What is the osmotic pressure in torr of a 0.0173 M glucose solution at body temperature (37 °C)? What are the boiling and freezing points for the same solution? The osmotic pressure = i torr Tf= i °C °C Tbp= [For this part, write your answer to the nearest ten-thousandth, rather than using significant figures rules.]

Q: This question is part one of three. When answering this problem, report the answer with the…

A: Colligative properties are dependent on the number of moles of solute in the solution. There are…

Q: The boiling point of pure ethanol (C₂H₅OH, MM = 46.07 g/mol) is 78.4 °C. A solution is made using…

A: Given,  Boiling point of pure ethanol = T0b = 78.4 °C  Mass of solvent, ethanol = 100.0 g  Mass of…

Q: A certain liquid X has a normal freezing point of 6.90°C and a freezing point depression constant…

A: The freezing point of a solution made of 92.g of glycine (C2H5NO2) dissolved in 700. g of X is 2.93…

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A: Given : Mass of solute i.e benzamide, C7H7NO = 80.7 g Mass of solvent i.e X = 900 g = 0.900 Kg…

Q: A certain liquid X has a normal freezing point of 1.90 °C and a freezing point depression constant…

A:

Q: A student placed 17.5 g of glucose (C6H12O6) in a volumetric flask, added enough water to dissolve…

A: Mass of Glucose = 17.5 g The volume of water = 100. mL Moles of Glucose = Mass/ Molar mass…

Q: In the lab, Stock bottles of concentrated solutions can be diluted to make solutions for use with a…

A: Given: Molarity of initial solution = 12 M Molarity of final solution = 3 M Volume of final solution…

Q: A certain liquid X has a normal freezing point of −7.30°C and a freezing point depression constant…

A: δTf = i x Kf x m----(1) where  δTf = To - Ts  To = freezing point of pure solvent =  −7.30°C Ts…

Q: A student dissolves 20. g of glucose (C,H,,0,) in 100. mL of a solvent with a density of 0.96 g/mL.…

A:

Q: A certain liquid X has a normal boiling point of 129.30°C and a boiling point elevation constant…

A: We are here given, normal boiling point of liquid X=129.3°C boiling point of solution (solution of X…

Q: The density of an aqueous solution containing 15.0 percent ethanol (C2H5OH) by mass is 0.974 g/mL.…

A:

Q: Consider a solution prepared by combining 0.398 moles of K4Fe(CN)6 with 195. g water. What is the…

A: Freezing point depression is a colligative property. It depends on the concentration of solute…

Q: Calculate the amount of water that must be added to each of the following substances to produce the…

A: The question is based on the concept of solutions. A solution is made by adding solute and solvent.…

Q: Part A Determine the required concentration (in percent by mass) for an aqueous ethylene glycol…

A:

Q: The boiling point of pure ethanol (C₂H5OH, MM = 46.07 g/mol) is 78.4 °C. A solution is made using…

A:

Q: At 60 degrees Celsius, a 225-g sample of KNO3 is entirely dissolved in 250 g of water. The…

A: The maximum amount of solute that can be dissolved in a particular amount of solvent is known as…

Q: The boiling point of pure ethanol (C₂H₅OH, MM = 46.07 g/mol) is 78.4 °C. A solution is made using…

A: To calculate the elevated boiling point of glucose and ethanol solution.

Q: An aqueous solution of nickel(II) fluoride, NiF2 , contains 3.42 grams of nickel(II) fluoride and…

A: Given,  Mass of NiF2 = 3.42 g  Mass of water = 17.2 g  What is the weight/weight percent of NiF2 in…

Q: What is the osmotic pressure in torr of a 0.0178 M glucose solution at body temperature (37 °C)?…

A: Given:  Concentration of glucose solution = 0.0178 M  Temperature = 37 °C = 310 K

Q: Calculate the mass of solute required to make a sodium chloride solution containing 1.70 x 102 g of…

A: Mass of Water (Solvent) = W1 = = 170 g = 0.170 kg Melting point = Freezing point of Solution = T =…

Q: Convert the experimental glucose concentration (provided in the table below) from mM (millimolar) to…

A:

Q: An aqueous solution that contains 425 ppm of potassium nitrate (KNO3) is being used in the lab.…

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Q: Ethylene glycol CH2(OH)CH2(OH) is a common automobile antifreeze. Calculate the freezing point and…

A: Given that: Mass of ethylene glycol = 343 g Mass of water = 1055 g = 1.055 kg Kb of water = 0.52…

Q: percent by volume

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Q: A certain liquid X has a normal freezing point of 7.10°C and a freezing point depression constant…

A:

Q: At a certain temperature, an aqueous solution is 34.5% Kl by mass and has a density of 1.311 g/cm³.…

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Q: The boiling point of pure ethanol (C₂H₅OH, MM = 46.07 g/mol) is 78.4 °C. A solution is made using…

A:

Q: 1 The solubility of phthalic acid in water varies greatly with temperature. At 14°C, the solubility…

A: We have find out the answer.

Q: A solution is prepared by mixing 10.0 g of hydrochloric acid (HCl; molar mass = 36.5 g/mol) and 90.0…

A: (1) Given data : Mass of hydrochloric acid = 10 gms Volume of water = 90 mL    Density of water = 1…

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A: Saturated solution is the solution in which no more solute can be dissolved at the same temperature.…

Q: A certain liquid X has a normal freezing point of 3.30°C and a freezing point depression constant…

A: We know that, depression in freezing point is given by,                                       ΔTf =…

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Q: Potassium perchlorate (KCIO4) has a lattice energy of -599 kJ/mol and a heat of hydration of -548…

A: Answer: When a salt is dissolved in water energy is absorbed during the break down of salt into its…

Q: Identify three colligative properties of solutions. Then, describe why the colligative prop- erties…

A: Colligative properties are those properties of solutions that depend on the number of solute…

Q: solution is prepared by mixing 7.05 grams of benzene (C6H6) in water to create a solution total…

A: Mass of benzene = 7.05 g Volume of solution = 100 mL = 0.1 L Molar mass of benzene= 78.11 g/mol

Q: Calculate the freezing point and boiling point of a solution containing 8.10 g of ethylene glycol…

A: Freezing point of pure ethanol = -114.6 °C Boiling point of pure ethanol = 78.4 °C Kf of ethanol = -…

Q: How many liters of a 3.85 M K2SO4 solution are needed to provide 95.4 g of K2SO4(molar mass 174.01…

A: The molarity of the solution is given as 3.85 M K2SO4 and it is required to calculate the volume. To…

Q: What is the molality, m, of the solution?

A:

Q: The solubility in water of ionic compound X is measured and found to be 0.529 would contain 34.0 g…

A: Given: Solubility of ionic compound X = 0.529 g/mL at 5 oC.And mass of X in solution = 34.0 g

Q: Calculate the molarity of a solution made by dissolving 0.382 mol glucose in enough water to make…

A: Given, moles of glucose = 0.382 moles Volume of Solution = 1.32 L  Molarity = ?

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A: Given :

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Q: An aqueous solution weighing 100.0 g contains 41.9 grams of sodium chloride. What is the mass…

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Q: What volume of ethylene glycol (C2H5 O2), a nonelectolyte, must be added to 18.0L water to produce…

A: Given that:        Volume of solvent (H2O) = 18.0 L         density of ethylene Glycol = 1.11g/cm3…

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A: We will first calculate the number of moles of solute, then volume of solution. Finally find…

Q: A carbohydrate contains 40.91% C, 4.58% H, and 54.51% O by mass. A solution of 11.2 g of this…

A: Given:Boiling point of ethanol solution = 78.50oC.Boiling point of ethanol = 78.29oC. The…

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.