(i)On mixing liquid X and liquid Y, the volume of the resulting solution increases. What type of deviation from Raoult’s law is shown by the resulting solution? What change in temperature would you observe after mixing liquids X and Y?(ii) How can the direction of osmosis be reversed? Write one use of reverseosmosis.

Q: When 14.0 g of a certain molecular compound X are dissolved in 85. g of benzene (CH), the freezing…

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Q: The freezing point of ethanol, CH3CH,OH, is -117.300 °C at 1 atmosphere. KAethanol) = 1.99 °C/m In a…

A: Given: Mass of compound (solute) = 12.60 g Mass of ethanol (solvent) = 265.8 g Freezing point of…

Q: Calculate the freezing point of a .2m CaCl2 aqueous solution, assuming it dissociates completely to…

A: Colligative properties: The colligative properties are those properties of solutions that depend on…

Q: The partial molar volumes of acetone and chloroform in a mixture in which the mole fraction of…

A: Given, The partial molar volume of acetone and trichloromethane in a mixture in which the mole…

Q: In addition to filling in the blanks below, show all of your work for this problem on paper for…

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Q: If 0.300 mol of a nonvolatile nonelectrolyte are dissolved in 3.50 mol of water, what is the vapor…

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Q: Do you expect the freezing-point depression constant, Kf, to change when you change the solute? When…

A: The properties of the solution that depend on the number of moles of solute are termed as…

Q: Calculate the mass of compound (molar mass = 256 g mol-1) to be dissolved in 75 g of benzene to…

A: According to colligative properties, the depression in freezing point is given as - ΔTf = Kf * m…

Q: The freezing point of ethanol, CH3CH,OH, is -117.300 °C at 1 atmosphere. Kgethanol) = 1.99 °C/m In a…

A: Given: The freezing point of pure ethanol is -117.300°C. The freezing point depression constant of…

Q: Describe what a colligative property is and explain the Van’t Hoff factor?

A: A colligative property is described below and explains the Van’t Hoff factor.

Q: What is the mole fraction, X, of solute and the molality, m (or b), for an aqueous solution that is…

A: The mole fraction of a component in the mixture is defined by the ratio of moles of that substance…

Q: What is the difference between a solution and a colloidal suspension? Give examples of each, and…

A: There are various differences between a solution and a colloidal suspension and due to the below…

Q: Given that an aqueous solution of ethylene glycol in water has a vapor pressure lowering of 16.0…

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Q: The concentration of ions in seawater is approximately the same as that in a solution containing 4.2…

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Q: The osmotic pressure of an aqueous solution of a non-ionic solute is 120 kPa at 300 K. Assuming that…

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Q: The mole fraction of iodine, I,, dissolved in dichloromethane, CH,CI,, is 0.115. What is the molal…

A: The mole fraction of a compound in a solution is calculated by dividing the number of moles of a…

Q: Referring to table 13.3, calculate the freezing point of a solution containg 0.600kg of CHCl3 and…

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Q: If the boiling-point elevation of an aqueous solution containing a nonvolatile electrolyte is…

A: Boiling point elevation can be defined as a phenomenon in which the boiling point of liquid will be…

Q: If the freezing point depression of a 0.110 m solution is 2.33 degrees Celsius, what is the freezing…

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Q: When 89.1 mg of a certain molecular compound X are dissolved in 90. g of benzonitrile (C,H,CN), the…

A: The freezing point of a solvent is the temperature at which, solvent converted to solid-state from…

Q: Aqueous ethanol solutions are prepared by mixing measured weights of assayed ethanol and…

A: Given an aqueous solution is 27.2 % ethanol, C2H5OH , by mass  We have to find its molality

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: 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 molality of the solution formed when 1.5g of urea (molar mass = 60g / mol) is…

A: Given, 1.5g of urea (molar mass = 60g / mol) is dissolved in 200g of benzene

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

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Q: How we can distinguishe between the homogeneous and heterogenous and colloidal mixture And can we…

A: Homogeneous mixture: Particles are uniformly distributed. They cannot be differentiate by eyes. It…

Q: What will be the osmotic pressure exerted by an aqueous solution of 500ml volume at 25 degree…

A: Since it is not given whether 2.33 is concentration or mass or moles. Hence I'm assuming it to be…

Q: Calculate the freezing point depression for a solution of 78.5 g toluene (C7H8) in 245 mL phenol (d…

A: Introduction: Freezing point depression: The freezing point depression is one of the colligative…

Q: Why are boiling point elevation and freezing point depression considered colligative properties?

A: Colligative property:  Properties which depends upon the number of solute particle present in the…

Q: Crude oil pumped out of the ground may be accompanied by formation water, a solution that contains…

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

Q: What is the freezing point of an aqueous calcium sulfate solution prepared by mixing 45.0 g of…

A: The freezing point of a solution is always less than that of the pure solvent. The freezing point…

Q: Calculate the mass of compound (molar mass = 256 g mol-1) to be dissolved in 75 g of benzene to…

A: A colligative property is a property that depends on the number of moles of solute, not on the…

Q: if

A:

Q: Calculate the vapor pressure at 25 °C of a solution containing 55.3 g ethylene glycol (HOCH2CH2OH)…

A: The amount of ethylene glycol is 55.3 g The amount of water is 285.2 g The vapor pressure of pure…

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

A: Colligative properties

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: concentration

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Q: The freezing point of ethanol, CH3CH2OH, is -117.300 °C at 1 atmosphere. Kf(ethanol) = 1.99 °C/m In…

A: Given, In a laboratory experiment, students synthesized a new compound and found that when 13.34…

Q: The freezing point of benzene, C,H6. is 5.500 °C at 1 atmosphere. K(benzene) = 5.12 °C/m In a…

A: A numerical problem based on colligative property, which is to be accomplished.

Q: If 528 mg of an unknown sample was dissolved in 10.00 grams of t-butanol (C4H9OH) and the freezing…

A: Solution Freezing point depression refers to the lowering of the temperature of solvents upon the…

Q: A sample of an organic compound (a nonelectrolyte) weighing 1.35 g lowered the freezing point of…

A: The molar mass of the compound is to be calculated

Q: A solution of HCl, 0.77% by weight, freezes at -0.805oC. Calculate the  apparent molality and the…

A: ΔTf = i*Kf*m ΔTf  = depression in freezing point = freezing point of pure solvent - freezing point…

Q: Calculate the osmotic pressure of a solution containing 24.6 g of glycerin (C3H8O3) in 250.0 mL of…

A: Given: Mass of glycerine = 24.6 g Temperature = 298 K Volume of solution = 250 mL

Q: A nonvolatile solute is dissolved in benzene and the resulting solution has a vapor pressure of 20.5…

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Q: When 911. mg of a certain molecular compound X are dissolved in 35.0 g of benzene (CH), the freezing…

A: Given: The given mass of compound X,(Wb)=911 mg=0.911 g. The freezing point of the…

Q: The enthalpy of hydration of Li+1 is -520 kj/mol. Calculate the enthalpy of solution of LiF(s)

A: Given: Enthalpy of hydration of Li+1 = -520 kj/mol Lattice energy of LiF(s) = 1030 kJ/mol

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.