le of commercial perchloric acid is 70.0% HCIO4 by mass, its density is 1.664 g/mL. How manyated HClo, would be required to prepare 500 ml of 1.50 МНО 104 solution?illiliters of this concentra. 33.0 mLb. 45.3 mLc. 54.1 mLd. 64.7 mLe. 78.6 mL

Calculate the mass of perchloric acid in the given solution,

Answered: le of commercial perchloric acid is…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 100AP

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A solution is 0.1% by mass calcium chloride. Therefore, 100. g of the solution contains g of calcium chloride.
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
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le of commercial perchloric acid is 70.0% HCIO4 by mass, its density is 1.664 g/mL. How many ated HClo, would be required to prepare 500 ml of 1.50 МНО 104 solution? illiliters of this concentr a. 33.0 mL b. 45.3 mL c. 54.1 mL d. 64.7 mL e. 78.6 mL