Exercise Construct a titration curve by plotting pH vs. VNaOH added. HCl(aq) + NaOH(aq) H₂O(1) + NaCl(aq) Volume NaOH (mL) [H'] pH 0.00 5.00 10.00 15.00 20.00 25.00 30.00 35.00 40.00 45.00 48.00 50.00 52.00 55.00 60.00 65.00 70.00 75.00 80.00 85.00 90 95 100 1×10¹ Hints: The pH of the solution is calculated using the following equations: (a) Initial conditions (VNaOH = 0), [H"]=[HCI] (b) After initial addition of NaOH and before the end point: [H]=Mc-Man V V/ LV (c) At the end point (Vsaou 50 mL), all the HC1 is being consumed and the acidity of the solution comes from auto ionization of water which is: [H]-1-10 (d) After the end point: 1x 10-¹4 MXV NOW VO+VY [H"]= ABERDEELC titrant: NaOH, 0.IM Question 1) What is the pH when the solution volume in the flask reaches 95 ml? a. 12.79 b. 12.82 c. 1.95 d. 12. 75e. 2.28 Question2) What is the maximum pH reached at the end of titration? a. 12.77b. 12.79c. 12.81 d. 12. 78 e. 12.82 analyte: HC1, 0.1 M, 50 ml.

Exercise Construct a titration curve by plotting pH vs. VNaOH added. HCl(aq) + NaOH(aq) H₂O(1) + NaCl(aq) Volume NaOH (mL) [H'] pH 0.00 5.00 10.00 15.00 20.00 25.00 30.00 35.00 40.00 45.00 48.00 50.00 52.00 55.00 60.00 65.00 70.00 75.00 80.00 85.00 90 95 100 1×10¹ Hints: The pH of the solution is calculated using the following equations: (a) Initial conditions (VNaOH = 0), [H"]=[HCI] (b) After initial addition of NaOH and before the end point: [H]=Mc-Man V V/ LV (c) At the end point (Vsaou 50 mL), all the HC1 is being consumed and the acidity of the solution comes from auto ionization of water which is: [H]-1-10 (d) After the end point: 1x 10-¹4 MXV NOW VO+VY [H"]= ABERDEELC titrant: NaOH, 0.IM Question 1) What is the pH when the solution volume in the flask reaches 95 ml? a. 12.79 b. 12.82 c. 1.95 d. 12. 75e. 2.28 Question2) What is the maximum pH reached at the end of titration? a. 12.77b. 12.79c. 12.81 d. 12. 78 e. 12.82 analyte: HC1, 0.1 M, 50 ml.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 51P

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A chemistry student is studying the effect of buffers. During his experiment, he collected the following data. However, is advisor informed him that his conclusions were incorrect. What are the likely conclusions the student provided that led to his advisor telling him this? (Select all that apply) Moles of pH of pH of buffer pH of buffer HCI water added (0.10 M HA/ (0.20 M HA/ Select 2 correct answer(s) 0.10 MA) 0.20 MA) O Buffer 2 is more concentrated, so its capacity to resist to changes in pH is higher than Buffer 1. 7.00 4.74 4.74 10-6 6.00 4.74 4.74 Any concentration of HCl will decrease the pH of water, while high concentrations of HCl is needed to change the pH of a buffer. 10-5 5.00 4.74 4.74 10-4 4.00 4.74 4.74 O Buffer 1 is less concentrated, so its capacity to resist changes in pH is higher than Buffer 2. 10-3 3.00 4.74 4.74 10-2 2.00 4.66 4.70 Adding HCl will increase the pH of water, but not the pH of the buffers 10-1 1.00 2.72 4.27
Exercise Construct a titration curve by plotting pH vs. VNaOH added. HCl(aq) + NaOH(aq) H₂O(1) + NaCl(aq) Volume NaOH (mL) [H] pH 0.00 5.00 10.00 15.00 20.00 25.00 30.00 35.00 40.00 45.00 48.00 50.00 $2.00 55.00 60.00 65.00 70.00 75.00 80.00 85.00 90 95 100 What is the pH when the solution volume in the flask reaches 95 ml? O a 1279 Ob 12.82 OC 1.95 O d. 12.75 De 2.28 Hints: The pH of the solution is calculated using the following equations: (a) Initial conditions (VNaOH = 0), [H"]=[HCI] (b) After initial addition of NaOH and before the end point: MC VC-M NOVNO [H"]= V LV (c) At the end point (Vou 50 mL), all the HCI is being consumed and the acidity of the solution comes from auto ionization of water which is: [H]-1-10 (d) After the end point: 1x10-¹4 M Isel Boy XV V₁W+VIRY [H"]= titrant: NaOH, 0.1M analyte: HC1, 0.1 M, 50 ml.
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tation The following pH curve is for the titration of 20.0 mL of a 0.10 M solution of a weak monoprotic base with a 0.10 M solution of a strong monoprotic acid. 12.0 10.0 Data points at 1 mL increments. 8.0 Hd 6.0 4.0 2.0 0.0- 0.0 10.0 20.0 30.0 Volume of titrant (mL) 40.0 ܠܕ ܠܐ ܒ ܬ ܤ ܐ ܠܐ 50.0 CD
help with titration problem find total volume of NaOh added (mL)
v Question Completion Status: QUESTION 13 Consider an acid-base titration in which the base is dispenssd from a burette into a flask containing an acid. If any drops of the base adhere to the inner walls of the flask, but do not ackially mix with the solution, the calculated acid concentration would be O the same as the actual value. O lower than the actual value. O higher than the actual value. O Need more information QUESTION 14 What is the BEST numerical value for the quantity of liquid in the graduated cylinder? Save A Click Save and Submit to save and submit. Click Save All Answers to save all answers.
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Student perform titration experiment to determine the concentration of NaOH he can not reach the accurate end point which of the following statements is correct? a) He Did not add indicator b) He use Ba(OH), as standard solution c) He add the standard solution rapidly d) All the previous
Exercise Construct a titration curve by plotting pH vs. VNaOH added. HCl(aq) + NaOH(aq) H₂O(1) + NaCl(aq) Volume NaOH (mL) [H'] pH 0.00 5.00 10.00 15.00 20.00 25.00 30.00 35.00 40.00 45.00 48.00 50.00 52.00 55.00 60.00 65.00 70.00 75.00 80.00 85.00 90 95 100 1×107 Hints: The pH of the solution is calculated using the following equations: [H]= (a) Initial conditions (VNaOH = 0), [H] = [HCI] (b) After initial addition of NaOH and before the end point: [H]= MHCI VHCI-M VHCI + V NaOH 1x10-14 XV. titrant: NaOH, 0.1M (c) At the end point (VNaOH = 50 mL), all the HCI is being consumed and the acidity of the solution comes from auto ionization of water which is: [H"]=1x107 (d) After the end point: Mo analyte: HC1, 0.1 M, 50 ml. NaOH *V NaOH NaOff V +V₂C² NaOH