A certain liquid X has a normal freezing point of -1.00 °C and a freezing point depression constant K, 5.67 °C kg'mol. A solution is prepared by dissolving -1 some ammonium chloride (NH, Cl) in 850. g of X. This solution freezes at -4.0 °C. Calculate the mass of NH, Cl that was dissolved. Round your answer to 2 significant digits. 50

A certain liquid X has a normal freezing point of -1.00 °C and a freezing point depression constant K, 5.67 °C kg'mol. A solution is prepared by dissolving -1 some ammonium chloride (NH, Cl) in 850. g of X. This solution freezes at -4.0 °C. Calculate the mass of NH, Cl that was dissolved. Round your answer to 2 significant digits. 50

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

How many moles of Mg(ClO2)2 are present in 60.0 mL of 1.00 M Mg(ClO2)2 solution? Note: Answers must be numeric, not alphanumeric—42, not forty-two. Do NOT express your answer in scientific form. KEY is supplied in decimal form only: — XXX.xxxx not X.X x 102
Questions 3 and 4 below refer to the image above. А. В. Н.С C. Н | H-CH H-C-H H-C-H H-CH H-CH HC H нсн H-CH Н H С C-c CH₂ H H₂Nt H CH₂ H D. NaCI Question 3 Which of the substances shown above will freely interact with/dissolve in water? (Choose all that apply)
What is the percent by mass NaCl of a solution that contains 85.7 grams of NaCl and 104.1 grams of water? Round your answer to 1 decimal.
How many grams of copper sulfate would you need to make 4 L of a 6 M copper sulfate solution (m.w. = 160.0 g/mol)? Report your answer in the requested units. Do not report the units in your answer; enter the numbers only. It is recommended that you do not round between calculation steps.
Calculate the volume in liters of a 0.49 mol/L sodium thiosulfate solution that contains 150.g of sodium thiosulfate Na2S2O3. Be sure your answer has the correct number of significant digits.
Reagent nitric acid is 67.74% HNO3 by mass and its molarity is 14.33 M. Calculate the mole fraction of nitric acid in the solution. Express final answer with two decimal places.
A chemistry student needs 75.00 g of acetyl bromide for an experiment. She has available 150. g of a 15.9% w/w solution of acetyl bromide in benzene. Calculate the mass of solution the student should use. If there's not enough solution, press the "No solution" button. Round your answer to 3 significant digits. No х10 solution
A certain substance X has a normal boiling point of 131.5 °C and a molal boiling point elevation constant K₁ = 1.17 °C-kg-mol prepared by dissolving some urea. A solution is ((NH,),CO) in in 250. g of X. This solution boils at 133.8 °C. Calculate the mass of urea that was dissolved. Round your answer to 2 significant digits. 0 x10 X
Determine the mass of NaCl needed to make the following solution: 2.7 % NaCl in a total volume of 146 mL Give your answer in units of grams, rounded to two places after the decimal place
One half tsp of table salt (NaCl) weighs aproximately 2.0 grams. (You will need to look up the molar mass for NaCl) There are approximately 237 ml in a cup. Determine the Molarity of the solution 1 cup water with one half tsp table salt. Determine the molarity of this solution using the formula M=g/MM/L. What is the molarity? Show your calculations. (Remember to convert 237 mL to L)
Alcoholic beverages come in many different concentrations denoted by their weight percent (w/w). If a beer is marked as 10.0%, it means there are 10.0 grams of ethanol (C2H6O) in every 100.00 grams of solution. Assuming this solution has a density of 1.00 g/mL, what is the molar concentration of this solution? Give your answer in in decimal format. When entering units, use proper abbreviated units with proper capitalization.
A certain liquid X has a normal boiling point of 147.30°C and a boiling point elevation constant =Kb2.24·°C·kgmol−1. Calculate the boiling point of a solution made of 14.0g of sodium chloride (NaCl) dissolved in 750.g of X.Round your answer to 5 significant digits. (Please dont round calculations untill the end.) °C