### Titration Problem - Calculating pHAn analytical chemist is titrating 238.1 mL of a 0.5500 M solution of propionic acid (\(HC_2H_5CO_2\)) with a 0.8000 M solution of KOH. The \(pK_a\) of propionic acid is 4.89. Calculate the pH of the acid solution after the chemist has added 119.8 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.**Instructions:** Round your answer to 2 decimal places and enter it in the provided box.**pH Calculation Box:**\[ \text{pH} = \boxed{} \]### Explanation:In this problem, we are dealing with a titration of a weak acid (propionic acid) with a strong base (KOH). The objective is to calculate the pH after the addition of a specific volume of KOH.### Detailed Solution Approach:1. **Determine the moles of propionic acid and KOH:** - Moles of propionic acid (\(HC_2H_5CO_2\)): \( \text{Molarity} \times \text{Volume} = 0.5500 \, M \times 0.2381 \, L = 0.130955 \, \text{moles} \) - Moles of KOH: \( \text{Molarity} \times \text{Volume} = 0.8000 \, M \times 0.1198 \, L = 0.09584 \, \text{moles} \)2. **Calculate the remaining moles of \(HC_2H_5CO_2\) and produced moles of \(HC_2H_5CO_2^- \):** - Stoichiometry: \(HC_2H_5CO_2H + OH^- \rightarrow HC_2H_5CO_2^- + H_2O \) - Moles of \(HC_2H_5CO_2H\) after reaction: \(0.130955 - 0.09584 = 0.035115 \, \text{moles}\

Answered: Image /qna-images/answer/87134b5f-e833-41ef-a254-0cf27a80b812.jpg

An analytical chemist is titrating 238.1 mL of a 0.5500M solution of propionic acid (HC₂H₂CO₂) with a 0.8000M solution of KOH. The p K of propionic acid is 4.89. Calculate the pH of the acid solution after the chemist has added 119.8 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 = X

An analytical chemist is titrating 238.1 mL of a 0.5500M solution of propionic acid (HC₂H₂CO₂) with a 0.8000M solution of KOH. The p K of propionic acid is 4.89. Calculate the pH of the acid solution after the chemist has added 119.8 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 = X

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...

See similar textbooks

Similar questions

An analytical chemist is titrating 127.5 mL of a 0.5600 M solution of cyanic acid (HCNO) with a 0.4600 M solution of NaOH. The p K of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 74.40 mL of the NaOH a solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = | ?
For the titration of 50. mL of 0.10 M ammonia with 0.10 M HCI, calculate the pH. For ammonia, NH3, Kp = 1.8 x 10-5. (a) Before the addition of any HCl solution. pH = Use correct number of significant digits; (b) After 20. mL of the acid has been added. pH = Use correct number of significant digits; (c) After half of the NH3 has been neutralized. pH Use correct number of significant digits; (d) At the equivalence point. pH Use correct number of significant digits;
A chemist titrates 90.0 mL of a 0.4988 M butanoic acid (HC3H,CO₂) solution with 0.0732M KOH solution at 25 °C. Calculate the pH at equivalence. The p K of butanoic acid is 4.82. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of KOH solution added. pH = X S
Please be correct!!
A chemist titrates 230.0 mL of a 0.5989 M butanoic acid (HC₂H,CO₂) solution with 0.6911 M KOH solution at 25 °C. Calculate the pH at equivalence. The PK of butanoic acid is 4.82. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of KOH solution added. pH = 0 X` S
The pH of a bicarbonate-carbonic acid buffer is 6.18. Calculate the ratio of the concentration of carbonic acid (H2CO3) to that of the bicarbonate ion (HCO3−). (Ka1 of carbonic acid is 4.2 × 10−7.)
An analytical chemist is titrating 83.7 mL of a 0.3300M solution of isopropylamine ((CH,) CHNH, with a 0.5300M 2 solution of HNO3. The p K, of isopropylamine is 3.33. Calculate the pH of the base solution after the chemist has added 42.4 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = | ?
An analytical chemist is titrating 144.6 mL of a 0.6600 M solution of benzoic acid (HC H,CO,) with a 0.8400 M solution of KOH. The p K, of benzoic acid is 4.20. Calculate the pH of the acid solution after the chemist has added 54.06 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
When a 23.3 mL sample of a 0.379 M aqueous hypochlorous acid solution is titrated with a 0.407 M aqueous sodium hydroxide solution,(1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 32.5 mL of sodium hydroxide have been added?
An analytical chemist is titrating 225.8 mL of a 0.5300 M solution of butanoic acid (HC,H,CO,) with a 0.8200 M solution of KOH. The p K, of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 40.67 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 = ||
3. Please help me answer all parts to this chemistry question:
An analytical chemist is titrating 111.5 mL of a 0.2600M solution of acetic acid (HCH,CO,) with a 0.5100M solution of NaOH. The p K, of acetic acid is 4.70. Calculate the pH of the acid solution after the chemist has added 10.45 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = |