1. Why are bubbles an issue when using the Titrette?2. The 50-mL titrette has a tolerance limit of ± 0.030 mL. What do the Titrette calculations indicatabout your technique? Support your answer using the calculated statistics.3. When measuring 40 mL, the micropipette has a tolerance limit of ± 0.8 mL. What do themicropipette calculations indicate about your technique? Support your answer using thecalculated statistics.

Titration is a laboratory technique for determining the concentration of a substance in a…

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1. Why are bubbles an issue when using the Titrette?

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter5: Errors In Chemical Analyses

Section: Chapter Questions

Problem 5.10QAP

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Students measured the concentration of HCl in a solution by titrating with different indicators to find the end point. (Use the table to find critical F values.) Mean HCl concentration (M) (+ standard deviation) Indicator Number of measurements 1. Bromothymol blue 0.09565 + 0.00170 28 2. Methyl red 0.08681 ± 0.00098 18 3. Bromocresol green 0.08641 + 0.00106 29 Is the difference between Indicators 1 and 2 significant at the 95% confidence level? O Yes O No Fenlculated clegrees of freedom Ecalculated Is the difference between indicators 2 and 3 significant at the 95% confidence level? O Yes O No Fealculated Spooled tcalculated
20.0 mL water sample was titrated with 0.0100 M EDTA solution that required 14.50 mL for CaCO3 hardness. The total hardness of the water sample in terms of CaCO3 (MW = 100.1 g/mole) in parts per million is _________? Note: Express final answer using least number of significant figures. 2. If 35.2 mL of EDTA solution is required to reach the endpoint with 0.3120-g of primary standard grade CaCO3 (MW = 100.1 g/mole), the normal concentration of the EDTA (MW = 292.24) solution is _________ N?
An EDTA solution was prepared by dissolving the disodium salt in 1 L of water. It was standardized using 0.5063 gram of primary standard calcium carbonate (MM: 100.08) and consumed 28.50 mL of the solution. The standard solution was used to determine the hardness of a 2 L sample of mineral water, which required 35.57 mL of EDTA solution. 1. What is the analyte in the analysis? Answer 2. What is concentration (M) of the EDTA solution used in the analysis? Answer 3. What is the concentration (ppm) of CaCO3 in the sample?
5. Which term is INCORRECTLY defined? a. linear range - the range over which the response of an analytical method is proportional to analyte concentration b. dynamic range concentration range over which there is a measurable response to analyte, though the response is not linear c. blank solution - a solution containing all reagents and solvents used in the analysis to which no analyte is deliberately added d. standard solutions - solutions for which the standard deviation is known - 6. True or False: Internal standards correct random error caused by run-to-run variation. a. True b. False
Please give me both right solutions.. urgenttttttttt
Jessica made 300 mL of primary standard using 2.35 g of sodium carbonate. She then conducted a titration to determine the concentration of her secondary standard, a sample of sulfuric acid. Her experimental results are in the table below. Trial 1 Trial 2 Trial 3 Trial 4 Trial 5 Volume of primary standard used 35.00 35.00 35.00 35.00 35.00 (ml) Initial burette 0.00 24.00 0.00 0.00 24.90 reading Final burette 24.70 48.85 24.80 24.90 47.95 reading (a) Determine the concentration of the secondary standard.
I PUIRE UVVIS spectrophotometry of water sample containing cobalt (Co) and nickel (Ni) is performed in a lab. In the beginning, blank reading is taken by taking in the cuvette. A Water only Both A and C Water sample having Ni and Co Co and Ni solution
Concentration sodium thiosulfate solution used: 0.056 mol L-1 ACCURATE TITRATION VOLUME OF SODIUM THIOSULFATE SOLUTION USED Volume titration 1, (ml) Volume titration 2, (ml) Your Group 15.80 15.75 Group 1 16.05 15.70 Group 2 16.30 16.25 ANALYSIS Average volume used, (mL) Standard deviation Number of moles sodium thiosulfate used, (mol) Number of moles calcium iodate in solution, (mol) Volume of calcium iodate used, (mL) Concentration of saturated calcium iodate solution (mol L-¹) Unrounded value 15.9750 0.26220 Rounded value 15.97 0.262 10.0
Concentration sodium thiosulfate solution used: 0.056 mol L-1 ACCURATE TITRATION VOLUME OF SODIUM THIOSULFATE SOLUTION USED Volume titration 1, (mL) Volume titration 2, (mL) Your Group 15.80 15.75 Group 1 16.05 15.70 Group 2 16.30 16.25 ANALYSIS Average volume used, (ml) Standard deviation Number of moles sodium thiosulfate used, (mol) Number of moles calcium iodate in solution, (mol) Volume of calcium iodate used, (mL) Concentration of saturated calcium iodate solution (mol L-¹) Unrounded value 15.9750 0.26220 0.00089400 0.00036700 A Rounded value 15.97 0.262 8.94 x 10-4 10.0 Minimize
Consider Table 1, which lists the volumes of the Fe3+ and SCN- solutions used for the continuous variation method. Note that each of the stock solutions is 0.002 M before mixing. What are the initial concentrations of Fe3+ and SCN- for solution 4, where the volumes are both 5 mL? [Initial meaning after they are mixed, but before]they reach equilibrium)
The sample containing 4.2 % NaCl will be determined gravimetrically as AgCl. What weight (in milligrams) of the sample must be taken to obtain a precipitate that will weigh about 0.39 mg? FM: NaCl = 58.44 AgCl = 143.3 %3D Answer in two decimal places. Do not include units in the answer. Answer:
Standardization of 0.10 M HCl1. Take three (3) clean and properly labeled 250-mL Erlenmeyer flasks. Into the three flasks, weigh 0.1 g of the primary standard Na2CO3 to the nearest 0.1 mg. Record the weights of the primary standard.2. Add about 75.0 mL of boiled distilled water and swirl to dissolve the solids.3. Add 2 to 3 drops of phenolphthalein indicator. Record the initial burette reading and titrate with the prepared 0.10 M HCl solution until phenolphthalein endpoint.4. Record the final burette reading for each titration in your data sheetDetermination of Ksp and Molar Solubility1. Add Ca(OH)2 to 250.0 mL distilled water with stirring until equilibrium is achieved. 2. Filter the undissolved precipitate. Measure out 50.0 mL of the supernate into a 250-mL Erlenmeyer flask using a pipette.3. Add a few drops of phenolphthalein indicator and titrate with standardized HCl solution until endpoint is achieved.4. Record the volume the HCl solution used. Perform two more trials.…