17.100 ml of 5:3:2 ethylene: chloroform: isoamyl alcohol18. Convert 50 ppm to g/L19. Convert 50 ppm to mg/L20. Convert 5 ppb to ul/l How would you prepare the following solutions? Unless stated otherwise, assume that thesolvent is purified water and that you will dissolve the solute in a lesser amount of solvent andthen “bring the solution to volume"CuSO4 FW 159.61Nacl FW 58.44CaCl FW 111.0NazSO4 · 10H2O FW 322.04

17.100 ml of 5:3:2 ethylene: chloroform: isoamyl alcohol Add 50ml ethylene + 30ml chloroform + 20ml…

Answered: 17.100 ml of 5:3:2 ethylene:…

17.100 ml of 5:3:2 ethylene: chloroform: isoamyl alcohol 18. Convert 50 ppm to g/L 19. Convert 50 ppm to mg/L 20. Convert 5 ppb to ul/l

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...

See similar textbooks

Similar questions

A certain liquid X has a normal freezing point of -3.10 °C and a freezing point depression constant K₁=5.02 °C-kg-mol. A solution is prepared by dissolving some sodium chloride (NaCl) in 300. g of X. This solution freezes at -4.1 °C. Calculate the mass of NaCl that was dissolved. Round your answer to 2 significant digits. 1 g 1 x10
114.7 mg of NaCl (MM=58.44 g) is dissolved in 246.42 L of water. What is the concentration of Na+ ion (MM=22.99 g/mol) in ppm? Give your answer rounded to four digits to the right of the decimal point. Hint: If you are stuck, calculate the %w/w of Na in NaCl using the molar masses - from pe106. Convert g to mg.
A chemist mixes 59.3 g of acetone with 97.8 g of 2-ethyltoluene and 47.1 g of isopropenylbenzene. Calculate the percent by mass of each component of this solution. Be sure each of your answer entries has the correct number of significant digits. component mass percent x10 % acetone 2-ethyltoluene isopropenylbenzene 0%
A certain liquid X has a normal boiling point of 105.30 °C and a boiling point elevation constant K₁ = 1.74 °C-kg-mol¯¹. Calculate the boiling point of a solution made of 8.59g of ammonium chloride (NHCl) dissolved in 150. g of X. Round you answer to 5 significant digits. пос x10 X
Grams of solute per 100 g H₂O 140 130 120 110 100 90 80 70 60 50 40 30 20 10 NH37 NaNO3 KCIO3. KNO3 NHẠC KCI Naci -Ce₂(SO4)3 0 10 20 30 40 50 60 70 80 90 100 6. How many grams of KCI can be dissolved in 100g of water at 80°C? 7. At 40°C, how much KNO3 can be dissolved in 100g of water? 8. At 30°C, 90g of NaNO3 is dissolved in 100g of water. Is this solution saturated or unsaturated? 9. How could you tell by looking at a solution that was saturated? 10. A vinegar brand contains 4% acetic acid by volume. If the density of vinegar is 1.05 g/ml, how many grams of acetic acid are in a 250.0 mL of vinegar? 19
Given that the solubility of salicylic acid at room temperature is 0.2 g/100 mL of water? How much water should be used to dissolve 100 mg of impure salicylic acid. Consider the impurity to be an insoluble solid. Group of answer choices 100 mL 500 mL 200 mL 50 mL
Using the cooling curve (shown above), identify the freezing temperature for the solution. A. 6°C B. 0°C C. −8°C D. −8.5°C E. −9°C
A 147. ml. solution was made by mixing 98.0 mL of cyclohexane, which has a density of 0.78 g/ml., and 47.7 ml. of toluene, which has a density of 0.87 g/mL.. Calculate the volume percent of cyclohexane in this solution. Be sure your answer has the right number of significant digits. %(w/v) X 5
You need to analyze an aqueous alcohol solution in the laboratory. You separated 367 mL of this solution and diluted with 40 mL of water. You then get 50 mL of the resulting solution and mixed with 50 mL 30% v/v aqueous alcohol solution. You analyzed the final solution and found out that it's concentration is 40% v/v alcohol. How much alcohol in mL does the initial solution contains?"
Macmillan Learning A 43.8 g sample of ground water is found to have a lead concentration of 13.31 ppm. Calculate the mass of lead in the sample in milligrams. mass: mg
5-10
Data Table Mass of Zn HCI Volume Tinitial Tfinal 0.55 g 100.0 mL 20.0 °C 23.1°C The density of the 6M HCI is 1.07 g/mL. Which of the following shows how to convert the volume of the solution used into grams of solution? O a. 100.0 mL x 1mL 1.07 g Ob. 1.07 g 100.0 mL 1.07 g 1ml OC. 100.0 ml x The amount of heat absorbed by the solution can be found using the equation q = m x SH x AT. It can also be written as qsolution = msolution X SHsolution X ATsolution: We can assume that the specific heat of the solution is the same as the specific heat of water which is 1.00 cal/(g °C). Data Table Mass of Zn HCI Volume T;initial Tfinal 0.55 g 100.0 mL 20.0 °C 23.1°c Which of the following shows the correct calculation of gsolution? cal "x 3.1°C g°C O a. 100.0 mL x 1.00 Ob. cal 107 grams x 1.00 g °C х 3.1°C 0.55 grams x 1.00 cal х 3.1°C g °C