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In this double titration experiment determining composition of soda ash, you are given the following data:
- M HCl titrant: 0.0501 M +/- 0.0507
- Mass of soda ash sample, g: 0.2505 ± 2.0e-4 (Analytical Balance)
- Total volume of Sample Stock, mL: 75 ± 0.05 (100mL graduated cylinder)
- Volume of Sample Stock Aliquot, mL: 25 ± 0.3
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- A 50.00 (±0.03) mL portion of an HCl solution required 29.71(±0.03) mL of 0.01963(±0.0030) M Ba(OH)2 to reach an end point with bromocresol green indicator. The molar concentration of the HCl is calculated using the equation below (attached image): a.) Calculate the uncertainty of the result (absolute error). M=0.02333(±?????) M b.) Calculate the coefficient of variation for the result. CV= (Sy/y) x 100%SCE students measured the concentration of HCl in a solution by titrating with different indicators to find the end point.Indicator Mean HCl concentration (M)(± standard deviation)Number of measurementsBromothymol blue 0.09565 ± 0.00225 28Methyl red 0.08686 ± 0.00098 18Bromocresol green 0.08641 ± 0.00113 29Is the difference between indicators 1 and 2 significant at the 95% confidence level? Answer the same question for indicators 2 and 3Study the tabulated data during an gravimetric analysis of BaSO4 experiment Trial T1 T2 T3 Mass of sample (g) 1.0040 1.0100 1.0050 Constant weight of empty crucible (g) 10.2453 10.2454 10.2454 Constant weight after ignition (g) 10.3253 10.3252 10.3253 1. Calculate the mean mass of precipitate as BaSO4 a. 0.0799 g b. 0.0800 c. 0.08 g 2. Calculate the mean weight of sulphate (MM BaSO4 = 233.39 g/mol, So42- = 176 g/mol)? a. 0.0603 g b. 0.06 g c. 0.06025 g 3. Calculate the mean % SO42- in the sample a. 6.00% b. 5.991% c. 5.9908%
- (a) During the analysis of water sample by argentometric titration, results obtained are as follows: Experiment1 2 3 4 Volume 15.5, 15.2 ,15.1 ,15.4 A)Calculate average deviation and relative average deviation for the given data. (b)Calculate the molecular weight of an unknown acid if 8.5 g of it is dissolved in 200.0 ml of water and requires 50.0 ml of 1.5 M sodium hydroxide for complete neutralization .You have Falcon tubes containing 10 ml and you should add ,that you have in a voltage series, from which concentration in the dilution series you should pipette 0.1 ml to reach the final concentration of 10-5M in the organ bath Group of response options 10-5M 10-4M 10-3M 10-2MIf pH (± 0.5 pH units) strips were used to determine the equivalence point at pH=8.5. What is the relative error (%) in pH at the equivalence point? I assumed it should be 0.5/8.5 * 100 = 5.88, rounded to 5.9 for sig figs. but I got the answer wrong. Please help and let me know how to solve this.
- If an instrument gives a response of 1240 for a standard containing 8 ppm of a substance, how much if this substance is in a sample that gives a response of 1705? Are any assumptions needed?Standardization of Sodium Thiosulfate Solution Primary Standard used: Potassium Dichromate Formula mass of 1o standard: __________________ % Purity of 1o standard: 99.80% Trials 1 2 3 Weight of K2Cr2O7 (g)Weight of K2Cr2O7 (g) 0.0315 0.0331 0.0380 Final Volume Reading Na2S2O3 (ml) 27.50 27.50 34.90 Initial Volume Reading Na2S2O3 (ml) 1.10 0.00 1.00 Net Volume Na2S2O3 used (ml) Molarity of Na2S2O3A mixture of pure BaCO3 and pure Na2CO3 weighs 1.000 g and has the total neutralizing power of 15.37 meq of CaCO3. Calculate the percentage of combined CO2 in the mixture and the weight of Li2CO3 that has the same neutralizing power as 1.000 g of the above mixture. Note: include up to 4 decimal places Please explain each step
- A 10.0mL (10.0g) sample of blood was found to contain lead at a concentration of 0.5ppm. What mass of lead was contained in the blood sample? (report answer in scientific notation) Please show the breakdown of how to do the problem as I get confused when steps aren't explained. Thank you!The thiourea in a 1.455 g sample of organic material was extracted into a dilute sulfuric acid solution and titrated with 37.31 mL of 0.009372 M Hg2+ via reaction: 4(NH2)2CS + Hg2+ →[(NH2)2CS]4 Hg2+ P.S. Answer only the last two letters of the following questions. (Only C and D) a. Is this an example of total analysis technique or concentration technique? Explain. b. Calculate the percent (NH2)2CS ( 76.12 g/mol) in the sample. c. What is classification of the analysis based on the amount of sample and amount of analytes present? Explain. d. If the true value is 10.00%, calculate the absolute and relative error.help with Part B Please. 5. Compare the values of Keq for each of the five solutions: a. Are any of the values outside the sample standard deviation for the set? b. Does the value of the equilibrium constant change when the concentration of either the reactants or products is altered? Why or why not? Explain this based on your calculations of Keq: c. What caused variation (three reasons) in your values of Keq? NOTE: the standard deviation is 3.9x102 The procedure is in the images Data: Unknown solution Equilibrium concentration of {FeNCS2+} in unknown solution(M) Equilibrium concentration [Fe3+](M) Equilibrium concentration [SCN-](M) Keq 1 3.7x10-5 9.6x10-4 1.6x10-4 2.4x102 2 6.2x10-5 9.4x10-4 3.4x10-4 1.9x102 3 1.1x10-4 8.9x10-4 4.9x10-4 2.5x102 4 1.1x10-4 8.9x10-4 6.9x10-4 1.8x102 5 1.8x10-4 8.2x10-4 8.2x10-4 2.7x102