The Henry’s law constant for helium gas in water at 30 °C is 3.7 * 10-4 M>atm and the constant for N2 at 30 °C is 6.0 * 10-4 M>atm. If the two gases are each present at 1.5 atm pressure, calculate the solubility of each gas

Q: The freezing point of water H,0 is 0.00°C at 1 atmosphere. A nonvolatile, nonelectrolyte that…

A: Introduction: The lowering of freezing temperature when a non-volatile solute is added to the…

Q: Water has a molal freezing point constant of 1.86°C kg/mol.  Calculate the freezing point of 38.734…

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Q: What is the molality of a solution consisting of 2.66 mL of carbon tetrachloride (CCl4; d = 1.59…

A: The given data contains, Volume of CCl4 = 2.66 ml. density = 1.59 g/ml. Volume of CH2Cl2 = 76.5 ml.…

Q: The freezing point of pure benzene (C₆H₆) is 5.49 °C. The freezing point of a solution made using…

A: Pure benzene (solvent) freezing point = Tp = 5.49 °C Freezing point of Solution = Ts = -13.0 °C Kf…

Q: What volume of ethanol (density = 0.7893 g/mL) should be added to 650.0 mL of water (density = 1.00…

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Q: A solution is made by dissolving 4.35 g of glucose (C6H12O6) in 25.0 mL of water at 25 °C. Calculate…

A: Given that mass of glucose is 4.35 g in 25.0 m L of water. Density of water is given as 1.00 g/m L.

Q: The freezing point of pure benzene is 5.49 °C. The freezing point of a solution made using toluene…

A: freezing point is defined as a temperature at which liquid is converted into solid.

Q: Lithium chloride (LiCl) has a lattice energy of -834.0 kJ/mol and a heat of hydration of –871.0…

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Q: The solubility of CaCl2 at 10 C is 64 g in 100 g water. Which of the following concentrations would…

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Q: A solution that contains 16.6 g of a covalent compound dissolved in 500. g of benzene freezes at…

A: Given,           Weight of the covalent compound (W2) = 16.6 g           Weight of the solvent…

Q: dissolving 4.555 g of ZnSO 4 in 150.0 g of water? The freezing point constant of water is 1.86…

A: We have to calculate the decrease in freezing point of the guven solution

Q: A solution was prepared by dissolving solute T in 115 g benzene. The freezing point of this solution…

A: Depression in freezing point is given by the expression:ΔT = Kf x m…

Q: A solution contains 22.4 g glucose (C6H12O6) dissolved in 0.500 L of water. What is the molality of…

A: Molality is the number of moles of solute dissolved in per kg of solvent. It is denoted by m. Its SI…

Q: 10 grams of a non volatile and non dissociating solute is dissolved in 200 g of Benzene the…

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Q: What would be the theoretical freezing point of a solution made by dissolving 7.511 g of CoSO 4 in…

A: Please find the answer attached.

Q: At a particular temperature the solubility of O2 in water is 0.590 g/L at an oxygen pressure of…

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Q: Determine the vapor pressure of a solution at 25°C that contains 210.3 g of glucose (C6H1206, molar…

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Q: What would be the theoretical freezing point of a solution made by dissolving 5.551 g of CrSO 4 in…

A: Depression of freezing point is a colligative property which depends upon the concentration of…

Q: An old sample of concentrated sulfuric acid to be used in the laboratory is approximately 97.4…

A: Given: Percent of H2SO4 = 97.4 %  Density of solution = 1.83 g/mL

Q: An automobile antifreeze consists of ethylene glycol C2H6O2 a nonvolatile nonelectrolyte . Calculate…

A: The colligative property is determined by the number of moles of solute, not by the solute's nature.…

Q: Maple syrup contains 41.0% sugar, C 12H 22O 11 (MW=342g/mol), and has a density of 2.78 g/mL. At…

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Q: Which solution will have the lowest freezing point? Which solution will have the lowest boiling…

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Q: Calculate the mass of ethylene glycol (formula mass = 62.1 g/mol, an antifreeze component, that must…

A: The properties associated with the solution that is altered by the addition of the non-volatile…

Q: Calculate the molarity and molality of an NH3 solution made up of 25.0 g of NH3 in 55.0 g of water.…

A: Answers are explained below. Calculation for the molarity of the solution is as follows:

Q: A solution is prepared (data below). Calculation the molality (mol/Kg) of the solution. Solvent:…

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Q: 1 A certain liquid X has a normal freezing point of –1.00 °C and a freezing point depression…

A: Given:  Normal freezing point of X=-1.00oC Freezing point depression constantKf=2.88oCKgmol-1 Mass…

Q: A glucose solution contains 55.8 g of glucose (MW = 180.1 u) in 455 g of H2O(l). What are the…

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Q: Calculate the solubility of N, in water when the partial pressure of nitrogen above water is 1.15…

A: Given  partial presure = 1.15 atm Henry law 's constant  = 1.04 ×10-3 mole/L-atm Calculation  of…

Q: A 3.34 g sample of an unknown organic molecule is dissolved in 15.0 g of water solvent. The…

A: When solute is added to a pure solvent the freezing point decreases for the solution and the boiling…

Q: Calculate the molality of a solution containing 3.4 moles of MgCl2 in 1206 g of water? 4.10 m 2.82 m…

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Q: calculate the molality of ethylene glycol required to decrease the freezing point of water by 6.2 °C…

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Q: Calculate the molality of a 2.92 M potassium nitrate solution in which methanol, not water, is the…

A: To solve this problem we have to calculate the mass of solvent and number of moles of Solute .

Q: The vapor pressure of chloroform is 173.11 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that…

A: According to Raoult’s Law, the partial pressure (Psolution ) of a particular solvent above the…

Q: A 0.608 g sample of a protein was dissolved in 25.00 mL of water and the resulting osmotic pressure…

A: Ans : Mass of protien sample, (w) = 0.608g Volume of solution, (v) = 25.00ml = 0.025l Temperature,…

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 freezing point of an aqueous solution of MgBr2 was found to   be   -3.0 °C. Calculate the…

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Q: Water has a molal freezing point constant of 1.86°C kg/mol.  Calculate the freezing point of 37.378…

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Q: At 298 K, the Henry's law constant for oxygen is 0.00130 M/atm. Air is 21.0% oxygen. At 298 K, what…

A: Henry’s law states that the amount of dissolved gas in the liquid is directly proportional to its…

Q: The density of 3M solution of sodium chloride is 1.252 g mL. The molality of the solution will be…

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Q: The Henry’s law constant for helium gas in water at 30 °Cis 3.7 x 10-4 M/atm and the constant for N2…

A: The solubility of any gas is given by  S = KH X P where S = solubility of gas P = pressure of gas…

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: An ethanol water solution is prepared by dissolving 10.00 mL of ethanol, CH3CH2OH (density = 0.789…

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Q: A solution is prepared by mixing 1.00 g of ethanol (C2H5OH) with 100.0g of water to give a final…

A: Given mass of ethanol = 1 g mass of water = 100 g volume of solution = 101 ml molar mass of water =…

Q: Calculate the freezing point of a solution containing 25.0 g. of ClF3 (MM = 92.45 g/mol) in 450. g.…

A: Mass of ClF3 = 25 g Molar mass of ClF3 = 92.45 g/mol Moles of ClF3 =MassMolar mass=25 g92.45…

Q: 2 The solubility of O₂ in water is 0.590 g/L at an oxygen pressure 15 atm. What is the Henry's law…

A: Solubility of oxygen, S = 0.590 g/L Pressure of oxygen gas, PO2 = 15 atm Henry's law constant, KH =…

Q: 2. The Henry's law constant for helium gas in water at 30°C is 3.7 x 10-4 M/atm and the constant for…

A: Answer is given below

Q: What would be the theoretical freezing point of a solution made by dissolving 5.052 g of CuCl 2 in…

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Q: Assuming complete dissociation of the solute, how many grams of KNO3 must be added to 275 mL of…

A: Given : Freezing point of solution = -14.5 ⁰C  Volume of solvent = 275 ml  Kf = 1.86 ⁰C kg mol-1

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.