23. What is the concentration (by mass) of the solute in a 25 °C solution prepared by dissolving 2.50x10 mol Na3PO4 in 1.000L of water (in ppm, ppb, and ppt, all to two decimal places)? A: 4.00 x 10- ppm; 4.10 × 10' ppb; 4.10×10* ppt
23. What is the concentration (by mass) of the solute in a 25 °C solution prepared by dissolving 2.50x10 mol Na3PO4 in 1.000L of water (in ppm, ppb, and ppt, all to two decimal places)? A: 4.00 x 10- ppm; 4.10 × 10' ppb; 4.10×10* ppt
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter12: Solutions
Section: Chapter Questions
Problem 12.61QP: Concentrated hydrochloric acid contains 1.00 mol HCl dissolved in 3.31 mol H2O. What is the mole...
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Step 1
According to question
No. Of moles = 2.50× 10-7
Volume = 1L
So, Molarity = no. Of moles/Volume(L)
= 2.50×10-7 /1 = 2.50×10-7 M
Mass percentage =
Mass of solute/Mass of solution ×100
Mass of solute = 2.50×10-⁷ × 163.941 (molar mass of Na3PO4 )
= 4.098×10-⁵ g
Mass of solution = mass of solvent + water
= 4.098×10-⁵ + 1000 = 1000.00004g (density of water taken as 1g/ml)
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