Example:-You wish to prepare a calibration curve for the spectrophotometric determination of permanganate. You have a stock 0.100 M solution of KMnO4 and a series of 100 mL volumetric flasks. What volumes of the stock solution will you have to pipet into the flasks to prepare standards of 1.00, 2.00, 5.00, and 10.0x10-3 M KMnO4 solutions. Solution-1: 10x10 M (M₁ x V₁) conc = (M₂ x V₂)dilu. mm 0.1 x V₁ = 1.0 x 10-3 x 100 (mL) mL mL V₁ = 1.0 mL stock solution (conc.),Also to prepare 2.0, 5.0, 10.0x10³ M

Example:-You wish to prepare a calibration curve for the spectrophotometric determination of permanganate. You have a stock 0.100 M solution of KMnO4 and a series of 100 mL volumetric flasks. What volumes of the stock solution will you have to pipet into the flasks to prepare standards of 1.00, 2.00, 5.00, and 10.0x10-3 M KMnO4 solutions. Solution-1: 10x10 M (M₁ x V₁) conc = (M₂ x V₂)dilu. mm 0.1 x V₁ = 1.0 x 10-3 x 100 (mL) mL mL V₁ = 1.0 mL stock solution (conc.),Also to prepare 2.0, 5.0, 10.0x10³ M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

You are provided with a stock standard with a concentration of 100 mg/L, and a solution of unknown concentration. Prepare calibration standards using a 10 mL volumetric flask and a 1 mL piston pipette, and measure on the UV/Vis spectrophotometer (400 nm). Determine the concentration of the unknown after a 1:40 dilution, and provide the concentration of the initial solution. i need to learn how to do the calculations and draw a calibration curve to find concentration of unknown sample after i find the absorbances.
i have hard time geting it stright even after I do the experiment can u help me with the one pls Material ChemicalsSealed NO2 tubes, KSCN solution (0.002 M), acidified Fe(NO3)3 solution (0.2 M), KSCN crystals, Fe(NO3)3 crystals, KOH (concentrated (8 M)), distilled waterApparatus:Bunsen burner, ring stand, wire gauze, matches, thermometer, dropper, test tubes, glass stirring rod, beaker tongs Procedure Part A: Fill a 600 mL beaker to the 3/4 mark with water. Bring to a boil using a Bunsen burner. In another 600 mL beaker, fill to the 1/2 mark with water; add ice in order to lower the temperature to about 0°C. Note the room temperature. Observe the NO2 thoroughly at room temperature. Place the sealed NO2 tube in the cold bath. Note your observations. Remove the test tube from the cold bath. Let the test tube stand until it reaches room temperature. Note your observations. Place the test tube in the hot bath. Note your observations. Remove the test tube from the hot bath. Let the test…
4- A sample containing H2C204 had a purity equal to 90.50% (w/w). An unknown mass of this sample was dissolved in water and transferred to a 50.00 mL flask. An aliquot of 25.00 mL was transferred to an erlenmeyer flask and 50.00 mL of a 0.2000 mol L^-1 NaOH solution were added. %3 Excess NaOH was titrated with 0.09000 mol L^-1 HCI solution using 2.000 mL. Calculate the mass (g) of the sample used. Data: H = 1.008 C= 12.01 O = 16.00
A clinical chemist obtained the following data for the alcohol content of a sample of blood: % C,H OH: o.084, 0.089, and o.079. Calculate the 95% confi- dence interval for the mean assuming that (a) the three results obtained are the only indication of the precision of the method and that (b), from previous
Need help with dimesional analysis
percentage purity of an ibuprofen sample was determined by a reversed phase HPLC method as follows: Y Der ● A calibration curve of peak area versus concentration (ug/mL) of pure ibuprofen was constructed The ibuprofen sample for analysis was prepared by taking 10.0204 g of powder and dissolving it in/1Lbf distilled water (solution A). 1 ml of the latter solution was further diluted to IL with distilled water (solution B). Solution B was analysed by HPLC analysis Results The equation for the best-fit line of the calibration curve is: y=26820x-1323.8. ● The average peak area for the ibuprofen sample (solution B) was 266796.2 Calculate the percentage purity of the ibuprofen powder.
By the data gathered calculate the amount of BaCl2 needed fortitration.
The concentration of acetylsalicylic acid in an antipyretic tablet was determined by HPLC using a normal calibration curve. Standard solutions of acetylsalicylic acid were prepared and analysed using a 10µL loop. The results obtained for the standards are tabulated below: Conc. of Acetylsalicylic Acid (ppm); Signal (arbitrary units) 50; 6352 100; 12869 150; 19175 200; 25536 250; 31936 To determine the concentration of acetylsalicylic acid in an antipyretic tablet, 10 tablets were weighed (6.500 g total) and crushed to a fine powder using a mortar and pestle. A quantity of powder equal the mass of one tablet was added to a 100 mL volumetric flask. The tablet powder was dissolved with 20 mL of methanol and the flask was made to volume using water. The solution was filtered. A 1.000 ml aliquot was transferred to a 10 ml volumetric flask, which was then made to volume with water. Analysis was conducted using a Bio Sil HL C18, 250mm x 4.6mm column; 5um, with a mobile phase of acetonitrile:…
Payal
A spectrometry method was applied to determine component A in solution. The result is shown in the table. Supposing an unknown sample gives result of 525, 536, 529, please calculate the concentration of A in the sample. \table [[C (u),0.00, 1.00, 2.00, 4.00, 8.00, 16.00], [1, 1.2, 110, 216, 445,869, 1750]] A m J c 1) A spectrometry method was applied to determine component A in solution. The result is shown in the table. Supposing an unknown sample gives result of 525, 536, 529, please calculate the concentration of A in the sample. CA (ug/ml) 0.00 1.00 2.00 4.00 8.00 16.00 I 1.2 110 216 445 869 1750
Following the monograph procedure, a 724-mg of aspirin (MW=180 g/mol) dissolved in 18.5 ml of cold neutralized alcohol. This solution was then initially titrated with 0.101 N sodium hydroxide solution, then later neutralized with 0.104 sulfuric acid. What is the percentage purity of the sample? 1. What is the milliequivalent weight consumed by the acidic titrant? a. 1.5392 g-meq b. 2.0907 g-meq c. 1.4948 g-meq d. 2.1528 g-meq 2. What is the milliequivalent weight consumed by the basic titrant? a. 5.8656 g-meq b. 1.5392 g-meq c. 5.6964 g-meq d. 1.4948 g-meq 3. What is the difference of milliequivalent weight consumed in the reaction? a. -4.1572 g-meq b. 4.3708 g-meq c. 0.5515 g-meq d. 4.1572 g-meq
Pls help ASAP. Pls show all work and calculations.