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3, The molor mass and ionization constant of an unknowm weak monopronc acta Concentration of standardized NaOH titrant 00 mol/L 2029/ Mass concentration of unknown weak monoprotic acid 2402 Tridl3 7.60 mL Trial 1 Trial 2 8.12 30.0 Measured pi of the unknown acid solution 3.42 in kal b.30 30.0 14 21.9 139 Vol Mads of unknown acid solution taken for titration 14. mL 27.6ML Initial buret reading of NaOH titrant ml ml 13.5 13.5 Final buret reading of NaOH titrant ml ml Net volume of NaOH ml ml 13.bmL Millimoles of NaOH to end point of titration mmol mmol Millimoles of unknown acid in sample mmol mmol eash Molar concentration of unknown acid solution mol/L mol/L Calculated molar mass of unknown acid g/mol R/mol Calculation of the lonization constant for an unknown acid from the measured pH of the unknown acid samples. (Average the pH and molar concentration values for the samples of unknown acid you titrated; use the average values in the calculation of the lonization constant.) Average molar concentration of unknown for the samples you titrated 13.7 mol/L Average pH6.85 Calculate the corresponding [H,O'), compute the concentration ofA and HA, and calculate the dissociation constant, K MH,O MA M HA K - 0A. (HA pK,-

3, The molor mass and ionization constant of an unknowm weak monopronc acta Concentration of standardized NaOH titrant 00 mol/L 2029/ Mass concentration of unknown weak monoprotic acid 2402 Tridl3 7.60 mL Trial 1 Trial 2 8.12 30.0 Measured pi of the unknown acid solution 3.42 in kal b.30 30.0 14 21.9 139 Vol Mads of unknown acid solution taken for titration 14. mL 27.6ML Initial buret reading of NaOH titrant ml ml 13.5 13.5 Final buret reading of NaOH titrant ml ml Net volume of NaOH ml ml 13.bmL Millimoles of NaOH to end point of titration mmol mmol Millimoles of unknown acid in sample mmol mmol eash Molar concentration of unknown acid solution mol/L mol/L Calculated molar mass of unknown acid g/mol R/mol Calculation of the lonization constant for an unknown acid from the measured pH of the unknown acid samples. (Average the pH and molar concentration values for the samples of unknown acid you titrated; use the average values in the calculation of the lonization constant.) Average molar concentration of unknown for the samples you titrated 13.7 mol/L Average pH6.85 Calculate the corresponding [H,O'), compute the concentration ofA and HA, and calculate the dissociation constant, K MH,O MA M HA K - 0A. (HA pK,-

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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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3. The molar mass and ionization constant of an unknown weak monoprohć öčid Concentration of standardized NaOH titrant .100 mol/L 2 407-9/ Mass concentration of unknown weak monoprotic acid 240 2 g/L Tridl3 7.60 vmL Trial 1 Trial 2 ut Measured pH of the unknown acid solution 3.42 in kal 6.30 8.12 30.0 30.0 14 27.9 139 vol Mass of unknown acid solution taken for titration 14. mL 27.6 ML 13.bmL Initial buret reading of NaOH titrant ml mL Final buret reading of NAOH titrant 13.5 13.5 ml mL Net volume of NAOH ml mL W. Millimoles of NaOH to end point of titration mmol mmol Millimoles of unknown acid in sample eash mmol mmol Molar concentration of unknown acid solution mol/L mol/L Calculated molar mass of unknown acid g/mol g/mol Calculation of the lonization constant for an unknown acid from the measured pH of the unknown acid samples. (Average the pH and molar concentration values for the samples of unknown acid you titrated; use the average values in the calculation of the lonization constant.) Average molar concentration of unknown for the samples you titrated 13.7 mol/L Average pHO.85 Calculate the corresponding (H,0), compute the concentration of A and HA, and calculate the dissociation constant, K it th MH,0 MA M HA K, (HA pk,-
Transcribed Image Text:3. The molar mass and ionization constant of an unknown weak monoprohć öčid Concentration of standardized NaOH titrant .100 mol/L 2 407-9/ Mass concentration of unknown weak monoprotic acid 240 2 g/L Tridl3 7.60 vmL Trial 1 Trial 2 ut Measured pH of the unknown acid solution 3.42 in kal 6.30 8.12 30.0 30.0 14 27.9 139 vol Mass of unknown acid solution taken for titration 14. mL 27.6 ML 13.bmL Initial buret reading of NaOH titrant ml mL Final buret reading of NAOH titrant 13.5 13.5 ml mL Net volume of NAOH ml mL W. Millimoles of NaOH to end point of titration mmol mmol Millimoles of unknown acid in sample eash mmol mmol Molar concentration of unknown acid solution mol/L mol/L Calculated molar mass of unknown acid g/mol g/mol Calculation of the lonization constant for an unknown acid from the measured pH of the unknown acid samples. (Average the pH and molar concentration values for the samples of unknown acid you titrated; use the average values in the calculation of the lonization constant.) Average molar concentration of unknown for the samples you titrated 13.7 mol/L Average pHO.85 Calculate the corresponding (H,0), compute the concentration of A and HA, and calculate the dissociation constant, K it th MH,0 MA M HA K, (HA pk,-
Unknown Measurement of the pk, of an unknown acid by the half-neutralization method Concentration of standardized NaOH titrant mol/L 100 Trial 1 Trial 2 Not Mass of unknown acid solution 30-0 m 30-0 mL Volume of NaOH added to half-neutralize the unknown acid 6-85 4.92 6.85 4.91 mL mL Measured pH of half-neutralized solution 4.915 Average pH value pk, K, = Calculate the (H,0] and the concentration of A" and HA, In the half-neutralized solution. (Note: In this solution, (H,0'] [A ]) M H,0* MA M HA Comparing both the calculated molar mass and the lonization constant, which acid in Table 6 of the Appendix is the unknown acid most likely to be? Give the molar mass and pK, for the unknown acid that you measured: Give the molar mass and K, for the acid listed in Table 6 of the Appendix that you think is the same as your unknown acid.
Transcribed Image Text:Unknown Measurement of the pk, of an unknown acid by the half-neutralization method Concentration of standardized NaOH titrant mol/L 100 Trial 1 Trial 2 Not Mass of unknown acid solution 30-0 m 30-0 mL Volume of NaOH added to half-neutralize the unknown acid 6-85 4.92 6.85 4.91 mL mL Measured pH of half-neutralized solution 4.915 Average pH value pk, K, = Calculate the (H,0] and the concentration of A" and HA, In the half-neutralized solution. (Note: In this solution, (H,0'] [A ]) M H,0* MA M HA Comparing both the calculated molar mass and the lonization constant, which acid in Table 6 of the Appendix is the unknown acid most likely to be? Give the molar mass and pK, for the unknown acid that you measured: Give the molar mass and K, for the acid listed in Table 6 of the Appendix that you think is the same as your unknown acid.
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