A 2 m solution formed with BaCl2 and water. If the cryoscopic constant for water is 1.853 K Kg/mol, what would you expect the new freezing point of the solution? Keep in mind that the freezing point of pure water is 273.15 K.  Report your answer to two decimal places.

Q: When 634. mg of a certain molecular compound X are dissolved in 60. g of cyclohexane (C,H,2), the…

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Q: A 45 g sample of urea (MW = 56.7 g mol-1) (non-dissociating, non-volatile solute) is dissolved into…

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Q: The molal freezing point depression constant K = 3.50 °C-kg-mol X, the solution freezes at -8.0 °C.…

A: Consider the given information as follows;

Q: A researcher prepares a new compound and uses freezing point depression measurements to determine…

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Q: Students are investigating a solvent for use in freezing point depression experiments. They measured…

A: Given, Freezing point of solvent (T°) = -12.6°C Freezing point of solution (T) = -18.3°C Mass of…

Q: A researcher prepares a new compound and uses freezing point depression measurements to determine…

A: Given Mass of compound = 1.538 g mass of cyclohexane = 75 g  freezing point of the solution = 2.16°C…

Q: Determine the freezing point of a solution consisting of 0.350 m KCl in water. The freezing point…

A: Cryoscopic constant of water is 1.86oC/molal Van’t Hoff factor (i) is 2 since each KCl give on one…

Q: At a certain temperature the vapor pressure of pure benzene (C,H) is measured to be 0.44 atm.…

A: Given data: Mass of benzene = 137 g Mass of heptane = 131 g  Vapor pressure of pure benzene = 0.44…

Q: The freezing point of a liquid will change when a solute is added. Explain how the addition of salt…

A: The freezing point of the solution is the temperature at which the liquid state of a substance…

Q: Plants that thrive in saltwater must have internal solutions (inside the plant cell) that are…

A: Temperature = T = 25 °C = 298 K  Density at 25 °C = d = 1.025 g/L   Freezing point depression = ∆Tf…

Q: A certain substance X melts at a temperature of 7.4 °C. But if a 350. g sample of X is prepared with…

A: To calculate the molal freezing point depression constant Kƒ of substance X, we first need to…

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A: Henry's Law is used to calculate the molar solubility of a gas in solution. It states that the molar…

Q: 6.50

A: Dear student I have given answer to your question in the image format.

Q: -1 The molal boiling point elevation constant K₁=0.57 °C-kg-mol for a certain substance X. When 34.…

A: To solve this problem we have to calculate the Boiling Point of pure X

Q: When 136. g of urea (CH₂N₂O) are dissolved in 750. g of a certain mystery liquid X, the freezing…

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Q: t a certain temperature the vapor pressure of pure acetyl bromide (CH,COB1) is measured to be 172.…

A: Given- Pressure= 172 mmHg  Weight of acetyl bromide =121 gram  Weight of thiophene= 86.9 g

Q: A researcher prepares a new compound and uses freezing point depression measurements to determine…

A: Given,  Mass of the compound (w) =  1.966 g Mass of cyclohexane (W) = 75.00 g Freezing point of…

Q: Determine the freezing point of a solution that contains 78.8 g of naphthalene (C10Hg, molar mass =…

A: Given:Mass of napthalene (C10H8) = 78.8 gMolar mass of (C10H8) = 128.16 g/molDensity of benzene =…

Q: The solution prepared by dissolving 6.06 g of triphenyl methane [(C6H5)CH] in 1000 g of benzene,…

A: Given : Mass of solute i.e triphenyl methane = 6.06 g Mass of solvent i.e Benzene = 1000 g = 1 Kg…

Q: A. FREEZING POINT DEPRESSION Kf (*C/m) of water 1.86 Freezing Point of Water, 0.00 °C SOLVENT 100.0…

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Q: A student made a solution by mixing 28.20 g of an unknown substance with 500.0 g of benzene (C6H63,…

A: Depression in freezing point (∆Tf) solvent will calculated as:-∆Tf= kf×W2W1×M2Where∆Tf=Depression in…

Q: The normal boiling point of a certain liquid X is 134.60 °C, but when 91.3 g of urea (CH4N₂O) are…

A: Given : data  Tip: apply equation of elevation in Boiling point

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Q: A chemist is given a nonelectrolyte white powder for analysis. 38.7 g of this substance is dissolved…

A: Colligative properties are the properties which depend on the number of atoms or molecules or ions…

Q: At a certain temperature the vapor pressure of pure benzene (CH6) is measured to be 0.24 atm.…

A: Solution is made up of solute and solvent.Solute is present in small amount and solvent is present…

Q: At a certain temperature the vapor pressure of pure thiophene (C4H4S) is measured to be 0.16 atm.…

A: Information about the question

Q: At a certain temperature the vapor pressure of pure acetyl bromide (CH,COB1) is measured to be 363.…

A: we need to calculate partial pressure of acetyl bromide

Q: Please provide detailed solution and give the explanation of the concept..

A: The freezing point of a solution is lower than that of the pure solvent. This is known as freezing…

Q: A solution is made by mixing 100.0 g acetone (CH3COCH3) and 100.0g methanol (CH3OH). part 1. what…

A: Given:Mole fraction is the ratio of the number of moles of a specific gas and the total number of…

Q: Find the freezing point of a water solution obtained by dissolving 6.38 g of NaCl(s) in 159 g of…

A: The freezing point depression of a solution is given by the equation: ΔTF=KF·m·iwhere,KF is the…

Q: Calculate the freezing point of a solution of 5.00 g of diphenyl, C12H10, and 7.50 g of naphthalene,…

A: Depression in freezing point is equal to the product of molality and depression in freezing point…

Q: A 12.7 g substance was dissolved in 2.00 g of solvent. The molar mass of the unknown substance is…

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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: Temperature, °C 3.0 2.0 1.0 0.0 4.0 5.0 8.0 7.0 6.0 0 In an experiment, the freezing point curve of…

A: Freezing point depression : It is defined as the  lowering of the freezing point of a solvent upon…

Q: A certain substance X has a normal freezing point of -2.5 °C and a molal freezing point depression…

A: Given that: Freezing point of pure substance X (Tf°) = -2.5°CKf = 7.95 °C kg mol-1Mass of urea =…

Q: When 59.8 mg of a certain molecular compound X are dissolved in 50. g of cyclohexane (C6H₁2), the…

A: Here the solute is compound X and the solvent is cyclohexane.  We use the below formula to find the…

Q: At a certain temperature the vapor pressure of pure benzene (CH) is measured to be 0.19 atm. Suppose…

A: • For the calculation of the partial pressure of benzene vapour for the given solution of benzene…

Q: The freezing point of 57.08 g of a pure solvent is measured to be 50.83 ºC. When 2.86 g of an…

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Q: The molal boiling point elevation constant K, =0.88 °C·kg•mol for a certain substance X. When 67. g…

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Q: Given the following mixture of two compounds 65.00 mL of X (MW =75.00 g/mol)(density 1.292 g/mL) and…

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Q: 1. A 0.194 g sample of a nonvolatile solute dissolves in 9.82 g of cyclohexane. The change in…

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Q: The normal boiling point of a certain liquid X is 124.9 °C, but when 31. g of urea (NH),CO)- are…

A: Given :- Normal boiling point of X = 124.9°C  Mass of urea = 31. g  Mass of X = 350. g  Boiling…

Q: What would be the theoretical freezing point of a solution made by dissolving 10.43 g of NiCl 2 in…

A: Given,  the theoretical freezing point of a solution is:  by dissolving 10.43 g of NiCl 2 in 365.0 g…

Q: At a certain temperature the vapor pressure of pure acetyl bromide (CH,COBR) is measured to be 218.…

A: Given data :  1. Mass of acetyl bromide = 110 g  2. Mass of benzene = 120 g  3. Vapor pressure of…