QUESTION 8A 0.9600 M NAOH solution was diluted with a factor of 4.Then the diluted solution of NaOH was titrated against an unknown acld.The volumes of NaOH(aq) titrated are shown in the table below.Volumes of NaOH(aq):RoughtitrationFirsttitrationThirdtitrationSecondThirdtitrationtitrationFinal burette reading:(mL)Initial burette reading:(mL)19.0034.0520.8636.0123.5719.0019.075.7621.028.54The molarity of the unknown acid is 0.08108 M and the volume of the unknown acid used ineach titration is 14.80 mL.Was the unknown acid monoprotic, diprotic or triprotic? Show your calculations andreasoning.(i)

Answer :- Triprotic The given Unknow acid is triprotic…

A 0.9600 M NAOH solution was diluted with a factor of 4. Then the diluted solution of NAOH was titrated against an unknown acld. The volumes of NaOH(aq) titrated are shown in the table below. Volumes of NaOH(aq): Rough titration First titration Second titration Third titration Third titration Final burette reading: (mL) Initial burette reading: (mL) 19.00 34.05 20.86 36.01 23.57 19.00 19.07 5.76 21.02 8.54 The molarity of the unknown acid is 0.08108 M and the volume of the unknown acid used in each titration is 14.80 mL. Was the unknown acid monoprotic, diprotic or triprotic? Show your calculations and reasoning. (i)

A 0.9600 M NAOH solution was diluted with a factor of 4. Then the diluted solution of NAOH was titrated against an unknown acld. The volumes of NaOH(aq) titrated are shown in the table below. Volumes of NaOH(aq): Rough titration First titration Second titration Third titration Third titration Final burette reading: (mL) Initial burette reading: (mL) 19.00 34.05 20.86 36.01 23.57 19.00 19.07 5.76 21.02 8.54 The molarity of the unknown acid is 0.08108 M and the volume of the unknown acid used in each titration is 14.80 mL. Was the unknown acid monoprotic, diprotic or triprotic? Show your calculations and reasoning. (i)

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

85.0 mL of 0.375 M HNO3 is titrated by 0.750 M KOH. Calculate the pH of the acid solution before any titrant is added. pH = Calculate the pH after 35.92 mL of 0.750 M KOH is added to 85.0 mL of 0.375 M HNO3. pH = Calculate the pH after 42.50 mL of 0.750 M KOH is added to 85.0 mL of 0.375 M HNO3. pH = Calculate the pH after 83.5 mL of 0.750 M KOH is added to 85.0 mL of 0.375 M HNO3. pH = (Please type answer not write by hend)
A 28.00 mLmL sample of an H2SO4H2SO4 solution of unknown concentration is titrated with a 0.1422 MM KOHKOH solution. A volume of 43.22 mLmL of KOHKOH was required to reach the equivalence point. What is the concentration of the unknown H2SO4H2SO4 solution? Express your answer using four significant figures.
Please explain to me how to find the blank boxes. This is for an experiment that titrated an antacid tablet (mass of solid=500 mg) containing the base CaCO3 dissolved in 50 mL of 0.30 M HCl. Then a burette was filled to the 0 mark of a burette (so 50 mL in the burette) of 0.30 M NaOH and the NaOH was titrated into the HCl solution containing the antacid tablet.
A 29.00 mLmL sample of an H2SO4H2SO4 solution of unknown concentration is titrated with a 0.1372 MM KOHKOH solution. A volume of 41.22 mLmL of KOHKOH was required to reach the equivalence point. What is the concentration of the unknown H2SO4H2SO4 solution? Express your answer using four significant figures.
A buffer system is prepared by combining 0.603 moles of ammonium chloride (NH4CI) and 0.713 moles of ammonia (NH3). What will the solution pH be if 0.239 moles of the nitric acid (HNO3) is added to the solution. Nitric acid is a strong acid. The K₁ of ammonia is 1.8 x 10-5. (Two decimal places)
A titration is carried out for 50.00 mL of 0.100 M HNO3 (strong acid) with 0.200 M of a strong base NaOH (the titration curve is shown to the right). Calculate the pH at these volumes of added base solution: A B C D 0.200 M NaOH added 00.0 mL 15.0 mL 25.0 mL 40.0 mL HNO3(aq) + NaOH(aq) H₂O(9) + NaNO3(aq) pH of solution - Equivale point Midpoint HAlaq). Volume c
Please don't provide handwritten solution ....
What weight of soda ash must be taken for analysis so that by using 0.5000N HCl for titrating, (a) buret reading will equal the percentage of Na2O, (b) three times the buret reading will equal the percentage of Na2O, (c) every 3 mL will represent 1% Na2O (d) each mL will represent 3% Na2O (e) the buret reading and the percentage of Na2O will be in the respective ratio 2:3? pls answer letter d and e
Consider the titration of 100.0 mL of 0.100 M NaOH with 1.00 M HBr. Find the pH at the following volumes of acid added. See the picture below. Kindly answer all the questions, thanks!