Can I please get help on steps 1-3 Directions:(1) Determine the total volume of the standards by using a formula in the appropriate boxes (your instructor will help you with this).(2) Determine the concentration of Cu2+ in each standard, also using a formula in the appropriate cells.(3) Plot the absorbance as a function of Cu2+ concentration. Determine the equation for the best-fit line.1.0 M ethylenediamine(mL)concentration Cu2+ absorbance (AU)at 550 nm0.01 M CuSO4 5H2OH2Ototal volumestock Cu2+standard(mL)(mL)(mL)(units)concentration (M)10.500.009.500.0250.0120.500.509.000.0310.0130.501.008.500.0480.0140.502.007.500.1530.0150.503.006.500.2230.010.504.005.500.3070.0170.505.004.500.3840.01 (4) Using your calibration curve, determine the concentration of Cu2+ in unknown A.(5) Next, calculate the concentration of Cu2+ in the stock solution A used to make unknown A.volume of CUSO4absorbance (AU)1.0 M ethylenediamine(mL)H2Ototal volumeconcentration Cu2+stock A Cu2+unknown5H20 of unknown(mL)(mL)(units)at 550 nmconcentration (M)conc; stock A (mL)A0.502.007.500.25(6) Repeat steps 4-5 for unknowns B and C.volume of CuSO41.0 M ethylenediamine(mL)total volume(mL)concentration Cu2+ absorbance (AU)at 550 nmH2Ostock B Cu2+unknown5H2O of unknown(mL)(units)concentration (M)conc; stock B (mL)В0.503.006.500.451volume of CuSO4concentration Cu2+| absorbance (AU)1.0 M ethylenediamine(mL)H2Ototal volumestock C Cu2+unknown5H2O of unknown(mL)(mL)(units)at xx nmconcentration (M)conc; stock C (mL)0.504.505.000.283

The data is given for absorbance versus concentration of different solutions.

1) Determine the total volume of the standards by using a formula in the appropriate boxes (your instructor will help you with this). 2) Determine the concentration of Cu2+ in each standard, also using a formula in the appropriate cells. 3) Plot the absorbance as a function of Cu2+ concentration. Determine the equation for the best-fit line.

1) Determine the total volume of the standards by using a formula in the appropriate boxes (your instructor will help you with this). 2) Determine the concentration of Cu2+ in each standard, also using a formula in the appropriate cells. 3) Plot the absorbance as a function of Cu2+ concentration. Determine the equation for the best-fit line.

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

Ben ran through the experiment and found the best-fit line listed below for his standard calibration curve of absorbance vs concentration in M. y = 3214.0x + 0.0076 Ben then prepared a solution that had 5.00 mL 0.002 M iron(III) nitrate in 1 M nitric acid, 3.00 mL 0.002 M potassium thiocyanate, and 2.00 mL DI water. If the absorbance for the solution was 0.436, calculate the equilibrium concentration of iron(III) thiocyanate in the solution. Report your answer in mM with three places after the decimal.
The table shows a series of standard additions of Cu(II)to acidified water samples measured by anodic stripping voltammetry at a platinum electrode. The unknown and all standard additions were made up to the same final volume. 1. What chemical reaction occurs during the concentration stage of the analysis?2. What chemical reaction occurs during the stripping stage of the analysis?3. Plot absorbance as a function of the concentration of Cu (II) standard. Determine the equation of theline and the X intercept. Find the concentration of Cu(II) in the water.
What conclusion can be derived from the following sentences regarding analytical methods: I. Classical methods (gravimetry and volumetric methods) are no longer useful in analytical chemistry. II. Volumetric methods do not require calibration if a primary standard is used as titrant. III. Instrumental methods are useful with analyte solutions that are less than 1.00 mM. IV. Classical methods yield high precision and accuracy at concentrations greater than 1.00 mM. What conclusion can be derived from the following sentences regarding analytical methods: Two statements are incorrect. All statements are correct. One statement is incorrect. Only one statement is correct. All statements are incorrect.
Nitrite ion, NO2-, is a preservative for bacon and other foods, but it is potentially carcinogenic. A spectrophotometric determination of NO2- makes use of the following reactions: A 5.00 cm cell was used to measure absorbance. Here is an abbreviated procedure for the determination. 1. To 50.0 mL of unknown solution containing nitrite is added 1.00 mL of sulfanilic acid solution. 2. After 10 min, 2.00 mL of 1-aminonapthalene solution and 1.00 mL of buffer are added. 3. After 15 min, the absorbance is read at 520 nm in a 5.00-cm cell. The following solutions were annaylzed: A. 50.0 mL of food extract known to contain no nitrite(that is a neglible amount); final absorbance =0.153 B. 50.0 mL of food extract suspected of containg nitrite ; final absorbance= 0.622 C. Same as B, but with 10 microliters of 7.50x10^-3 M NaNO2 added to the 50.0 mL sample; final absorbance= 0.967 a) Calculate the molar absorptivity of the colored product. Remember that a 5.00 cm cell was used b) How many…
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.
Sally obtains a standard calibration curve for their assigned food dye by plotting absorbance versus concentration (in M) of known solutions and finds the following slope and intercept: y = 1.646x + 0.026 Sally finds that her original Kool-aid sample is too concentrated, so they dilute it by transferring 13.00 mL of the original Kool-aid sample into a new container and diluting to a total volume of 37.00 mL. If the absorbance of the dilute Kool-aid sample at the appropriate wavelength for their assigned dye is 0.950, determine the concentration (in M) of the assigned food dye in the original Kool-aid sample. Report answer with three places after the decimal.
If an analytical method relies on a measurable property of an analyte that can be correlated with the amount of the said analyte, what type of analytical method is it? Oxidative methods Instrumental methods Blank Correction methods Classical methods
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.
You are given 2 ml of a stock solution of phenol red at a concentration of 258 mg/ml and 20 ml of 0.5 potassium phosphate buffer pH 7. You need 100 ml of a solution containing 50 mM potassium phosphate buffer pH 7 and 87 ug/ml phenol red to do a spectrophotometric analysis. How would you make this new solution?
The table shows a series of standard additions of Cu(II)to acidified tap water samples measured by anodic stripping voltammetry at a platinum electrode. The unknown and all standard additions were made up to the same final volume. 1. Plot absorbance as a function of the concentration of Cu (II) standard. Determine the equation of the line and the X intercept. Find the concentration of Cu(II) in the water.
what is the purpose and what is it for Spectrophotometric of a Cobalt Chloride Solution Analysis?
An unknown sample of Cu2+ gave an absorbance of 0.475 in an atomic absorption analysis. Then 5.00 mL of solution containing 75.0 ppm (= µg/mL) Cu2+ was mixed with 45.0 mL of unknown, and the mixture was diluted to 500.0 mL in a volumetric flask. a) Write an expression for the final concentration after dilution. b) Calculate the final concentration of the added standard. c) The absorbance of the new solution was 0.987. Find the initial concentration of Cu2+ in the unknown sample