To assay a chlorquine tablet having an average weightof 334.3 mg with dosage strength of 250 mgchloroquine phosphate 0.1 M perchloric acid was used.2.0669 mg of potassium hydrogen phthalatewasdissolved to 100 mL and 25 mL of the resultant solutionwas used to to standardize the 0.1 Molar perchloricacid. The titre volume observed was 25.9 mL. Blank titrevolume of 0.2 mL was observed. 660.6 mg of well-grounded chloroquine power was dissolved to n 50 mL.25 mL of thesolution was pipetted and used for thetitration .9.3 mL of the perchlirc acid was observed astitre volume and blank titration was 0.3 mL of theperchloric acid. (i) Calculate the milliequivalent of thechloroquine phosphate giving that the balancedreaction of chloroquine phosphate is C18H26CIN32H3PO4 + 2HCLO4 - C18H26CIN3H2^2+ + 2CLO4. (ii)Calculate the assay value of chloroquine phosphate inthe test sample. in Chemistry

To calculate the milliequivalents of chloroquine phosphate and the assay value of chloroquine…

Answered: To assay a chlorquine tablet having an…

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...

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c) Give an example of a complexometric titration with equations explaining the reactions that occur. Include the role played by dye acting as indicator.
Which type of indicator is used in permanganatometry titrant plays role of indicator by itself; irreversible Red/Ox indicator; reversible Red/Ox indicator; metallochrome indicator;
I made some titrations and the calculated molarity of HCI was 0.096, 0.097 and 0.098. The nomical concentrsrion of HCl is 0.1. How can I explain my results by comparing it to the nominal concentration if my confidence intervals don't include the nominal concentration?
A 250-mL buffer solution contains 0.0510 mole of KH2PO4 and 0.0875 mole of K2HPO4. (a) Calculate the molar concentrations of H2PO4–and HPO42–, respectively, in thesolution. (b) What is the pH of the solution? (H2PO4– has Ka = 6.2 x 10–8) (c) Write a net ionic equation for the buffering reaction against a strong acid by this buffer. (d) If 0.012 mole of hydrochloric acid (HCl) is added to the solution, create a reaction table to show the buffering reaction and calculate the molar concentration of H2PO4–and HPO42–, respectively, in the resulting solution after the buffering reaction. (e) What is the pH of the resulting solution?
The following titration curve shows the titration of triethylamine (C,H5)3N with hydrochloric acid. Which net ionic reaction explains the pH of the analyte solution before any titrant is added? 12 10 6. PH 4. 1. 10 50 mL of HCI 30 70 90 110 (CH;)3NH"(aq) + H,0(1) (C,Hg)gN(aq) + H3O*(aq) O C,H;)3N(aq) + H3O*(aq) (CH5)3NH*(aq) +OH (aq) (C2H5)3N(aq) + H*(aq) -> (C,H5)3NH"(aq) O H2O(1) H*(aq) + OH (aq) --> (C2H;)3N(aq) + H,0(1) OH (aq) + (CH5)3NH*(aq)
The pH at 10, 100, and 110% titration (% of the equivalence point volume) for the titration of 50.0mL of 0.100 M HCI with 0.10OM NaOH at 10=1.09 , at 100= 11.00 O at 10=1.09 , at 100= 10.68 at 10=1.09 , at 100= 12.68
A 1.0 g sample containing urea was dissolved in water and diluted in a 100.00 mL volumetric flask. 20.00 mL aliquot was mixed with 30.00 mL water and subjected to digestion with concentrated H2SO4. The ammonia produced is collected in 30.00 mL of 0.0500 M HCl and the excess acid is back titrated with 0.0500 M NaOH, requiring 6.80 mL. Calculate the weight percent urea [(NH2)2CO, FW=60.06 g/mol] in the sample.
A 1.0 g sample containing urea was dissolved in water and diluted in a 100.00 mL volumetric flask. 20.00 mL aliquot was mixed with 30.00 mL water and subjected to digestion with concentrated H2SO4. The ammonia produced is collected in 30.00 mL of 0.0500 M HCl and the excess acid is back titrated with 0.0500 M NaOH, requiring 6.80 mL. Calculate the weight percent urea [(NH2)2CO, FW=60.06 g/mol] in the sample. Please use the factor label method in answering.
A sample may contain NaOH, NazCO3 and NaHCO3, alone or in some combination, along with inert material. A samplewitha mass of 857.6 mgwas dissolved and titrated with0.1163 M HCI. The volume of HCl used from 0 to methyl red endpoint (Phenolphthalein endpoint was not monitored here) was found to be 36.54 mL. Another 228.8 mg portion of the sample was titrated to the phenolphthalein endpoint and 10.82 mL was used up for this titration. a. What is the composition of the sample? b. Calculate the percentage of each of the component present.
7.5mL of 333mM Tris was added to 192.5ml of water. The resulting solution was added to 240mL of water and the pH was adjusted to 8.0 using 10mL of HCl. A further 33.3mL of water was added. What is the concentration of the final solution (in millimolar)? The MW of Tris is 121.14
If a 3g sample of zinc oxide, 95% ZnO, were treated with 50ml of 1.1230N sulfuric acid in the usual way, what volume of 0.9765N sodium Hydroxide would be required in the residual titration?
I want the answer for Q2

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