1. Add 3 trailing zeros if your answer is a whole number 2. Encode the unit, attach it immediately to the preceding number, no spaces in between 3. For decimal answers, round off to 4 decimal places How much volume (mL) is needed to standardize 0.05M of EDTA using 180mg of magnesium ribbon? MW: 24g/mol* How many grams of EDTA is required to prepare 250mL of a 0.05M solution? MW: 292g/mol* What is the Molarity of the EDTA solution if 35mL of the titrant was added to 0.2g of calcium carbonate? Round off to four decimal places*

1. Add 3 trailing zeros if your answer is a whole number 2. Encode the unit, attach it immediately to the preceding number, no spaces in between 3. For decimal answers, round off to 4 decimal places How much volume (mL) is needed to standardize 0.05M of EDTA using 180mg of magnesium ribbon? MW: 24g/mol* How many grams of EDTA is required to prepare 250mL of a 0.05M solution? MW: 292g/mol* What is the Molarity of the EDTA solution if 35mL of the titrant was added to 0.2g of calcium carbonate? Round off to four decimal places*

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter22: Bulk Electrolysis: Electrogravimetry And Coulometry

Section: Chapter Questions

Problem 22.27QAP

See similar textbooks

Similar questions

A 47.6 mL aliquot from a 0.5 L solution that contains 0.45g of MnSO4 (MW is 151 g/mol) required 41.9 mL of an EDTA solution to reach the titration endpoint. What mass of CaCO3 (MW is 100.09 g/mol) will react with 1.58 mL of the EDTA solution?
Which of the following statements is/are correct for coulometry? I. Coulometric methods count the electrons used in a chemical reaction to measure the analyte. II. Coulometry uses constant current or constant potential conditions. III. An advantage of coulometric methods is low reproducibility and a disadvantage is low sensitivity. IV. Coulometric titrations are constant potential methods. V. Constant potential methods using a three-electrode cell are more selective than constant-current methods.
(Please give clear handwritten answer) 0.1 M HNO3 solution at 298K was electrolyzed in Hittorf cell using platinum electrodes. After electrolysis, 34.2 mg of copper was deposited in coulometer which in series with the Hittorf cell. 50 mL of HNO3 solution was withdrawn from anode compartment after electrolysis and found to have a concentration of 0.0821 M. [Atomic mass Cu = 63]. (i) Find the transference number of H + and NO3 −. (ii) If 50 mL HNO3 solution was run off from cathode compartment, what would its concentration be?
A 0.2653 g of pure potassium dichromate was dissolved in 15 mL of 1.5 M sulfuric acid and transferred to a 250.0 mL volumetric flask and diluted to the mark with distilled water. A 25.0 mL aliquot of this solution was transferred to another 250.0 mL volumetric flask and diluted to the mark with distilled water and this solution has an absorbance 0f 0.387 in a 2.00 cm cell. Calculate the molar absorptivity of potassium dichromate.
Which is not an error associated with an incorrectly defined pH measurement? A) contact potential deviation-AgCl or Ag precipitates due to dilution of KCl or presence of reducing reagentB) alkaline fault - electrode responds to Na+ instead of H+ when [Na+] is low and [H+] is highC) acid error – the measured pH is higher than the actual pH because the glass is saturated with H+ and can no longer be protonatedD) temperature – the pH meter is calibrated at different temperatures from the sample
Which of the following statements is/are correct for coulometry? I. Coulometric methods count the electrons used in a chemical reaction to measure the analyte. II. Coulometry uses constant current or constant potential conditions. III. An advantage of coulometric methods is low reproducibility and a disadvantage is low sensitivity. IV. Coulometric titrations are constant potential methods. V. Constant potential methods using a three-electrode cell are more selective than constant-current methods. A). I, II and V B). I, II, IV and V C). I, III and IV D.) II, IV and V
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.
One method for determining whether an individual has recently fired a gun is to look for traces of antimony in the residue collected from the individual’s hands. Anodic stripping voltammetry at a mercury film electrode is ideally suited for this analysis. In a typical analysis a sample is collected from a suspect with a cotton-tipped swab wetted with 5% v/v HNO3. After returning to thelab, the swab is placed in a vial containing 5.0 mL of 4 M HCl that is 0.02 Min hydrazine sulfate. After allowing the swab to soak overnight, a 4.0-mL portion of the solution is transferred to an electrochemical cell along with 100 mL of 0.01 M HgCl2. After depositing the thin film of mercury and the antimony, the stripping step gives a peak current of 0.38 μA. After adding a standard addition of 100 μL of 5.00×102 ppb Sb, the peak current increases to 1.14 μA. How many nanograms of Sb were collected from the suspect’s
A 15.00 g sample containing mixed alkali and other inert components was dissolved and diluted to 300 mL with water. A 20 mL aliquot was titrated with 5.02 mL of 0.5352 M HCl to reach PHP endpoint. Another 20 mL aliquot was titrated to the BCG endpoint, using up 18.87 mL of titrant in the process. Note: Answer in two decimal places only. If there is no answer, type in 0.00. Use the molar masses 105.989 ?/??l ??2cO3 and 84.007 g/mol NaHCO3 indicated. The volume of titrant needed to neutralize NaOH is _________ mL.The volume of titrant needed to neutralize Na2CO3 is _____________ mL.The volume of titrant needed to neutralize NaHCO3 is _____________ mL. The mass of NaOH is ___________ g.The mass of Na2CO3 is __________ g.The mass of NaHCO3 is __________ g. The percent weight of NaOH is __________ %.The percent weight of Na2CO3 is __________ %.The percent weight of NaHCO3 is __________ %.
If you have a sample of 100 mg/L of calcium, and you have two standardized EDTA solutions of 0.005 M and 0.001 M, which one is more adequate to spend approximately 15.00 mL of the titrant if 25.00 mL of sample are added in the Erlenmeyer flask? How many mL of titrant will be used? Solution: The 0.005 M solution. 12.5 mL will be used.
One method for determining whether an individual recently fired a gun is to look for traces of antimony in residue collected from the individual’s hands. Anodic stripping voltammetry at a mercury film electrode is ideally suited for this analysis. In a typical analysis a sample is collected from a suspect using a cotton-tipped swab wetted with 5% v/v HNO3. After returning to the lab, the swab is placed in a vial that contains 5.0 mL of 4 M HCl that is 0.02 M in hydrazine sulfate. After soaking the swab, a 4.0-mL portion of the solution is transferred to an electrochemical cell along with 100 μL of 0.01 M HgCl2. After depositing the thin film of mercury and the antimony, the stripping step gives a peak current of 0.38 μA. After adding a standard addition of 100 μL of 00×102 ppb Sb, the peak current increases to 1.14 μA. How many nanograms of Sb were collected from the suspect’s hand?
Indicate the option that is true:(1). An indicator electrode has an upper limit of measurement; That is, it does not serve as a precise analytical instrument when the concentrations of the analyte are very high.(2). Some electrodes take a long time to respond, but that is usually not an insurmountable drawback.(3). The representation of the potential of an indicator electrode against the analyte concentration is a straight line for analyte concentrations below a certain value.(4). For activities lower than the lower detection limit, the electrode always measures the same potential.