Calculate the milligrams of zinc and nickel present per milliliter in your original sample by taking the average of the two trials. To do this, determine the amount in moles that was in the 10-mL of diluted sample placed onto the column. Take this concentration and correct for the first sample prep dilution where you took the original unknown and diluted to 100 mL. Molarity of EDTA = 0.003298 M Ni: Trial 1= 20.80 mL Trial 2= 20.81 mL EDTA used in titration Zn: Trial 1= 31.18 mL Trial 2 - 21 80 ml E DTA UC ed in titration

Calculate the milligrams of zinc and nickel present per milliliter in your original sample by taking the average of the two trials. To do this, determine the amount in moles that was in the 10-mL of diluted sample placed onto the column. Take this concentration and correct for the first sample prep dilution where you took the original unknown and diluted to 100 mL. Molarity of EDTA = 0.003298 M Ni: Trial 1= 20.80 mL Trial 2= 20.81 mL EDTA used in titration Zn: Trial 1= 31.18 mL Trial 2 - 21 80 ml E DTA UC ed in titration

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

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

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

ChapterA1: Evaluation Of Analytical Data

Section: Chapter Questions

Problem A1.23QAP

See similar textbooks

Similar questions

A water sample was analyzed for Fe content using the iron- phenanthroline method. The following data were obtained from the analysis: Reagent Blank Absorbance Absorbance (au) Reagent Blank Absorbance 0.003 Concentration of Stock Solution: 10 ppm Volume of Stock Solution (mL) Total Volume of Standard Solution Concentration of Standard Solution (ppm) Absorbance (au) (mL) 0.50 10.00 0.012 1.00 10.00 0.132 2.00 10.00 0.267 3.00 10.00 0.349 4.00 10.00 0.428 5.00 10.00 0.560 Volume of Unknown Solution Total Volume of Unknown Solution Trial Absorbance (au) (mL) (mL) 1 5.00 10.00 0.289 2 5.00 10.00 0.296 3 5.00 10.00 0.281 Determine the value of the slope (m), y-intercept (b), and the coefficient of determination (r²) A m = 0.1128; b = -4.0 x 10-5; r2 = 0.9880 B m = 0.1128; b = -4.0 x 10-5; r² = 0.9762 C) m = 0.1128; b = -3.0 x 10-³; r² = 0.9880 D m = 0.1128; b = -3.0 x 10-³; r² = 0.9762
Preparation and Standardization of KMnO4 solution Experimental data Complete the table below. Trial 1 0.2001 g Trial 2 0.2065 g Trial 3 Weight of sodium oxalate (Na2C2O4, MM= 134 g/mol) Titration data 0.2050 g Final reading Initial reading 29.86 mL 0.00 mL 30.66 mL 30.52 mL 0.00 mL 0.00 mL Total vol. of KMNO4 used Computed Molarity of KMNO4 solution Mean Molarity Computed Normality of KMNO4 Mean Normality of KMNO4 solution Reaction Involved: Calculations:
1. Data & Results 4.0 mglmL Concentration of stock solution (include units): Table 1-Beer's Law Plot Data V Volume of standard solution dispensed (mL) M, Diluted concentration (include units) Sample Absorbance A 2.00 mL 0.084 4.00 mL 0.173 l6.00 mL 0.259 8.00 mL 0.340 E 10.00 mL 0.418 Equation of trendline from Beer's Law plot: whats the diluted concentration and equation of trendline from the beers law plot once created?
Standardization of EDTA was done using MgSO4 standard wherein a 50-mL aliquot of solution obtained from 0.480 g MgSO4 in 500 mL needed 39.4 mL of the EDTA solution to reach the endpoint. Determine how many milligrams of CaCO3 will react per mL of this EDTA solution.
An sample of eggshell that weighs 1.0014g and is 51μm thick is titrated with disodium EDTA. A solution of the 1.0014g sample and 30 mL of HCl is vacuum filtered after being mixed. The product of the filtration is added to a 250mL volumetric flask and is diluted by being filled to the 250 mL mark with deionized water. 10 mL of this diluted mixture is mixed with EBT indicator and titrated with 0.05 M disodium EDTA. It takes 12.3 mL of disodium EDTA to notice a change in color. What percent mass of calcium is in the eggshell?
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 end point. Report the purity of Na2CO3 sample.
A 0.9092 g sample of wheat flour was analyzed by the Kjeldahl procedure. The ammonia formed was distilled into 50.00 mL of 0.02532 M H2SO4. A 7.46 mL back-titration of 0.04917 M NaOH was required. (Note the stoichiometry of your acid and base) Calculate the a. %N (FM=14.007) in the sample, b. %Protein in the sample (factor = 5.70)
Mass of Sample Volume of KMnO, solution used in titration Equivalents of permanganate used Equivalents of iron (II) in sample Moles of iron (II) in sample Grams of Iron in Sample % Iron in Sample Average % Iron in Unknown Instructor's Grade for Precision in Part B. Sample Calculations Part B: 0.58179 0.68719 28.19 ml 31,96m6 007662 00266 2 11 n
The Zn in a 0.6185 g sample of foot powder was titrated with 23.74 mL of 0.01485 M EDTA. Calculate the % Zn in this sample. Answer: %Zn = ____ %
Nitrite (NO2) can be determined by oxidation with excess Ce4*, followed by back titration of the unreacted Ce4*. A 4.030-g sample of solid containing only NANO2 (FM 68.995) and NANO3 was dissolved in 500.0 mL. A 25.00-mL sample of this solution was treated with 50.00 ml of 0.118 6 M Ce4*in strong acid for 5 min, and the excess Ce4* was back-titrated with 31.13 ml of 0.04289 M ferrous ammonium sulfate. Calculate the weight percent of NANO2 in the solid. 2Ce** + NO, + H2O → 2Ce³* + NO, + 2H* Ce*+ + Fe2+ → Ce³+ + Fe3+ Show your solutions by sending your answers.
You are to make 300mL of 20mM EDTA buffer (C10H16N2O8) solution from powder. How much EDTA powder must be dissolved in water? [Atomic Weight: C = 12.011; H = 1.0079; O = 15.999; N = 14.0067]
One of the CHEM3341 student Ms. Fatima Al Wahaibi wanted to analyse phosphate ion concentration in Fertilizer industry wastewater sample collected from Rusayl Industrial Estate using spectrophotometer method. She mixed 200.00 mL of wastewater sample which contains only Na;PO, (unknown molarity) with 400.00 mL of 0.0200 M K,PO4 in a one liter beaker to make a Solution A. She then transferred 25.00 mL of Solution A to a 250.00 mL volumetric flask and added distilled water up to the calibration mark to make up Solution B. The Concentration of phosphate ions in Solution B is known to contain 3.00 x 103 mol/L from the spectrophotometric analysis at 460 nm using 1 cm cuvette. Calculate the concentration of phosphate ion in wastewater and how many phosphate ions are present in this wastewater.