A) Determine the ionic formula of one Cr+6, 4 oxygen atoms (polyatomic ion with a charge of -8) and 2H+ ions. B) Find the molar mass of one mole of the compound in part A. C) The Michigan standard for the maximum permissible level of Cr+6 in ground water is 0.10 mg/L. You take 1.00 Liter of ground water and discover that there is 0.15 mg of Cr+6 present. Convert 0.15mg of Chromium (the +6 charge does NOT change the molar mass) to moles of Cr. D) How many formula units of H2CrO4 are in the number of moles of Cr+6 you calculated in part C? r
A) Determine the ionic formula of one Cr+6, 4 oxygen atoms (polyatomic ion with a charge of -8) and 2H+ ions. B) Find the molar mass of one mole of the compound in part A. C) The Michigan standard for the maximum permissible level of Cr+6 in ground water is 0.10 mg/L. You take 1.00 Liter of ground water and discover that there is 0.15 mg of Cr+6 present. Convert 0.15mg of Chromium (the +6 charge does NOT change the molar mass) to moles of Cr. D) How many formula units of H2CrO4 are in the number of moles of Cr+6 you calculated in part C? r
Chemistry
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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) Determine the ionic formula of one Cr+6, 4 oxygen atoms (polyatomic ion with a charge of -8) and 2H+ ions.
B) Find the molar mass of one mole of the compound in part A.
C) The Michigan standard for the maximum permissible level of Cr+6 in ground water is 0.10 mg/L. You take 1.00 Liter of ground water and discover that there is 0.15 mg of Cr+6 present. Convert 0.15mg of Chromium (the +6 charge does NOT change the molar mass) to moles of Cr.
D) How many formula units of H2CrO4 are in the number of moles of Cr+6 you calculated in part C?
r
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