How can I solve this question? I need full details and accurate answer. Calculate the freezing point of a 10.50 m aqueous solution of sucrose. Freezing point constants can be found in the list ofcolligative constants.T =°C Coligative ConstantsamacmillanlearningChempendixConstants for freezing-point depression and boiling-point elevation calculations at 1 atm:K{ value* Normal freezing K, value Normal boiling(°C/ m)SolventFormula(°C/ m)point ( °C)point (°C)H20C 6H6Physical Constants1.860.000.512100.00waterbenzene5.125.492.5380.1Acids and Basesсyclohexane C sН 12C2H6020.86.592.9280.7Activity Coefficientsethanol1.99|-117.31.2278.4carbonCCI 429.8-22.95.0376.8tetrachlorideActivity SeriescamphorC 10 H 16 O 37.8176Amino AcidsRoiling Dointc

Answered: Calculate the freezing point of a 10.50…

Calculate the freezing point of a 10.50 m aqueous solution of sucrose. Freezing point constants can be found in the list of colligative constants. Tf = °C

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter11: Properties Of Solutions

Section: Chapter Questions

Problem 88E: The freezing-point depression of a 0.091-m solution of CsCl is 0.320C. The freezing-point depression...

See similar textbooks

Related questions

Q: Calculate the molality of a sulfuric acid solution (density = 1.230 g/mL) whose concentration is…

A: molarity is defined as defined as no of moles of solute devided by volume of solution in liter.

Q: What is the freezing point in degrees Celsius of a solution prepared by dissolving 15.6 g aluminum…

A: The freezing point of a substance represents the temperature at which there exists an equilibrium…

Q: Determine the molal concentration of a sugar solution in water that has a freezing point of –2.1°C.…

A: Given information, Freezing point = –2.1°C Value of Kf = 1.86°C/m for water

Q: Calculate the molality of chloride ions in an aqueous solution of magnesium chloride in which the…

A: To solve this problem we will use the formula of molality

Q: Calculate the molality of a sucrose solution made by dissolving 39.5 grams sucrose into 99.6 grams…

Q: Calculate the molality of a sulfuric acid solution (density = 1.230 g/mL) whose concentration is…

A: Given, Density of sulfuric acid solution is 1.230 g/mL. Concentration of sulfuric acid is 1.25M.…

Q: Determine the molality of an aqueous solution prepared by dissolving 0.112 moles of LiCl in 13.7…

Q: has been transferred from areas As a system reaches thermal equilibrium, of high to low A) solute;…

A: The heat or thermal energy flows from the high-temperature area to the low-temperature area.

Q: Calculate the molality of a 0.410 molar aqueous glucose solution whose density is 1.15 g/mol

Q: Calculate the freezing point of a 10.00 m aqueous solution of ethylene glycol. Freezing point…

Q: Determine the molality of a solution prepared by dissolving 75g of Ba(NO3)2(s) in 374g of water at…

A: Given that: mass of Ba(NO3)2(s) = 75 g mass of water = 374 g To find: molality of a solution?

Q: Assuming 100% dissociation in aqueous solution, calculate the freezing point of a solution made by…

A: It is given that there is 100 % dissociation of NaCl in the solution. Mass of NaCl = 16.94 g The…

Q: 1. Estimate the freezing and normal boiling points of 0.25 m aqueous solutions of NH4NO3 and NiCl3

A: Any solution's "boiling point (Tb)", as well as "freezing point(Tf)", is directly related to the…

Q: Calculate the osmotic pressure in bar units glucose aqueous solution at 25.000C with a concentration…

A: Temperature = 25.00°C ...Or because °C + 273 = k ...So 25.00 °C + 273 = 298 k Concentration =…

Q: Explain the meaning of the van’t Hoff factor and its role in determining the colligative properties…

A: Colligative properties are the properties which are dependent on the number of solute…

Q: A 100. mL aqueous solution prepared by dissolving 25.0 g of a non-electrolyte solute had a freezing…

A: Given : Kf = 1.86 °C/m Freezing point of solution (Tf) = -1.26 °C Mass of solute = 25.0 gm…

Q: The freezing point of a solution containing 65 g of a compound in 100 g of benzene is 3.80C. What…

Q: A student calculates that a .200 m aqueous solution of CH3OH and a .100 m solution of NaCl should…

A: The ratio of actual particles' concentration (due to association or dissociation) to the dissolved…

Q: What is the molality of a solution in which 13.7 g of sodium sulfate, Na2SO4, has been dissolved in…

Q: Find molal concentration of a sugar solution in water that has a freezing point of -2.1C. Kf=1.86C/m…

A: The molality of the species can be expressed as the ratio of the moles of the species to the solvent…

Q: Calculate the freezing point of a 2.6 m aqueous sucrose solution

A: The freezing point of the given sucrose solution can be determined as follows, ΔTf = kf x m ΔTf =…

Q: A 10% solution (by mass) of sucrose in water has freezing point of 269.15 K. Calculate the freezing…

A: Colligative properties explain the physical change observed on the addition of solute to solvent.…

Q: Express the 1% Sodium Lauryl Sulfate (NaC 12 H 25 SO 4; ρ=1.01 g/ml) solution in the following…

Q: 3. A 100. mL aqueous solution prepared by dissolving 25.0 g of a non-electrolyte solute had a…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Calculate the freezing temperature of the following solution of 0.50 M sodium chloride (an ionic…

A: Introduction: Depression in Freezing point: The phenomenon by which…

Q: Calculate the molality of NaCl in a 500 ml 20% aqueous NaCl solution whose density is 1.148 g/mL at…

A: Given data is: Density = 1.148 g/mL Molar mass of NaCl = 58.44 g/mol Calculation of molality,…

Q: The molality of an aqueous solution of sugar (C12H22O11) is 2.58 m. Calculate the mole fractions of…

A: 2.58 m - 2.58 of sugar present in 1 kg water. Molality = moles of soluteweight of solvent in kg 2.58…

Q: Determine the molality of a solution prepared by dissolving 0.500 moles Bal2 in 11.5 moles H2O

A: Since we know that molality is calculated as Molality = number of mole of solute / mass of solvent…

Q: A solution consisting of a molecular substance of mass 1.14 g dissolved in 100. g of camphor freezes…

Q: What is the effect on vapor pressure of a solution with particularly strong solute–solvent…

A: Vapor pressure is the pressure of vapors that are in contact with its liquid form. In case of…

Q: Calculate the freezing-point depression and osmotic pressure in torr at 25°C for an aqueous solution…

Q: Calculate the osmotic pressure of a 1 M aqueous solution of a non-dissociated solute at 20 °C.

A: Given that: Concentration(C) = 1M Temperature(T) = 20°C = 20°C + 273 = 293K

Q: Calculate the molality of a 20.0% (by mass) aqueous solution of hydrochloric acid. A. 2.26 m B. 250…

Q: After the addition of 24 g of ethanol (CH;OH) to 1 kg of water, the freezing point of the solution…

A: ∆Tf = Kf .m Where ∆Tf = (T° - Ts) Where T° =freezing point of pure water = 273 K Ts =freezing…

Q: A 1.25 M fructose (C6H12O6) solution has a density of 1.69 g/mL. What is the molality of this…

A: Given, Molarity of fructose solution = 1.25 M Density of the solution = 1.69 g/mL Note: Molar mass…

Q: Calculate the molarity of a 5%vinegar solution. Calculate the molality of a 5%vinegar solution.…

A: Given 5% vinegar solution Calculate molarity and mole fraction of vinegar

Q: Calculate the freezing point of 10% MgCl2 solution (MWMgCl2 = 95.3, kf = 1.86 kg C / mol)

A: 1) Molality of solution 10% MgCl2 solution 10 g MgCl2 dissolved in 100 g solution mass of MgCl2…

Q: Explain the existence of colligative properties using the concept of chemical potentials.

A: Colligative properties

Q: Calculate the molalities of the following aqueous solutions: (a) 1.21 M sugar (C12H22011) solution…

A: Molality = no. of moles of solute/Mass of solvent (kg) Now, we have to calculate 'no. of moles of…

Q: Calculate the freezing point of a 1.7 m aqueous ethylene glycol solution.

Q: The normal freezing point of a certain liquid X is 0.60°C, but when 0.14 kg of barium hydroxide…

A: Given : Mass of barium hydroxide, Ba(OH)2 i.e solute = 0.14 Kg = 140 g (since 1 Kg = 1000 g)…

Q: Lithium chloride has a lattice energy of 861 kj/mol, and a solvation energy of -898 kj/mol. When…

A: When the lithium chloride solid is dissolved in water, energy will be required to break the lattice…

Q: Calculate the molality of a 40.0% H3PO4 solution in water. 0.380 m 6.80 m 1.13 m…

A: Given: (w/w) % of H3PO4 solution in water = 40.0 % molar mass of H3PO4 = 97.994 g/mol Let mass of…

Q: Calculate the molality of a sucrose solution made by dissolving 26.8 grams sucrose into 93.6 grams…

A: Molality(m). It is defined as number of moles of solute dissolved in per kilogram of solvent.

Q: Explain the difference between an ideal and a nonideal solution.

A: In an ideal solution, the magnitude of solute-solvent interactions is similar to solvent-solvent and…

Q: The molal elevation constant for water is 0.513 °C kg mol–. When 0.8 mole of sugar is dissolved in…

Q: Calculate the molality of a 25.8% (by mass) aqueous solution of phosphoric acid (H3PO4). A. 348 m…

A: % by mass is defined as the mass percent of the solute present in the solution Hence % by mass =…

Q: Determine the molality of a 6.930 wt % aqueous solution of LiCl

Q: The freezing point of a 0.01 m aqueous solution of a nonvolatile electrolyte is -0.0720C. What is…

A: The freezing point, Tf , of 0.01 m solution is -0.072o C. As the solution is aqueous, that is the…

Concept explainers

UV Visible Spectroscopy

Spectroscopy refers to the absorption or emission of light or other radiations by matter. When a substance or chemical absorbs light or radiation, they reach an excited state followed by de-excitation or emission of the light or radiation forming distinct spectra. UV-visible spectroscopy or ultraviolet-visible refers to the absorption and emission in the ultraviolet and visible regions of the electromagnetic spectrum.

Question

How can I solve this question? I need full details and accurate answer.

Calculate the freezing point of a 10.50 m aqueous solution of sucrose. Freezing point constants can be found in the list of
colligative constants.
T =
°C

Coligative Constants
amacmillan
learning
Chempendix
Constants for freezing-point depression and boiling-point elevation calculations at 1 atm:
K{ value* Normal freezing K, value Normal boiling
(°C/ m)
Solvent
Formula
(°C/ m)
point ( °C)
point (°C)
H20
C 6H6
Physical Constants
1.86
0.00
0.512
100.00
water
benzene
5.12
5.49
2.53
80.1
Acids and Bases
сyclohexane C sН 12
C2H60
20.8
6.59
2.92
80.7
Activity Coefficients
ethanol
1.99
|-117.3
1.22
78.4
carbon
CCI 4
29.8
-22.9
5.03
76.8
tetrachloride
Activity Series
camphor
C 10 H 16 O 37.8
176
Amino Acids
Roiling Dointc

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A 1.00 mol/kg aqueous sulfuric acid solution, H2SO4,freezes at 4.04 C. Calculate i, the vant Hoff factor,for sulfuric acid in this solution.
The osmotic pressure of a solution containing 7.0 g of insulin per liter is 23 torr at 25 C. What is the molar mass of insulin?
The vapor pressures of several solutions of water-propanol (CH3CH2CH2OH) were determined at various compositions, with the following data collected at 45C: H2O Vapor pressure(torr) 0 74.0 0.15 77.3 0.37 80.2 0.54 81.6 0.69 80.6 0.83 78.2 1.00 71.9 a. Are solutions of water and propanol ideal? Explain. b. Predict the sign of Hsoln for water-propanol solutions. c. Are the interactive forces between propanol and water molecules weaker than, stronger than, or equal to the interactive forces between the pure substances? Explain. d. Which of the solutions in the data would have the lowest normal boiling point?
Which solute has the greatest effect on the boiling pointof 1.00 kg of water: 50.0 g of strontium chloride (SrCl2) or 150.0 g of carbon tetrachloride (CCl4) ? Justify youranswer.
What would be the freezing point of a solution formed by adding 1.0 mole of glucose (a molecular compound) to the following amounts of water? a. 250 g (0.25 kg) b. 500 g (0.500 kg) c. 1000 g (1.000 kg) d. 2000 g (2.000 kg)
The freezing-point depression of a 0.091-m solution of CsCl is 0.320C. The freezing-point depression of a 0.091-m solution of CaCl2 is 0.440C. In which solution does ion association appear to be greater? Explain.
The vapor pressure of an aqueous solution of urea. CH4N2O, is 291.2 mmHg at a measured temperature. The vapor pressure of pure water at that temperature is 355.1 mmHg. Calculate the mole fraction of each component.