Help me answer part b Part AHow many milliliters of a stock solution of 7.0 M HNO3 would you have to use to prepare 110 mL of 0.500 M HNO3?Express the volume in milliliters to two significant figures.V=9.17 mL4SubmitPrevious AnswersCompletedPart BIf you dilute 17.0 mL of the stock solution to a final volume of 0.300 L, what will be the concentration of the diluted solution?Express the molarity in moles per liter to three significant figures.Molarity=VΟ ΑΣΦSubmitRequest AnswerProvide FeedbackMLG

4 Part B If you dilute 17.0 mL of the stock solution to a final volume of 0.300 L, what will be the concentration of the diluted solution? Express the molarity in moles per liter to three significant figures. ΜΕ ΑΣΦ Molarity= Submit Request Answer ? M

4 Part B If you dilute 17.0 mL of the stock solution to a final volume of 0.300 L, what will be the concentration of the diluted solution? Express the molarity in moles per liter to three significant figures. ΜΕ ΑΣΦ Molarity= Submit Request Answer ? M

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

Chapter4: Types Of Chemical Reactions And Solution Stoichiometry

Section: Chapter Questions

Problem 101AE: You wish to prepare 1 L of a 0.02-M potassium iodate solution. You require that the final...

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When 10. L of water is added to 3.0 L of 6.0 M H2SO4, what is the molarity of the resulting solution? Assume the volumes are additive.
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A student tries to determine experimentally the molar mass of aspirin (HAsp). She takes 1.00 g of aspirin, dissolves it in water, and neutralizes it with 17.6 mL of 0.315 M KOH. The equation for the reaction is HAsp(aq)+OH(aq)Asp(aq)+H2OWhat is the molar mass of aspirin?
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39. Standard solutions of calcium ion used to test for water hardness are prepared by dissolving pure calcium carbonate. CaCO3, in dilute hydrochloric acid. A 1.745-g sample of CaCO3 is placed in a 250.O-mL volumetric flask and dissolved in HCI. Then the solution is diluted to the calibration mark of the volumetric flask. Calculate the resulting molarity of calcium ion.
What is the molarity of pure water with a density of 1.00 g/mL?
The units of parts per million (ppm) and parts per billion (ppb) are commonly used by environmental chemists. In general, 1 ppm means 1 part of solute for every 106 parts of solution. Mathematically, by mass: ppm=gsolutegsolution=mgsolutekgsolution In the case of very dilute aqueous solutions, a concentration of 1.0 ppm is equal to 1.0 g of solute per 1.0 mL, which equals 1.0 g solution. Parts per billion is defined in a similar fashion. Calculate the molarity of each of the following aqueous solutions. a. 5.0 ppb Hg in H2O b. 1.0 ppb CHCl3 in H2O c. 10.0 ppm As in H2O d. 0.10 ppm DDT (C14H9Cl5) in H2O