Determine the molarity and mole fraction of a 1.03 m solution of acetone (CH3COCH3) dissolved in ethanol (C₂H5OH). (Density of acetone = 0.788 g/cm³; density of ethanol = 0.789 g/cm³.) Assume that the final volume equals the sum of the volumes of acetone and ethanol. mol/L molarity mole fraction

Q: A solution of ethylene glycol and water has a vapor pressure of 7.88 torr at 10°C. Pure water has a…

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Q: A solution contains 10.0 g of carbon tetrachloride, CCl4, and 20.0 g of benzene, C6H6. Calculate the…

A: Given: Mass of carbon tetrachloride =10g Molar mass Carbon tetrachloride = 153.82 g/mol Moles of…

Q: Calculate the mole fraction of nitric acid of a(n) 19.5% (by mass) aqueous solution of nitric acid.

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Q: You have a solution which is 43.9% by mass isopropyl alcohol (MM = 60.11 g/mol) in water. The…

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Q: 1. A solution is prepared by dissolving 12 grams of turmeric powder in 350 grams of water. Calculate…

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Q: mass

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Q: What is the mole fraction of ethanol in a solution made by dissolving 25.0 g of ethanol, C2H5OH, in…

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Q: A solution was made by dissolving 8.01 g sodium chloride (NaCl) in 46.5 g water (H2O). What is the…

A: Given: Mass of sodium chloride (NaCl)=8.01 g Mass of water (H2O)=46.5 g The molar mass of sodium…

Q: A solution is prepared by dissolving 52 g sucrose (C12H22O11) in 565 mL of water. Determine the…

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Q: Density of Mole fraction of Molarity Molality % by Mass ppm solution solute 1.29 30.0

A: Given that:  Density of KOH solution = 1.29g/ml  % by mass of KOH = 30.0  Molar mass of KOH =…

Q: 2) For a solution of 4.60 m CUC12, calculate the molarity of the solute. The density of the solution…

A: Given molality of the solution is 4.60 m, which means 4.60 moles of the solute are present in 1 kg…

Q: What is the Molarity of a solution of NaCl in water, if the mole fraction of NaCl is 0.111? The…

A: Given,mole fraction of NaCl = 0.111density of the solution = 1.19 g/mL

Q: A chemist combined chloroform (CHC13) and acetone (C₂H₂O) to create a solution where the mole…

A: The sum of mole fractions of the components in a binary mixture is equal to 1. Xchloroform +…

Q: A 1.50 kg solution of NaOCl (aq) contains 2.98 mass percent of NaOCl. Calculate the mass of NaOCl in…

A: Given, mass of NaOCl solution = 1.50 Kg = 1.50 × 1000 g = 1500 g Mass percent of NaOCl = 2.98 % Mass…

Q: an aqueous solution is prepared by dissolving 2.50 g of NaBr (M.W. = 102.894 g/mole) in 7.82 mL of…

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Q: The mole fraction of silver nitrate, AgNO3, in an aqueous solution is 1.83×10². %. The percent by…

A: Given that mole fraction of silver nitrate is 1.83×10-2. The mass percent can be obtained by simply…

Q: The vapor pressure of an aqueous solution is found to be 19.4 mmHg at 25 °C. What is the mole…

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Q: Calculate the molarity of a solution made from 50.0 g LiCI in 500 mL of solution. Molar mass =…

A: Given data, Mass of LiCl = 50.0g Volume of solution = 500mL = 0.500L Molar mass of LiCl =…

Q: Calculate the molality, molarity, and mole fraction of FeCl3 in a 28.8 mass % aqueous solution (d =…

A: Given  density of solution : d = 1.280 g/mL mass % of FeCl3 in solution = 28.8 % Take 1.0 L (or 1000…

Q: A 9.97 M solution of NaOH has a density of 1.33 g/cm3 at 20°C.  Assume you have 1.00 L of solution.…

A: 1. First calculate the mole of NaOH. NaOH moles=1.00L×9.97M=9.97mol Next the mass of NaOH, solution…

Q: Calculate the molal concentration, molar concentration, and mole fraction of 6.25% solution of H3PO4…

A: Given,  Mass percentage of H3PO4 = 6.25%  Density of the solution = 1.06 g/mL  Calculate the molal…

Q: You have a solution prepared by dissolving 6.8 g of urea, CO(NH2)2 , in 33.5 g of methanol, CH3OH.…

A: A solution prepared by dissolving 6.8 g of urea, CO(NH2)2 , in 33.5 g of methanol, CH3OH. First…

Q: Calculate the mole fraction of nitric acid (HNO3) of a 17.5% (by mass) aqueous solution of nitric…

A: Given: 17.5 g of nitric acid in 100 g of solution mass of water = 100 - 17.5 = 82.5 g molar mass of…

Q: What is the mole fraction of formaldehyde (CH2O) in solution if 32.2 grams of CH2O is dissolved in…

A: Given : Mass of HCHO = 32.2g Moles of CCl4 = 3.5 moles

Q: 3. XYZ, a non-electrolyte, is miscible (highly soluble) with water and its molar mass is 132 g/mol.…

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Q: The vapor above a mixture of pentane and hexane at room temperature contains 35.5% pentane by mass.…

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Q: Determine the molarity and mole fraction of a 1.01 m solution of acetone (CH3COCH3) dissolved in…

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Q: In a 54.0-g aqueous solution of methanol, CH4O, the mole fraction of methanol is 0.220. What is the…

A: mole fraction : It is the ratio of moles of a particular component to that of the total moles of…

Q: What is the mole fraction of water in an aqueous solution (density = 1.20 g/mL) that is 2.5 m…

A: Density of aqueous solution = 1.20 g/mL Molality = 2.5m = number of moles/weight of solvent in kg…

Q: Calculate the mole fraction (of each component) of a solution prepared by dissolving 125 mL of pure…

A: It is defined as the number of moles of the solute to the total number of moles. mole fraction= no.…

Q: A solution was made by mixing sodium chloride ( NaCl) and water ( H2O). Given that the mole fraction…

A: Given a solution, mixture of sodium chloride and water.mole fraction of sodium chloride =0.0541 and…

Q: The concentrated sulfuric acid we use in the laboratory is 98.0 percent H2SO4 by mass. Calculate the…

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Q: Calculate the molal concentration, molar concentration, and mole fraction of 6.25% solution of H3PO4…

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Q: What is the osmotic pressure, in torr, of a solution formed by dissolving 0.3323 g of ammonium…

A: First Calculate molarity=mole/volume Then use  π=CRT

Q: An aqueous solution is 22.0 % by mass silver nitrate, AGNO3, and has a density of 1.22 g/mL. The…

A: The relative quantities of substances present in a mixture is determined using mole fraction, 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.