A 0.2985 g sample of an antibiotic powder was dissolved in HCl and the solution diluted to 100.0 mL. A20.00 ml aliquot was transferred to a flask and followed by 25.00 ml of 0.01886 M KBRO3. An excess ofKBr was added to form Br2, and the flask was stoppered. After 10 min, during which time the Br2brominated the sulfanilamide, an excess of KI was added. The liberated iodine titrated with 12.88 ml of0.1235 M sodium thiosulfate. Calculate the percent sulfanilamide (NH2C,H4SO2NH2) in the powder.Bro, + 5Br + 6H*3Br, + 3H,0NH2NH2Br.Br+ 2B12+ 2H++ 2BrSO,NH2SO,NH2sulfanilamideBr, + 512Br + 12excess2 + 25,0,-25,0,2 + 21--MM: NH2C6H4SO2NH2 = 172.21KBRO3= 167.00KBr119.00

The explanation is given below-

Answered: A 0.2985 g sample of an antibiotic…

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

43-45 An EDTA solution was prepared by dissolving approximately 4 g of the disodium salt in approximately 1 L of water. An average of 41.87 mL of this solution was required to titrate 50.00-mL aliquots of a standard that contained 0.6987 g of MgCO₃ (84.31 g/mol) per liter. Titration of a 25.00-mL sample of mineral water at pH 10 required 19.32 mL of the EDTA solution. A 50.00-mL aliquot of the mineral water was rendered strongly alkaline to precipitate the magnesium. Titration with a calcium-specific indicator required 30.27 mL of the EDTA solution. a) Calculate the molar concentration of the EDTA solution. b) Calculate concentration of CaCO₃ (100.09 g/mol) of the mineral water in ppm. c) Calculate concentration of MgCO₃ (84.31 g/mol) of the mineral water in ppm.
A 2.067 g of macrogol monostearate (average molecular weight 706. 5) was added to a 200 ml flask and 25 ml of an ethanolic solution of potassium hydroxide (molecular weight 56.11, ca 0.5 M) was added. The sample was heated under a reflux condenser for 1 hour. The excess of alkali was then titrated with 0.5126 M hydrochloric acid using phenolphthalein solution as an indicator. The operation was repeated without the macrogol monostearate. Results Volume of HCI required to titrate the excess alkali = 18.35 ml Volume of HCI required to titrate the blank = 24.03 ml Calculate the saponification value for the macrogol stearate. Answer: _____ mg/g
NH3 obtained when 0.5 g of an organic compound substance was subjected to Kjeldahl's method was neutralized by 10 mL of 1 N HCl. Estimate the composition (percentage) of nitrogen in the given organic compound. How can we eliminate CO₂ and H₂O in Dumas method ?
A 5.0 g sample containing a pesticide with molecular formula [C14H9Cl5], was decomposed with metallic sodium in alcohol, and the liberated chloride ion was precipitated as AgCl. (i) Express the results of this analysis in terms of percent based on the recovery of 0.1606 g of AgCl. (ii) Convert your answer (g/g) to ppm.
How many covalent bonds are predicted for an atom of N? Enter your answer in the provided box.
A 28.93 mL aliquot of trimethylamine that has a concentration of 0.661 M will be titrated with 0.752 M HCl. Calculate the pH of the solution upon the addition of 32.6 mL of HCl. The Kb at the temperature of the experiment is equal to 6.11 x 10-5. Kw = 1.00 x 10-14
5 The amount of ascorbic acid, C6HSO6, in orange juice was determined by oxidizing the ascorbic acid to dehydroascorbic acid, C6H6O6, with a known excess of I3, and back titrating the excess Is with Na2S2O3. A 5.00-mL sample of filtered orange juice was treated with 50.00 mL of excess 0.01023 M I3. After the oxidation was complete, 13.82 mL of 0.07203 M NazS2O3 was needed to reach the starch indicator end point. Report the concentration of ascorbic acid in milligrams per 100 mL.
A solid containing tris was dissolved in water and brought to a total volume of 50.00 ml. A 10.00 ml aliquot of the solution was titrated with 0.09978 M HCl to a bromcresol green endpoint. The aliquot consumed 38.93 ml of titrant. Calculate the weight of tris in the original sample.
In a reaction involving the iodination of acetone, the following reaction mixture was used: 5.00mL 4.0M acetone, 5.00mL 1.0 M HCl, 5.00mL 0.0050 M I2, and 10.0 mL water. what was the molarity of the acetone in the reaction mixture? (Recall that M1V1=M2V2) the color of the above reaction mixture disappeared in 250 seconds. What was the rate of the reaction?
You prepare a buffer solution from 10.0 mL of 0.100M MOPS (3‑morpholinopropane‑1‑sulfonic acid) and 10.0 mL of 0.075 M NaOH. Next, you add 1.00 mL of 4.15×10−4 M lidocaine to this mixture. Denoting lidocaine as L, calculate the fraction of lidocaine present in the form LH+. MOPS Ka = 6.3 * 10^-8 Lidocaine Kb = 8.7 * 10^-7 ( Please type answer note write by hend )
Using the 1 mM solution of p-nitrophenol (PNP) provided, create a series of dilutions. You will make 10, 25, 50, 75, and 100 μM solutions. In making these solutions, use 1x reaction buffer (0.2 M Tris, pH 8.0; 5 mM MgCl2) as the diluent. You will need 1 mL of each of these solutions
A standard solution contains 100 ppm of Fe, which was found to have an absorbance of 0.151 au at 508 nm after the addition of 1,10-phenanthroline, pH 4 buffer, and hydroxylamine. Then, a water sample treated similarly exhibited an absorbance of 0.109 au. Which of the following statements is true? The Fe concentration of the water sample is higher than 100 ppm. It is impossible to estimate the Fe content of the water sample from information presented. The Fe concentration of the water sample is lower than 100 ppm. The Fe concentration of the water sample is equal to 100 ppm.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS