To determine the concentration of an EDTA solution, the following zinc(II) solution is prepared: metallic zinc (m(Zn) = 0.505 g) is dissolved in dilute sulfuric acid, the resulting solution is poured into a volumetric flask with a volume of 0.200 L and is filled to the graduation mark with water. The titration of an aliquot of zinc(II) solution with a volume of 25.00 ml consumes (10.42 ml; 10.39 ml; 10.48 ml; 10.44 ml; 10.49 ml) of EDTA. Calculate the concentration of EDTA solution with accuracy corresponding to the starting data, give confidence interval.

To determine the concentration of an EDTA solution, the following zinc(II) solution is prepared: metallic zinc (m(Zn) = 0.505 g) is dissolved in dilute sulfuric acid, the resulting solution is poured into a volumetric flask with a volume of 0.200 L and is filled to the graduation mark with water. The titration of an aliquot of zinc(II) solution with a volume of 25.00 ml consumes (10.42 ml; 10.39 ml; 10.48 ml; 10.44 ml; 10.49 ml) of EDTA. Calculate the concentration of EDTA solution with accuracy corresponding to the starting data, give confidence interval.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 37QAP: An artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is...

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An artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is titrated with a basic solution that has a density of 1.045 g/cm3 and contains 5.00 mass percent KOH. What volume of the basic solution is required? (One mole of tartaric acid reacts with two moles of hydroxide ion.)
A student measured 20 drops of vinegar and one drop of phenolphthalein solution into a well of her well plate. After she had added 35 drops of NaOH solution to the same well, the well was full, but she had still not reached the titration endpoint. She then took a clean pipet and transferred some of the titration mixture into a second well. She rinsed the pipet with a few drops of distilled water and transferred the rinse water into the titration mixture in the second well. Then she continued adding NaOH solution to both wells until she reached the endpoint in both wells. She then recorded the total number of drops of NaOH solution added to both wells and used it to calculate the data for her vinegar titration. Briefly comment on her procedure and the accuracy of her results.
A 11.00 gram sample of Vodka was analysed for its alcohol content. The sample was placed in a300 mL volumetric flask and made to the mark with distilled water. A 20.0 mL aliquot of the dilutedVodka was taken from the volumetric flask and placed in a conical flask containing some distilled water from a previous washing.The 20.0 mL aliquots were titrated against a 0.1302 M Cr2O72-solution and an average titre of13.25 mL was obtained.The reaction between the alcohol and the dichromate solution is given below2Cr2O72–(aq) + 3CH3CH2OH(aq) + 16H+(aq)  4Cr3+(aq) + 3CH3COOH(aq) + 11H2O(l)a) Calculate the amount in mol of Cr2O72– in the average titre. b) Calculate the percentage, by mass, of ethanol in the vodka.
A sample of CaCO3 (molar mass=100.1) weighing 0.4856 g is dissolved in HCl and the solution diluted to 500.0 mL in a volumetric flask. A 25.00-mL aliquot requires 21.37 mL of an EDTA solution for titration. How many grams of Na2H2Y.2H2O (molar mass=372.2) are required to prepare 500.0 mL of this solution.
A quantitative analysis for ethanol, C2H6O, can be accomplished by a redox back titration.Ethanol is oxidized to acetic acid, C2H4O2, using excess dichromate, Cr2O72–, which is reduced toCr3+. The excess dichromate is titrated with Fe2+, giving Cr3+ and Fe3+ as products. In a typicalanalysis, a 5.00-mL sample of a brandy is diluted to 500 mL in a volumetric flask. A 10.00-mLsample is taken and the ethanol is removed by distillation and collected in 50.00 mL of anacidified solution of 0.0200 M K2Cr2O7. A back titration of the unreacted Cr2O72–requires 21.48mL of 0.1014 M Fe2+. Calculate the %w/v ethanol in the brandy
Write the balanced NET ionic equation for the reaction when aqueous KBr and aqueous AgC₂H₃O₂ are mixed in solution to form aqueous KC₂H₃O₂ and solid AgBr
A student was asked to determine the concentration of ammonia, a volatile substance, in a commercially available cloudy ammonia solution used for cleaning. First the student pipetted 25.00 mL of the cloudy ammonia solution into a 250.0 mL conical flask. 50.00 mL of 0.100 mol L-¹ HCl(aq) was immed added to the conical flask which reactedwith the ammonia in solution. The excess (unreacted) HC1 was then titrated with 21.50 mL 0. 050 M Na2CO3 (aq). Calculate the concentration of the ammonia in the cloudy ammonia solution.
A sample of solid Ca(OH)2 was stirred in water at a certain temperature until the solution contained as much dissolved Ca(OH)2 as it could hold. A 84.3-mL sample of this solution was withdrawn and titrated with 0.0948 M HBr. It required 64.6 mL of the acid solution for neutralization.(a) What was the molarity of the Ca(OH)2 solution? M(b) What is the solubility of Ca(OH)2 in water, at the experimental temperature, in grams of Ca(OH)2 per 100 mL of solution? g/100mL
the calcium in a 5.00ml serum sample is precipitated as CaC2O4 with ammonium oxalate. the filtered precipitate is dissolved in acid, the solution is heated, and the oxalate is titrated with 4.00 x 10^-5 M KMnO4, requiring 4.94mL. calculate the concentration of cqlcium in the serum in mg/L Molar mass Ca= 40.08 g/mol balanced chemical equation:
The tartaric acid, H2C4H4O6 (150.087 g/mol ) in 100.0 mL wine sample was determined using sodium hydroxide standard solution. In the experiment, 35.21 mL of the base was initially standardized against 3.001 grams primary standard of KHP (204.22 g/mol). What is the standard concentration of the prepared NaOH solution?
A Medical Technology student was given a capsule of a multivitamins and she was asked to determine the % by mass (w/w) of ascorbic acid present in the capsule. The student analyzed the 2.001 g sample using volumetric titration. The following data was generated in the analysis: KIO3 + 5KI + 6H+ → 3I2 + 6K+ + 3H2O C6H8O6 + I2 → C6H6O6 + 2I- + 2H+ Table 1. Standardization of KIO3 Molarity of Ascorbic Acid Standard Solution 0.03542 M Volume of Ascorbic Acid 25.00 mL Volume of KIO3 8.70 mL Molarity of KIO3 ______________M Table 2. Determination of Ascorbic Acid Concnetration Initial burette reading, KIO3 0.00 mL Final burette reading, KIO3 33.60 mL Volume consumed, KIO3 33.60 mL MM of Ascorbic Acid 176.12 g/mole choices 7.30% 30.1% 33.6% 32.5%
To determine the concentration of an EDTA solution, the following magnesium(II) solution is prepared: metallic magnesium (m(Mg) = 0.5915 g) is dissolved in dilute sulfuric acid, the resulting solution is poured into a volumetric flask with a volume of 0.250 L and is filled to the graduation mark with water. The titration of an aliquot of magnesium(II) solution with a volume of 25.00 ml consumes (11.11 ml; 11.32 ml; 11.24 ml; 11.29 ml) of EDTA. Calculate the concentration of EDTA solution with accuracy corresponding to the starting data, give confidence interval.