(1)(15 points) An AA was used to analyze the arsenic in samples of well water. ThreeAs standards 1 ppm, 5 ppm, and 10 ppm were prepared. Using the data below,determine the amount of arsenic in the well water. Samples on 3 different days wereobtained. Report the mean and 95% CLSample0 ppm standardA-0.00341.00 ppm standard0.02335.00 ppm standard0.109910.00 ppm standard0.2401sample 10.0322sample 20.0201sample 30.1829

To determine the amount of arsenic in well water samples using atomic absorption (AA) spectrometry…

Answered: (1)(15 points) An AA was used to…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter7: Statistical Data Treatment And Evaluation

Section: Chapter Questions

Problem 7.16QAP

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(A) if both sentences are true,(B) if both sentences are false,(C) if the first sentence is true but the second is false, and(D) if the first sentence is false but the second is true. 1. In the Winkler Titration Method, sodium thiosulfate is standardized against a known concentration of magnesium iodate. The normality (N) of a solution is always equal to its molarity (M). 2. In the experiment on determining the dissolved oxygen concentration of a water sample, the compound used to acidify the sample was hydrochloric acid. An acidic solution will have a pH greater than 7. 3. Radioactive wastes, like uranium, must be handled and disposed of according to special regulations designed to protect people and the environment. Nuclear power plants produce too much greenhouse gases due to the burning of uranium.
A STOCK SOLUTION containing 0.1581 g/L K2CrO4 was prepared.In order to make the CALIBRATION STANDARD, 5 ml of the STOCK was transferredinto a 50ml volumetric flask and then diluted with an appropriate solvent.Calculate:(a) The ppm of K2CrO4 in the CALIBRATION STANDARD.(b) The molarity of K2CrO4 in the CALIBRATION STANDARD. (c) Calculate the molar absorptivity of K2CrO4 (at 371.0 nm). Assume that Beer's Law isobeyed over this concentration range.At 371.0 nm, this CALIBRATION STANDARD in a cell of path length 1.00 cm gave a %T of 59.752.
A solution of HCl was titrated against sodium carbonate. What is the average normality of acid in the given data? (MW Na₂CO3 = 106) T2 0.3479 0.3562 0.3042 Weight (g) Initial V (ml) 0.80 1.60 35.20 36.70 39.80 Final V (mL) Vol HCl used (mL) 35.10 39.40 N of HCl (eq/L) 0.1954 0.1870 Average N of HCl (eq/L)
0.01 mol of solid NaOH was added to a 500 mL solution containing 0.55 M C6H5CH2COOH and 0.75 MC6H5CH2COON (Ka for C6H,CH2COOH = 4.9 x 10-5). Drag and drop the appropriate choices from below to fill the following table and answer the questions. Reaction Table (aq) + OH (ag) + H20 (1) (aq) Initial Changes Final What is the pH of this solution? pH = 8.65 0.02 0.5 0.53 10.32 0.51 0.03 0.73 0.01 0.2 0.75 -0.03 No -0.01 4.47 0.3 +0.01 0.57 +0.03 -0.02 9.85 +0.02 Yes 0.55 C6H5CH2COOH 0.4 0.45 0.1 C6H5CH2CO0- 3.65 3.22 0.77
A chemist receive different mixtures for analysis with the statement that it contain NaOH, NaHCO3 , Na2CO3 or compatible mixtures of these substances together with the inert material. From the data given, identify the respective materials and calculate the percentage of each component. 1.000g samples and 0.2500 N HCl were used in all cases. Sample 1 With phenolphthalein as the indicator, 24.32 ml of HCl was used. A duplicate sample required 48.64 ml HCl using methyl orange as the indicator. Sample 2. With phenolphthalein as the indicator it uses 28.2 ml of HCl to make it colorless and added with methyl orange indicator and uses 11.3 ml of HCl to reach the end point.
Calculate the gravimetric factor of the following. 2 Fe3O4 is sought(Analyte), 3 Fe2O3 is weighed (Precipitate)
In the standardization of HCl using pure anhydrous sodium carbonate as the primarystandard for methyl orange as an indicator, 1.0 mL HCl was found to be equivalent to 0.05gof sodium carbonate (MW =106). The normality of HCl is:
The following data give the constant dissociation, K (for acetic acid at various temperatures) T("C) 0 10 15 25 K₂ 1.657 x 10 1.729 x 10 1.745 x 10-5 1.753 x 10 Part A Using the information that InK versus 1/T is a straight line with slope-AH/R. calculate AH for the lonization of acetic acid Express your answer with the appropriate units. AH 2.732 HA kJ mol Submit Previous Answers Request Answer Part B Complete previous panis) ? X Incorrect; Try Again; 4 attempts remaining Review | Constants I Periodic Table
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…
A 0.1475-M solution of Ba(OH)2 was used to titrate the acetic acid (60.05 g/mol) in a dilute aqueous solution. The following results were obtained. (See attached image)(a) Calculate the mean w/v percentage of acetic acid in the sample.(b) Calculate the standard deviation for the results.(c) Calculate the 90% confidence interval for the mean.(d) (d) At the 90% confidence level, could any of the results be discarded?
Ans. 17.15 mg. 54) A 1.000-g sample of a mixture which contains only NaCl and KCl gare a precipitate of AgCl which weighed 2.000 g. What are the percentages of Na and K in the mixture? ins 10 g Ans. 44.77% K; 5.75% Na. 1:J 55. I- can be sernarated from othor
Standardization of a sodium hydroxide (NaOH) solution against potassium hydrogen phthalate (KHP) yielded the following results: Mass of KHP, g Volume of NaOH, mL 0.7987 38.29 0.8365 38.96 0.8104 38.51 0.8039 38.29 MM KHP: 204.22 MM NaOH: 40.00 a. Calculate the mean molar concentration of sodium hydroxide. (First, compute the concentration of NAOH in each titration then compute for its mean/average value.) b. Calculate the standard deviation. Please provide solutions for your answers. If you have used your calculator for calculating for mean and standard deviation, you can just provide the formula with the values indicated.

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