Part A that contains 0.0745 mol? Aspirin, CgH8O4, is a common pain reliever and is also often given in low doses daily for prevention of heart attacks. How many grams of aspirin are present in a sample ► View Available Hint(s) 0.000414 g 13.421473 g Next > 55°F Mostly clear ^ @ 4») @ 9:45 PM 4/29/2022 S delete home prt sc ← backspace Ⓒ2420 g 13.4 g Submit Provide Feedback B = 0 search NO ICDI % H H hp K 0 0 (23) num lock Onter See product reviews demos, offers and featu ** home COF

Part A that contains 0.0745 mol? Aspirin, CgH8O4, is a common pain reliever and is also often given in low doses daily for prevention of heart attacks. How many grams of aspirin are present in a sample ► View Available Hint(s) 0.000414 g 13.421473 g Next > 55°F Mostly clear ^ @ 4») @ 9:45 PM 4/29/2022 S delete home prt sc ← backspace Ⓒ2420 g 13.4 g Submit Provide Feedback B = 0 search NO ICDI % H H hp K 0 0 (23) num lock Onter See product reviews demos, offers and featu ** home COF

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter3: Statistical Tests With Excel

Section: Chapter Questions

Problem 1P

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and Employees CH STATE GE 90 ENDULERSE IS FOREVER "ON-Tame Name Jodi Rayal Molarity = wt. x1000 3. Calculate the massof Potassium hydrogen phthalate (KHP) to prepare a 250.0 mL solution of 0.1000 M KHP solution. Mol ut. x Voluse the 2500×1000 204.22250 mass Initial Buret Reading Final Buret Reading Vol NaOH Added Moles of NaOH Moles of HCI Volume of unknown HCI solution Concentration of HCI Average concentration of HCI of KHP = 5.11g 4. Complete the table below for the following neutralization reaction of an unknown concentration of hydrochloric acid with 0.100 M sodium hydroxide: Mu spate solution Trial 1 0 11.15 го data and calculate the concentration 15 Trial 2 11.15 22.15 Trial 3 22.15 33.25 abyh 067 LANDINUKASHU TROWTHCENTISSATE ARAD Ma That par މއކނި REMURNAR MISAMARALISERDRY Tile
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 aluminum in a 1.200-g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous Al2O3.xH2O. The precipitate was filtered and ignited at to give anhydrous Al2O3, which weighed 0.2001 g. Express the result of this analysis in terms of %NH4Al(So4)2 %Al2O3 %Al
A solution is prepared by dissolving 30g CH₃COOH (CH₃COOM = 60g/mol MM) in water and the final volume of the solution is 250 mL/5M. What is the molarity of the solution?
the volume is 207.16ml for the "Dry" oxygen at STP.. I need to determine the purity of the orginal potassium chlorate sample. Do I need moles of oxygen? (Moles)/(0.765g)X100% ??
How many grams of GaAs04 are required to prepare 2800 mL. of dissolution 0.035 N. ?
A solution is prepared by dissolving 155.0 mL of methanol (CH3OH, density = 0.791 g/mL) in 250 mL of water (density 1.00 g/mL) to give a final solution volume of 350.0 mL. Calculate the (a) molarity of the solution, (b) %wt/wt, (c) %wt/vol, (d) %vol/vol
25.0mL of a 0.515 M K2S solution is mixed with 30.0 mL of 0.833 M HNO3 acid solution to give the following reaction: K2S(aq) + 2HNO3(aq) → 2KNO3(aq) + H2S(g) H2S is an unwanted by-product in a pulp and paper industry. To capture H2S gas, it is bubbled through a NaOH solution to produce Na2S with a yield of 94%. H2S(g) + 2NaOH (aq) → Na2S (aq) + 2H2O(l) The mass of H2S(g) that was processed (in kg) if 10.76 kg of Na2S was collected is
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Water and acetonitrile, CH3CN, are miscible (can be mixed in any proportions). However, whenwater and acetonitrile are mixed, the volumes are not additive (the total volume of the resultingsolution is not equal to the sum of the pure liquid volumes). For example, when 100.0 mL ofwater and 100.0 mL of CH3CN(l), are mixed at 20 °C, the total volume of the solution is 192.0mL,not 200.0 mL.a. Provide an explanation for this phenomenon.b. Calculate the molarity, molality and mol fraction of CH3CN in a solution preparedby mixing 100.0 mL of water and 100.0 mL of CH3CN(l) at 20 °C. The total volume of themixture is 192.0 mL and the densities of water and acetonitrile are 0.998 g/mL and 0.782g/mL, respectively, at this temperature.c. When 70.0 g H2O and 190.0 g CH3CN(l) are mixed, to resulting solution has adensity of 0.860 g/mL at 20 °C. Calculate the volumes of the pure liquid samples and thesolution, and show that the pure liquid volumes are not additive.
When concentrated sulfuric acid is sold to chemist, the label contains no mentionof the molarity of the acid. Determine the volume of the acid needed to prepare500 mL, 0.5 M H2SO4 from the commercial H2SO4 that is 98% (w/w) and density1.80 g/mL.
Bleach is a 6.0% (mass/volume) solution of NaClO. That means that there are 6 grams of NaClO(MM = 74.44 g/mol) per 100 mL of bleach. Calculate the molarity (mol/L) of NaClO in bleach tothree significant figures (one extra sig fig).