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Question 2 Use the following information to answer the question. A technician prepares 500 mL of a 0.100 mol/L solution of acetic (ethanoic) acid by diluting a concentrated solution of acetic acid with water. The equilibrium equation that represents the reaction that occurs when acetic acid and water react is shown below. CH,COOH(aq) + H₂O(1)→ CH₂C00¹ (aq) + H₂0¹(aq) a. For the prepared acetic acid solution, calculate the concentration of H₂O*(aq) and the pH. CH₂COOH + H₂0 → сносоо + НО V= 0.5L 40.100201/1 n=cv-> (0-100) (0.5)=>0.05 mol · ===0 عا neo.osnid = 0.05 mol

Question 2 Use the following information to answer the question. A technician prepares 500 mL of a 0.100 mol/L solution of acetic (ethanoic) acid by diluting a concentrated solution of acetic acid with water. The equilibrium equation that represents the reaction that occurs when acetic acid and water react is shown below. CH,COOH(aq) + H₂O(1)→ CH₂C00¹ (aq) + H₂0¹(aq) a. For the prepared acetic acid solution, calculate the concentration of H₂O*(aq) and the pH. CH₂COOH + H₂0 → сносоо + НО V= 0.5L 40.100201/1 n=cv-> (0-100) (0.5)=>0.05 mol · ===0 عا neo.osnid = 0.05 mol

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter3: Chemical Reactions
Section: Chapter Questions
Problem 87SCQ: Most naturally occurring acids are weak acids. Lactic acid is one example....
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Question 2 Use the following information to answer the question. A technician prepares 500 mL of a 0.100 mol/L solution of acetic (ethanoic) acid by diluting a concentrated solution of acetic acid with water. The equilibrium equation that represents the reaction that occurs when acetic acid and water react is shown below. CH,COOH(aq) + H₂O(1) CH,CO0¹ (aq) + H₂O*(aq) a. For the prepared acetic acid solution, calculate the concentration of H3O*(aq) and the pH. CH₂COOH + H₂O. → CH₂COO H30 V= 0.5L C0.100m0111 n=cv-> (0-100) (0.5) => 0.05 mol = =0.0smol. neo 05 nul Show Transcribed Text Use the following additional information to answer the next part of the question. A technician uses the 500 mL of 0.100 mol/L acetic acid to prepare an acetic acid-sodium acetate buffer solution. She does this by adding 0.100 mol/L sodium acetate to the 0.100 mol/L acetic acid until the required pH is reached. b. Identify the shift in equilibrium that will occur when sodium acetate is added to the equilibrium reaction. Predict whether or not there is an effect on the equilibrium constant and if so, what the effect on the equilibrium constant is. c. If small quantities of aqueous sodium hydroxide are added to the buffer solution, predict whether the pH of the acetic acid-sodium acetate buffer solution will change or stay the same. Explain your answer.
Transcribed Image Text:Question 2 Use the following information to answer the question. A technician prepares 500 mL of a 0.100 mol/L solution of acetic (ethanoic) acid by diluting a concentrated solution of acetic acid with water. The equilibrium equation that represents the reaction that occurs when acetic acid and water react is shown below. CH,COOH(aq) + H₂O(1) CH,CO0¹ (aq) + H₂O*(aq) a. For the prepared acetic acid solution, calculate the concentration of H3O*(aq) and the pH. CH₂COOH + H₂O. → CH₂COO H30 V= 0.5L C0.100m0111 n=cv-> (0-100) (0.5) => 0.05 mol = =0.0smol. neo 05 nul Show Transcribed Text Use the following additional information to answer the next part of the question. A technician uses the 500 mL of 0.100 mol/L acetic acid to prepare an acetic acid-sodium acetate buffer solution. She does this by adding 0.100 mol/L sodium acetate to the 0.100 mol/L acetic acid until the required pH is reached. b. Identify the shift in equilibrium that will occur when sodium acetate is added to the equilibrium reaction. Predict whether or not there is an effect on the equilibrium constant and if so, what the effect on the equilibrium constant is. c. If small quantities of aqueous sodium hydroxide are added to the buffer solution, predict whether the pH of the acetic acid-sodium acetate buffer solution will change or stay the same. Explain your answer.
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