A college student is trying to determine thefreezing point of an aqueous solution. Heknow it will be less than 0°C because of theconcept of freezing point depression (waterhas a freezing point of 0°C, so the solution willhave one lower). Here is the information hehas:· Solute: Ammonium phosphate,(NH4)3PO4, molar mass of approximately149 g/mol. i = 4Kf for water = -1.86 °C/m· Amount of solute: 74.5 g (NH4)3PO4· Amount of water (solvent): 425 g H201) Calculate the molality (m = mol solute / kg%3Dsolvent).2) Determine the freezing point of thesolution; show your work.3) Suppose he switched the ammoniumphosphate for a different solute, potassiumchloride. Explain how that change would alterthe freezing point. Justify your answermathematically.

As a non volatile substance is added to a solvent,the freezing point of solvent is depressed. It is…

A college student is trying to determine the freezing point of an aqueous solution. He know it will be less than 0°C because of the concept of freezing point depression (water has a freezing point of 0°C, so the solution will have one lower). Here is the information he has: · Solute: Ammonium phosphate, (NH4)3PO4 , molar mass of approximately 149 g/mol . i = 4 • KĘ for water = -; -1.86 °C/m · Amount of solute: 74.5 g (NH4)3PO4 · Amount of water (solvent): 425 g H20 1) Calculate the molality (m = mol solute / kg solvent). 2) Determine the freezing point of the solution; show your work. 3) Suppose he switched the ammonium phosphate for a different solute, potassium chloride. Explain how that change would alter the freezing point. Justify your answer mathematically.

A college student is trying to determine the freezing point of an aqueous solution. He know it will be less than 0°C because of the concept of freezing point depression (water has a freezing point of 0°C, so the solution will have one lower). Here is the information he has: · Solute: Ammonium phosphate, (NH4)3PO4 , molar mass of approximately 149 g/mol . i = 4 • KĘ for water = -; -1.86 °C/m · Amount of solute: 74.5 g (NH4)3PO4 · Amount of water (solvent): 425 g H20 1) Calculate the molality (m = mol solute / kg solvent). 2) Determine the freezing point of the solution; show your work. 3) Suppose he switched the ammonium phosphate for a different solute, potassium chloride. Explain how that change would alter the freezing point. Justify your answer mathematically.

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 10.27 g sample of a weak acid (HA) is dissolved in 509.0 g of water. The freezing point of the solution is -0.368 °C. The molar mass of the weak acid is 93.0 g/mol. Calculate the acid dissociation constant, K,, of the weak acid. K₁ = 8.17 X10-2 Incorrect
પાયલ બહેન
When 4.13 g of a certain molecular compound X are dissolved in 35. g of cyclohexane (C6H₁2), the freezing point of the solution is measured to be 3.7 °C. Calculate the molar mass of X.
At 55.0 ∘C∘C, what is the vapor pressure of a solution prepared by dissolving 75.8 g of LiF in 247 g of water? The vapor pressure of water at 55.0 ∘C∘C is 118 mmHg. Assume complete dissociation of the solute.
The vapor pressure of pure water at 70°C is normally 233.7 mmHg, but decreased to 227.4 mmHg upon addition of an unknown amount of sodium hypochlorite, NaOCl, to 242.9 g of water at this temperature. How many grams of sodium hypochlorite were added? Assume complete dissociation of solute.
Use the References to access important values if needed for this question. An aqueous solution of phosphoric acid, that is 0.500 percent by weight phosphoric acid, has a density of 1.0010 g/mL. A student determines that the freezing point of this solution is -0.122 °C. Based on the observed freezing point, what is the percent ionization of the acid and the value of K1? Assume that only the first ionization of the acid is important. Ke for H,O is 1.86 °C/m. % ionized =
The concentration of NaCl(aq) in a beaker is 2.00 M. What is the molality of the NaCl solution?(Molar mass of NaCl is 58.44 g·mol-1 and density of NaCl(aq) is 1.07 g/cm3)?:A 1.53 B 2.10 C 2.71 D 3.02 E 3.52
Which solution will have the highest freezing point?
Camphor is a white solid that melts at 179.50°C. It has been used to determine the molecular weights of organic compounds because of its unusually large freezing-point-depression constant (39.7°C/m), which allows ordinary thermometers to be used. The organic compound is dissolved in camphor, and then the melting point of the solution is determined. If 1.08 g of an unknown compound is dissolved in 73.6 g camphor, the freezing point is found to be 177.09°C. What is the molecular weight of the unknown compound?
A certain liquid X has a normal freezing point of -6.90 °C and a freezing point depression constant K=3.91 °C·kgmol . Calculate the freezing point of a solution made of 146.g of iron(III) chloride (FECI,) dissolved in 900. g of X. Round your answer to 3 significant digits.
What is the freezing point of a solution that is made by dissolving 36.8 grams of potassium hydroxide, KOH, in 1000 grams of water? Assume that KOH dissociates completely into ions when it dissolves. freezing point= "C
Calculate the molality of each of the following aqueous solutions. Part 1 of 2 2.80 M NaCl (density of solution Part 2 of 2 m x10 m X x10 - X 1.08 51.7 percent by mass KBr solution. Round your answer to 3 significant digits. Ś g −). Round your answer to 2 significant digits. mL Ś