Question     (Requires Microsoft Excel) Use the spreadsheet approach described in Section 11-10 to generate the titration curve for the titration of \( 50.0 \mathrm{~mL} \) of \( 0.200 \mathrm{M} \) propanoic acid with \( 0.100 \mathrm{M} \mathrm{NaOH} \) from question 2. 2. You are titrating \( 50.0 \mathrm{~mL} \) of \( 0.200 \mathrm{M} \) propanoic acid with \( 0.100 \mathrm{M} \mathrm{NaOH} \). Use the data in the table to answer the questions. a) Assuming that the equivalence point is considered \( 100 \% \) completion, calculate the \( \mathrm{pH} \) at the following points: \( 0 \%, 10 \%, 50 \%, 90 \%, 100 \% \), and \( 120 \% \). b) Sketch the titration curve. c) What would be an ideal \( \mathrm{p} K_{\mathrm{a}} \) for an indicator to use in this titration?

TN3SVZ The Asker · Chemistry

 

 

Transcribed Image Text: (Requires Microsoft Excel) Use the spreadsheet approach described in Section 11-10 to generate the titration curve for the titration of \( 50.0 \mathrm{~mL} \) of \( 0.200 \mathrm{M} \) propanoic acid with \( 0.100 \mathrm{M} \mathrm{NaOH} \) from question 2. 2. You are titrating \( 50.0 \mathrm{~mL} \) of \( 0.200 \mathrm{M} \) propanoic acid with \( 0.100 \mathrm{M} \mathrm{NaOH} \). Use the data in the table to answer the questions. a) Assuming that the equivalence point is considered \( 100 \% \) completion, calculate the \( \mathrm{pH} \) at the following points: \( 0 \%, 10 \%, 50 \%, 90 \%, 100 \% \), and \( 120 \% \). b) Sketch the titration curve. c) What would be an ideal \( \mathrm{p} K_{\mathrm{a}} \) for an indicator to use in this titration?
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Transcribed Image Text: (Requires Microsoft Excel) Use the spreadsheet approach described in Section 11-10 to generate the titration curve for the titration of \( 50.0 \mathrm{~mL} \) of \( 0.200 \mathrm{M} \) propanoic acid with \( 0.100 \mathrm{M} \mathrm{NaOH} \) from question 2. 2. You are titrating \( 50.0 \mathrm{~mL} \) of \( 0.200 \mathrm{M} \) propanoic acid with \( 0.100 \mathrm{M} \mathrm{NaOH} \). Use the data in the table to answer the questions. a) Assuming that the equivalence point is considered \( 100 \% \) completion, calculate the \( \mathrm{pH} \) at the following points: \( 0 \%, 10 \%, 50 \%, 90 \%, 100 \% \), and \( 120 \% \). b) Sketch the titration curve. c) What would be an ideal \( \mathrm{p} K_{\mathrm{a}} \) for an indicator to use in this titration?
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YY4BIQ

【General guidance】The answer provided below has been developed in a clear step by step manner.Step1/3To calculate the pH at various points in the titration, we need to determine the number of moles of propanoic acid that have reacted with the NaOH. We can do this using the balanced chemical equation for the reaction:C3H5COOH + NaOH -> C3H5COO- Na+ + H2Omoles of NaOH added = 0.100 M x volume of NaOH added= 0.100 M x 50.0 mL= 0.00500 moles NaOHmoles of propanoic acid reacted = 0.200 M x 50.0 mL - 0.00500 moles NaOH= 0.00950 moles propanoic acidWe can use an ICE table to calculate the pH at each point in the titration:i) Before any NaOH is added (0% completion):Initial: 0.200 M propanoic acid, 0.000 M NaOHChange: -x, +x, +xEquilibrium: 0.200-x M propanoic acid, x M propanoate ion, x M NaOHK_a = 1.3 x 10^-5pH = pK_a + log([propanoate ion]/[propanoic acid])pH = 4.87 + log(0/0.200)pH = 4.87Explanation: ... See the full answer