = 0.8500 \, M \times 0.0647 \, L \]2. **Determine the moles of KOH added**: \[ \text{Moles of KOH} = \text{Concentration} \times \text{Volume} \] \[ = 0.2700 \, M \times 0.0569 \, L \]3. **Identify the limiting reagent:** Compare the moles to establish which reactant is in excess.4. **Calculate the amount of acetic acid neutralized:** KOH will neutralize an equivalent amount of acetic acid.5. **Find the new concentrations after the reaction** using: \[ \text{Final Volume} = \text{Initial Volume of Acid + Volume of KOH} \]6. **Use the Henderson-Hasselbalch equation** to find pH: \[ \text{pH} = pK_a + \log \left( \frac{[\text{Conjugate Base}]}{[\text{Acid}]} \right) \]

Here we are required to find the PH of the solution .

An analytical chemist is titrating 64.7 mL of a 0.8500M solution of acetic acid (HCH₂CO₂) with a 0.2700M solution of KOH. The pK, of acetic acid is 4.70. Calculate the pH of the acid solution after the chemist has added 56.9 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pH = 0 X OL S

An analytical chemist is titrating 64.7 mL of a 0.8500M solution of acetic acid (HCH₂CO₂) with a 0.2700M solution of KOH. The pK, of acetic acid is 4.70. Calculate the pH of the acid solution after the chemist has added 56.9 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pH = 0 X OL S

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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