SHOW COMPLETE SOLUTION AND WRITE LEGIBLY When a certain liquid (with M = 46.1 g mol-1 ) freezes at 1 bar and at -3.65 °C its mass density changes from 0.789 g cm-3 to 0.801 g cm-3 . Its enthalpy of fusion is 8.68 kJ mol-1 . Estimate the freezing point of the liquid at 100 MPa

Q: Cyclohexanol (C6H12O) has a cryoscopic constant of 42.2 K kg mol−1, an Ebullioscopic constant of 3.5…

A: Cyclohexanol (C6H12O) has a cryoscopic constant of 42.2 K kg mol−1, an Ebullioscopic constant of 3.5…

Q: (b) Surface sanitizers were prepared using ethyl alcohol/water and isopropyl alcohol/water…

A: According to Raoult's law, we have the following relation regarding vapour pressure : P=xP0 .. (1)…

Q: What mass of non volatile solute sucrose needs to be dissolved in 100g of water in order to decrease…

A: The expression of Raoult's law is shown below: ∆P01P01 =W2 M1M2 W1 where; ∆P01 = change in vapor…

Q: The Henry's law constant for CO2(g)CO2⁢(g) in water at 25 ∘C25⁢ ∘C is 29.4 bar·M−129.4⁢ bar·M−1.…

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Q: Aniline, C6H5NH2, and hexane, C6H14 , form partially miscible liquid - liquid mixtures at…

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Q: Vapour-liquid equilibrium of a two-component ideal solution of trichloroethene (C₂HC13) and…

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Q: Naphthalene, C10H8 , melts at 80.2 °C. If the vapor pressure of the liquid is 1.3 kPa at 85.8 °C and…

A: Given that  Naphthalene has melting point =80.2oC. Vapour pressure of the liquid is 1.3 kpa at…

Q: The addition of 10.00 g of a compound to 250 g of naphthalene lowered the freezing point of the…

A: Given: Mass of the compound=10.00g Mass of naphthalene=250g lowered freezing point=1.560K Kf=7.026 K…

Q: At 25°C, the specific mass of a 50% weightsolution of ethanol in water is 0.914 g cm-3. The partial…

A: Given data:  Temperature = 250C The mass density of ethanol-water solution = 0.914 g cm-3 Partial…

Q: At 39.9 ◦C, a mixture of ethanol (x1 = 0.9060, p1 = 130.4 Torr) and isooctane ( p2 = 43.9 Torr)…

A: In this question, we delve into the world of solution chemistry and the application of Raoult's law…

Q: The osmotic pressu re of an aqueous solution of urea at 300 K is 150 kPa. Calculate the freezing…

A: Given, Osmotic pressure = 150kPa

Q: The Henry's law constant for CO2(g)CO2(g) in water at 25 ∘C25 ∘C is 29.4 bar·M−129.4 bar·M−1.…

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Q: There is a 15.85% by mass aqueous KCl (molecular weight 74.5513 g mol–1) solution at 25 °C. The…

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Q: 3. The partial molar volumes of propanone (acetone) and trichloromethane (chloroform) in a mixture…

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

Q: Aniline, C6H5NH2, and hexane, C6H14 , form partially miscible liquid - liquid mixtures at…

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Q: The partial molar volumes of water and ethanol in a solution with H₂O = 0.45 at 25 °C are 17.0 and…

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Q: Aniline, C6H5NH2, and hexane, C6H14, form partially miscible liquid–liquid mixtures at temperatures…

A: i)

Q: An ideal-dilute solution of chloroform and ethanol with a mole fraction of ethanol in the liquid…

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Q: Calculate the solubility of 1,4-dibromobenzene in benzene at 25.000C and at 45.000 assuming that…

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Q: Camphor (C10H16O) melts at 179.8 °C, and it has aparticularly large freezing-point-depression…

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Q: The Henry's law constant for CO2(g)CO2⁢(g) in water at 25 ∘C25⁢ ∘C is 29.4 bar·M−129.4⁢ bar·M−1.…

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Q: The osmotic pressure of an aqueous solution at 288 K is 99.0 kPa. Estimate the freezing point of the…

A: Given data : Temperature(T) = 288 K Osmotic Pressure(π) = 99 kPa = 0.977 atm For concentration of…

Q: The osmotic pressure of an aqueous solution at 300K is 250.0 kPa.  (1)Calculate the molarity of…

A: Assumed molarity and molality is same for solution. osmotic pressure= π=CRT ∆Tf=Kfm ∆Tf= Tf°-Tf Tf=…

Q: the ideal solubility

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Q: A solvent (molar mass = 98.2 g mol-¹) has a vapour pressure of 4930 Pa at 20 °C; at 50 °C this…

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A: The expressions for osmotic pressure of a solution are:

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.