A 5.00 mL tap water sample was measured out with a volumetric pipette, and added to a 25 mL Erlenmeyer flask. It was then titrated with a 0.0100 M Na2EDTA.2H2O solution, and found to take 0.635 mL of the EDTA solution to reach the blue endpoint. a.) How many moles of the 0.0100 M Na2EDTA.2H2O were added in the titration reaction? Show calculation. b.) How many moles of calcium ions were reacted?

A 5.00 mL tap water sample was measured out with a volumetric pipette, and added to a 25 mL Erlenmeyer flask. It was then titrated with a 0.0100 M Na2EDTA.2H2O solution, and found to take 0.635 mL of the EDTA solution to reach the blue endpoint. a.) How many moles of the 0.0100 M Na2EDTA.2H2O were added in the titration reaction? Show calculation. b.) How many moles of calcium ions were reacted?

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.19QAP

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A 5.00 mL tap water sample was measured out with a volumetric pipette, and added to a 25 mL Erlenmeyer flask. It was then titrated with a 0.0100 M Na2EDTA.2H2O solution, and found to take 0.635 mL of the EDTA solution to reach the blue endpoint.
A 0.1093-g sample of impure Na2CO3 was analyzed by the Volhard method. After adding 50.00 mL of 0.06911 M AgNO3, the sample was back-titrated with 0.05781 M KSCN, requiring 27.36 mL to reach the endpoint. Report the purity of the Na2CO3 sample. [Ans. 90.9 % (w /w )]
A 5.00 mL tap water sample was measured out with a volumetric pipette, and added to a 25 mL Erlenmeyer flask. It was then titrated with a 0.0100 M Na2EDTA.2H2O solution, and found to take 0.635 mL of the EDTA solution to reach the blue endpoint. How many moles of the 0.0100 M Na2EDTA.2H2O were added in the titration reaction? Show calculation. How many moles of calcium ions were reacted? Show calculation.
A 49.10 mL aliquot from a 0.500 L solution that contains 0.530 g of MnSO4 (MW=151.00 g/mol) required 41.6 mL of an EDTA solution to reach the end point in a titration. What mass, in milligrams, of CaCO3 ( MW=100.09 g/mol) will react with 1.53 mL of the EDTA solution?
You took 25.00 mL of unknown water solution and titrated it with EDTA. The EDTA solution molarity was 0.01 M, and it took 16.50 mL to reach the end point. With the blank it took only 0.98 mL to reach end point. 15.52 mL of EDTA solution were used to titrate hardness that actually came from the unknown 1.552×10−4 moles of EDTA reacted with hardness-causing ions from the unknown sample 1.552×10−4 moles of hardness-causing ions were present in the unknown sample A) Assuming that the total hardness of water is due to CaCO3, how many grams CaCO3 does it correspond to? B) What is the total hardness of the unknown water in ppm CaCO3?
1.) A 0.1278-g sample of primary standard Na2C2O4 required exactly 60.04 mL of permanganate solution to reach the end point. What is the molarity of the KMnO4 reagent? 2.) A 50.00 mL sample containing La3+ was added with sodium oxalate to precipitate La2(C2O4)3, which was washed, dissolved in dilute H2SO4, and titrated with 18.09 mL of the standard KMnO4 solution (in #1). Calculate the molarity of La3+ in the unknown sample.
A 30-mL portion of a solution containing Ca2+ and Mg2+ was titrated with 28.19 mL of 0.213 M EDTA at pH 10. Another 30-mL aliquot of the same Ca-Mg mixture was treated with NaOH to make the solution strongly alkaline and precipitate Mg(OH)2. This solution was then titrated with the same EDTA solution. What would be the required EDTA volume (in mL) to reach the endpoint of the second aliquot if it was found that there was 0.061 M of Mg2+ 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 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.