20 ml portion of a deep well water sample was diluted to 250 ml solution. a 50 ml aliquot of this diluted sample water was buffered at ph 10 and required 8. 50 ml of a standard EDTA.the titrant was standardized using 100ml containing 0.8622 mg primary standard calcium carbonate , which required 15.45 ml for titration.(a) identify a possible indicator and its endpoint color (b) calculate the molarity of the EDTA

20 ml portion of a deep well water sample was diluted to 250 ml solution. a 50 ml aliquot of this diluted sample water was buffered at ph 10 and required 8. 50 ml of a standard EDTA.the titrant was standardized using 100ml containing 0.8622 mg primary standard calcium carbonate , which required 15.45 ml for titration.(a) identify a possible indicator and its endpoint color (b) calculate the molarity of the EDTA

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter13: Titrations In Analytical Chemistry

Section: Chapter Questions

Problem 13.5QAP

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2) A 100.0 mL sample of drinking water was treated with ammonia buffer and after addition of Eriochrome Black T indicator, required 18.0 mL of 0.00559 M EDTA for titration. (a) Identify the role of ammonia buffer in the analysis. (b) Identify the indicator and endpoint color. (c) Calculate the total hardness of the water sample as ppm CaCO
WARIARTAM 2. 1.2589 g of a certain brand of milk powder required 25.89 mL of 0.01873M EDTA to titrate the calcium contained in the sample. (a) What is the percent calcium in the sample? (b) Would the true result be higher, lower, or not be affected if the milk powder sample has been slightly wet?
Five drops of dichlorofluorescein have been added to a solution containing 0.800 g sample which required 25.30 mL of 0.100 M AgNO3. (a) Identify the type of argentometric titration method used.
The phosphate in a 3.000-g sample of industrial detergent was precipitated by the addition of 1.000 g of AgNO3. The solution was filtered and filtrate, upon addition of 1.00 mL of 0.01 M fecl3, required 18.23 mL of 0.1377 M KSCN for titration to the end point. (a) the weight percent of phosphate in the detergent
5. A 300.0 mg sample containing Na,CO3, NaHCO, and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 ml to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.
Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2)3N (K, = 5.2 x 10), with 0.1000 M HCl solution after the following additions of titrant. %3D (a) 10.00 mL: pH =9.72 (b) 20.70 mL: pH =|8.25 (c) 28.00 mL: pH =|10.17 %3D
A carbonate mixture was titrated with 0.1100 M HCI. The sample weighing 850.0 mg took 21.00 mL to reach the phenolphthalein end point and an additional 14.00 mL to reach the methyl red end point. Calculate the weight percentage of the component/s.
A 25.00-mL solution containing NaOH, Na2CO3, and NaHCO3 alone or in compatible combination was titrated with 0.0998 M HCl using phenolphthalein as indicator. The solution turned colourless after addition of 25.65 mL of HCl. Methyl orange was then added to the solution and an additional 6.95 mL of the acid was needed to change the colour of the indicator. Identify the components in the mixture and calculate the concentration of each in milligrams per millilitre of solution.
5. A 300.0 mg sample containing Na,CO3, NaHCO3 and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 mL to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.
A 0.15mL of phenolphthalein indicator was dropped to 10.00mL of an unknown acid. Then, 52.00mL from the 100mL of 10M NaOH Solution was placed in a 50mL burette. A titration experiment was done using the 10.15mL unknown acid with phenolphthalein indicator as analyte and the 52mL of NaOH as titrant. The solution turned pink when the final volume of the analyte was 10.68mL and the final reading in the burette was 51.47mL. What is the concentration of the unknown acid?
Suppose that you want to titrate a sample of vinegar with standard sodium hydroxide solution to determine the concentration of acetic acid in it, and you want to use an indicator to help you determine the end-point. Which of the following indicator would be suitable? (A) Bromocresol Green (Ka ~ 2.0 x 10–5; color: yellow in acid; blue in base) (B) Methyl Red (Ka ~ 5.0 x 10–6; color: red in acid; yellow in base) (C) Bromothymol Blue (Ka ~ 6.0 x 10–8; color: yellow in acid; blue in base) (D) Any of them
(a) Calculate the pH of 1.00 x 10-2 M acetic acid solution. Ka for acetic acid is 1.75 x 10-5. (b) Sketch a titration curve for a 50.0 mL of 0.01M Sr2+ solution, buffered at pH 11 when 0.0,10.0, 24.0, 25.0, 26.0, 30.0, and 40.0 mL of 0.02 M EDTA are added. Given the KSrY2- is 4.3X108 and α4 is 0.85.