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 3.40-g sample of a mixture of naphthalene (C₁₀H₈) and pyrene (C₁₆H₁₀) is dissolved in 35.0 g benzene (C₆H₆). The freezing point of the solution is 2.29°C. What is the mass (in grams) of the naphthalene in the sample mixture? The freezing point of benzene is 5.51°C and Kf is 5.12°C･kg/mol.
When 571. mg of a certain molecular compound X are dissolved in 60.0 g of benzene (CH), the freezing point of the solution is measured to be 4.8 °C. Calculate the molar mass of X. If you need any additional information on benzene, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to the correct number of significant digits. 0 X x10 S
15.2 g of camphor dissolved in naphthalene lower the freezing temperature of naphthalene from 80.0 °C to 75.0 °C. What is the mass of naphthalene? The molal freezing depression point constant for naphthalene is: Kf = 7.00 °C/m . Both naphthalene and camphor are non-electrolytes, and the molar mass of camphor is about 152 g/mol.
Ethylene glycol, HOCH2CH2OH, is a common automobile antifreeze. It is water-soluble and fairly nonvolatile (boiling point = 197°C). Calculate the freezing point of a solution containing 568 g of this substance in 2621 g of water.
Calculate the boiling point (in oC) of an aqueous solution which is 0.347 m in potassium carbonate. Your answer should go to two places beyond the decimal point. (as an example: 105.21) As usual do not include the oC in your answer. Kb = 0.52 oC/m
The normal freezing point of a certain liquid x is -6.20 °C, but when 36. g of iron(III) chloride (FeCl,) are dissolved in 300. g of x the solution freezes at -9.4 °C instead. Use this information to calculate the molal freezing point depression constant K, of x. Round your answer to 2 significant digits. do °C · kg K, = 0- mol ?
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
A typical coal-fired electric generating plant will burn about 3 metric tons of coal per hour. Most of the coal burned in the United States contains 1 to 4 % by weight sulfur in the form of pyrite, which is oxidized as the coal burns: 4FeS2(s) + 11 O₂(g) 2 Fe2O3(s) + 8 SO2(9) Once in the atmosphere, the SO2 is oxidized to SO3, which then reacts with water in the atmosphere to form sulfuric acid: SO3(9) + H₂O(1)→→→→→→→ H₂SO4(aq) If 42.4 metric tons of coal that contains 1.44 % by weight S is burned and all of the sulfuric acid that is formed rains down into a pond of dimensions 397 m x 256 m x 4.96 m, what is the pH of the pond? (OK to assume 2 mol H30+ per mole H₂SO4.) Hint: 1 metric ton = 1000 kg
Compound XY is an ionic compound that dissociates as it dissolves in water. The lattice energy of XY is -594.4 kJ mol1. The hydration energy of its ions is -626.2 kJ mol-1. Write the thermochemical equations for the two steps in the formation of a solution of XY in water. Draw an enthalpy diagram for the formation of this solution. What is the net AH for the formation of a solution of XY? i kJ mol-1
The freezing point of a liquid will change when a solute is added. Explain how the addition of salt impacts the boiling point of water. Calculate the freezing point change for a given concentration. Given that water's freezing point is 0.00°C and the freezing point depression constant (Kf) is 1.86 °C·kg/mol, calculate the freezing point depression for a 2.80 molal solution (moles/kg) of CaCl, in water. Assume ideal behavior of the ions. 21 MacBook Air 吕0 888 F1 F2 F3 F4 F5 F7 ! @ $ % & 1 3 6. 7 8. Q W E R Y
પાયલ બહેન
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.