### Titration Problem on Calculating pH**Problem Statement:**An analytical chemist is titrating 56.7 mL of a 0.4900 M solution of formic acid ($H_2CO_2$) with a 0.7500 M solution of KOH. The $pK_a$ of formic acid is 3.74. Calculate the pH of the acid solution after the chemist has added 44.2 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.**Calculation:**1. **Determine moles of formic acid and KOH:** - Moles of formic acid = $0.4900 \, M \times 0.0567 \, L = 0.027783 \, moles$ - Moles of KOH = $0.7500 \, M \times 0.0442 \, L = 0.03315 \, moles$2. **Neutralization:** Since $KOH$ is a strong base, it will neutralize an equivalent amount of formic acid. The moles of formic acid will decrease by the number of moles of $KOH$ added: - Remaining moles of formic acid = $0.027783 \, moles - 0.03315 \, moles = -0.005367 \, moles$ Since the moles of $KOH$ exceed the moles of formic acid, formic acid is completely neutralized and excess $KOH$ remains in the solution.3. **Calculating the concentration of $OH^-$ ions:** - Excess moles of $KOH$ = $0.03315 \, moles - 0.027783 \, moles = 0.005367 \, moles$ - Total volume of the solution = $56.7\, mL + 44.2\, mL = 100.9\, mL = 0.1009\, L$ - Concentration of $KOH$ = \(\frac{0.005367 \, moles

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An analytical chemist is titrating 56.7 mL of a 0.4900M solution of formic acid (H,CO,) with a 0.7500M solution of KOH. The p K, of formic acid is 3.74. Calculate the pH of the acid solution after the chemist has added 44.2 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 =

An analytical chemist is titrating 56.7 mL of a 0.4900M solution of formic acid (H,CO,) with a 0.7500M solution of KOH. The p K, of formic acid is 3.74. Calculate the pH of the acid solution after the chemist has added 44.2 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 =

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 114CWP: Consider the following acids and bases: HCO2H Ka = 1.8 104 HOBr Ka = 2.0 109 (C2H5)2NH Kb = 1.3 ...

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