4 In the determination of sulphate ion concentration in natural water a turbidimeter was calibrated with a series of standard NazSO4 solutions. The following data were obtained in the calibration: Cx,mg SO4/L Turbidimeter reading, R 0.00 0.06 5.00 1.48 10.00 2.28 15.00 3.98 20.00 4.61 Assume that a linear relationship exists between the instrument reading and the concentration. a) Using a graph paper or Excel plot this data accurately b) Calculate the least-squares slope and intercept and write the equation of the line.

4 In the determination of sulphate ion concentration in natural water a turbidimeter was calibrated with a series of standard NazSO4 solutions. The following data were obtained in the calibration: Cx,mg SO4/L Turbidimeter reading, R 0.00 0.06 5.00 1.48 10.00 2.28 15.00 3.98 20.00 4.61 Assume that a linear relationship exists between the instrument reading and the concentration. a) Using a graph paper or Excel plot this data accurately b) Calculate the least-squares slope and intercept and write the equation of the line.

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

If the standard addition intercept is the major source of uncertainty, find the uncertainty in the concentration of Sr in tooth enamel in parts per million. Find the 95% confidence interval for Sr in tooth enamel.
Penicillin F is recovered from a dilute aqueous fermentation broth by extraction with amyl acetate, using 6.5 volumes of solvent per 100. volumes of the aqueous phase. At pH = 3.8 the distribution coefficient KD is 74. (a) What fraction of the penicillin would be recovered in a single ideal stage? (b) What would be the recovery with three-stage extraction using fresh solvent in both stages? (c) How many ideal stages would be needed to give the same recovery as in part (b) if a counterflow cascade were used with V/L = 0.065?
grammarly-G X * Content oard.odu.edu/ultra/courses/_393452_1/cl/outline F2 Question Completion Status: X GA student wan X 1 QUESTION 3 A student wants to determine the solubility of water and copper (1) bromide (a green solid) in ethyl acetate (a colorless organic liquid). She places 1 mL of ethyl acetate into each of two test tubes. To one, she adds 5 drops of water to it. To the other, she adds a small scoop of copper(1) bromide. 8.0 F3 2 - Which test tube represents the ethyl acetate and A. Test tube 1 copper(1) bromide if the copper(1) bromide is insoluble in ethyl B. Test tube 2 acetate? C. Test tube 3 D. Test tube 4 - Which test tube represents the mixture of the ethyl acetate and water if the water is insoluble in ethyl acetate? $ Question Com X C Chegg Search x 3 Which test tube represents the mixture of the ethyl acetate and water if the water is soluble in ethyl acetate? - Which test tube represents the ethyl acetate and copper(1) bromide if the copper(1) bromide is soluble…
Calculate the percentage purity of naproxen (FW 230.26) from the following data. 212.9 mg of naproxen was weighed and dissolved in a mixture of 25 ml of water and 75 ml methanol. It was titrated with 0.1024 M sodium hydroxide solution, using 1 ml of phenolphthalein solution as indicator. 8.08 mL of sodium hydroxide was required to neutralize the solution. Record your answer in decimal notation to 2 decimal places.
Blue Blue dye stock solution 0.293 M Absorbance at 630 nm 0.00265 Calibration curve y = 0.0833x A solution is prepared by diluting 2.81 mL of the blue dye stock solution to 25.00 mL. The measure absorbance for the prepared solution is listed in the data table. (a) What is the theoretical molar concentration? [Blue]theoretical | × 10 |M (b) What is the experimental molar concentration? [Bluelexperimental x 10 M (c) What is the percent error? Percent error (blue) =
Eºcell = 0.050 V. If the concentration of Y2+ = 0.025 M, what molar concentration of X3+ would be needed to have E = 0? Fill in the intermediate values requested below and the final answer. Use T = 298 K, R = 8.314 J/molk, and F = 96485 C/mol
Calculate the solubility at 25 °C of PbCO3 in pure water and in a 0.0100M Pb(NO3), solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. 0 // solubility in pure water: x10 solubility in 0.0100 M Pb(NO3)2 0-/- solution: L X 09 00 X S ?
Calculate the solubility at 25 °C of CaF2 in pure water and in a 0.0030M NaF solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. solubility in pure water: solubility in 0.0030 M NaF solution: 0.016 0²/ L 00 x10 X n' OXO 3 00 olo A
As part of an analytical chemistry laboratory course, a student measured the Ca2+ content in two water samples, city-supplied drinking water and well-supplied drinking water, using two different analytical methods, flame atomic absorption spectrometry (FAAS) and EDTA complexometric titration. The results of this experiment are given in the table as the mean Ca2+concentration (?¯) and standard deviation (?) in parts per million (ppm). Each sample was measured five times (n=5) by each method. Method City-Supplied Drinking Water (?¯±?x¯±s) Well-Supplied Drinking Water (?¯±?x¯±s) FAAS 57.57±0.68 ppm 64.77±0.70 ppm EDTA titration 58.32±0.96 ppm 65.62±0.97 ppm Method Comparison: For each drinking water sample (city and well), compare the Ca2+ content measured by FAAS and EDTA titration. Calculate the ? value for each sample. Do the methods produce statistically different results at the 95% confidence level when measuring the Ca2+content of the city-supplied drinking water? Do the…
The solubility of CaCO3 is pH dependent. (a) Calculate themolar solubility of CaCO3 (Ksp = 4.5 x 10-9) neglectingthe acid–base character of the carbonate ion. (b) Use the Kbexpression for the CO32 - ion to determine the equilibriumconstant for the reactionCaCO3(s) + H2O(l) ⇌ Ca2 + (aq) + HCO3-1 (aq) + OH-1 (a q)(c) If we assume that the only sources of Ca2 + , HCO3-,and OH- ions are from the dissolution of CaCO3, what is the molar solubility of CaCO3 using the equilibrium expressionfrom part (b)? (d) What is the molar solubility ofCaCO3 at the pH of the ocean (8.3)? (e) If the pH is bufferedat 7.5, what is the molar solubility of CaCO3?
Francis A. Santos A chemist obtained the following data for the percent compound Z in triplicates (n=3) of an insecticide preparation: 7.47, 6.98, and 7.27. Calculate the 90% confidence limit for the mean of the data assuming that only information about the precision of the method is the precision for the three data points. A 7.24 + 0.74% B) 7.24 + 0.27% 7.24 + 0.13% 7.24 + 0.42%