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A measurement of the mass of a specimen was determined to be 4.203 plus or minus 0.001 g. What is the fractional uncertainty in the mass?
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- Take the mass measurement with nitrogen (28 dalton or atomic mass units per molecule) and the mass measurement with helium (4 daltons per atom) and use the difference between the measured masses to find the mass of 1 dalton (one atomic mass unit) in grams. The standard value of the dalton is 1.66053906660×10−27 kg with an uncertainty of ±50 in the last two figures. Can you identify the sources of error in your measurement?1) Perform the indicated mathematical operations. State the uncertainty of the final answer as ± 1-digit variation in the least significant digit. (remember that the last significant digit's place holder is the most uncertain digit!) 7.700 x 2.1 = uncertainty: 2.132 + 17 + 4.04 = uncertainty: 27000 + 500 = uncertainty: 30.0 x 50.0 = uncertainty: (9.6 × 107)(1.24 × 10³)_ uncertainty: 1.897 x 102During a titration experiment, 50.00 mL of a certain solution needs to be transferred to an Erlenmeyer flask. To measure the volume, a student used a calibrated 10-mL pipette five times. If the pipette delivers an actual volume of 9.98 mL with an uncertainty of ±0.02 mL, what will be the uncertainty in the final volume?
- What is the percentage uncertainty with the following measurement 0.100 ± 0.005 g? Provide your answer to one decimal point.In order to find the density of a solution of unknown density, 10 mL of solution was drawn into a clean and dry beaker three times with a pipette and weighed and the weighing results were found to be 65.1452 g, 64.9982 g, 65.1027 g. Calculate the density of the solution and the standard deviation of the measurements, since the empty weight of the beaker is 52.2461 g.A sodium chloride solution was prepared by dissolving 0.0998 \pm 0.0005 g NaCI (58.443 \pm 0.001 g/mol) in 100.00 \pm 0.08 mL of water. Calculate the concentration of NaCl in the solution and its absolute uncertainty. Report the concentrationwith the appropriate number of significant figures.
- 7. 22 This question is about several salts. (a) A hydrated salt, compound A, is analysed and has the following percentage composition by mass: Cr, 19.51%; CI, 39.96%; H, 4.51%; O, 36.02%. Calculate the formula of compound A, showing clearly the water of crystallisation. Show your working. formula of compound A = (b) A student carries out an experiment to determine the amount of water of crystallisation in the formula of another hydrated salt. The student intends to remove the water by heating the hydrated salt. A diagram of the apparatus used by the student is shown below. crucible pipeclay triangie The student adds the hydrated salt to the crucible and weighs the crucible and contents. The student heats the crucible and contents and allows them to cool. The student weighs the crucible and residue. The student's results are shown below. 16,84 Mass of crucible + hydrated salt/g 16.26 Mass of crucible + residue after heating/gExpress the corresponding readings, taking into account the figures that you can read with certainty and the estimated figure. Remember to add the uncertainty, (±), to your measure.A researcher would like to determine whether there is any relationship between students’ grades and where they choose to sit in the classroom. Specifically, the researcher suspects that the better students choose to sit in the front of the room. To test this hypothesis, the researcher asks her colleagues to help identify a sample of n = 100 students who all sit in the front row in at least one class. At the end of the semester, the grades are obtained for these students and the average grade point average is M = 3.25. For the same semester, the average grade point average for the entire college is μ = 2.95 with σ = 1.10. Use a two-tailed test with α = .01 to determine whether students who sit in the front of the classroom have significantly different grade point averages than other students.NOTICE that you are asked to use α = .01! A) sig., p<.01 B) N.S. ("not significant"), p>.01 C) sig., p>.01 D) N.S., p<.01
- A solution of F− is prepared by dissolving 0.0944±0.0006 g NaF (molar mass = 41.989±0.001 g/mol) in 162.00±0.06 mL of water. Calculate the concentration of F− in solution and its absolute uncertainty. To avoid rounding errors, do not round your answers until the very end of your calculations.To prepare a solution of NaCI, you weigh out 2.634 (to.002) g and dissolve it in a volumetric flask whose volume is 100.00 (±o.08) mL. Express the molarity of the solution, along with its uncertainty, with an appropriate number of digits.A concentration solution of hydrochloric acid has a concentration of 1.202 (± 0.005) M. If 14.00 (± 0.07) mL of this solution is placed in a 250.00 (± 0.05) mL volumetric flask and water is added to the mark, what is the absolute uncertainty reported to the correct number of significant figures for the dilute concentration of HCl?
