[References]A chemist wants to prepare 0.740 M HCI, Commercial hydrochloric acid is 12.4 M. How many milliliters of the commercial acid does the chemist require to make up 1.40 L of the dilute acid?Try Another Version3 item attempts remainingSubmit Answer(PreviousNextSave andCengage Learning | Cengage Technical SupportLab 1 (3).pptxChapter 8 pres...pptxLab 1.pdfLab 6.pdflab 5.pdfD Lab 4.pdfnoys

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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A 2.00 L bottle of concentrated BBQ solution was purchased for the cookout. The solution contained 868.8 g of BBQ powder. What is the molarity of the solution? (The solution was prepared by dissolving BBQ powder(36.5 g/mol) in water.) 11.9 M 2.3 M 0.43 M 1.19 M not enough information to determine answer
Calculate the molarity of a solution made by dissolving 10.1 g NaNo3 (s) in water to make 350 mL of solution. Thank you i need help
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Common laboratory acids and bases Formula Label concentration Molarity Name Acids Acetic acid HC, H3O2 Glacial 18 Acetic acid HC,H,O2 Dilute 6. Bases NH3 Concentrated 15 Aqueous ammonia Aqueous ammonia NH3 None usually given 6. Often erroneously called ammonium hydroxide and given the formula NH,OH. a How many milliliters of concentrated aqueous ammonia are required to prepare 250 mL of 0.173 M NH3? Volume = mL 6 How many liters of glacial acetic acid are required to prepare 4.00 L of 0.286 M HC2 H3O2? Volume =
B. 55.3605% C. 60.7023% D. 61.9649% 33. In standardizing a solution of NaOH (40 g/mol) against 1.431 g of KHP (204.22 g/mol), the analyst uses 35.50 ML of the alkali and has to run back with 8.25 mL of acid (1 mL 10.75 mg NaOH). What is the molarity of the NaOH solution? A. 0.8520 M B. 0.6546 M C. 0.4572 M D. 0.2598 M 34. A sample of a pyrolusite weighs 0.5000 g. To this is added 0.6674 g of As203 and dilute acid. After solvent action has ceased, the excess three-valent arsenic is titrated with 45.00 mL of 0.1000 N KMNO4. Calculate the oxidizing power of the pyrolusite in tems of percentage MnO2. A. 78.1506% B. 55.8107% C. 39.0006% D. 19.5003% 35. A solution of iodine is such concentration that 20.00 mL are required to titrate the antimony in a 0.100 g sample containing 84.93% Sb2S3 (339.7 g/mol). What is the value of 1.00 mL of this iodine in terms of grams of sulfur in titration? A. 0.0248 N B. 0.0496 N C. 0.0744 N D. 0.1489 N 3.
Question 4 Ethanol has a Kb of 1.22 °C/m and usually boils at 78.4 °C. How many mol of an nonionizing solute would need to be added to 45.42 g ethanol in order to raise the boiling point to 82.4. Submit Question 280 45,195 APR
I Review I Constants I Periodic T A KNO3 solution is made using 82.4 g of KNO3 and diluting to a total solution volume of 1.20 L. Calculate the molarity of the solution. Submit Request Answer Part B Calculate the mass percent of the solution. (Assume a density of 1.03 g/mL for the solution.)
In the laboratory you dilute 3.53 mL of a concentrated 6.00 M hydrobromic acid solution to a total volume of 175 mL. What is the concentration of the dilute solution M Submit Answer & Next
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Try Another Version Submit Answer 3 item attempts remaining A chemist wants to prepare 0.740 M HCI, Commercial hydrochloric acid is 12.4 M. How many milliliters of the commercial acid does the chemist require to make up 1.40 L of the dilute acid? [References]