VII.(10).At 25°C the total volume V(cms) of a solution formed from MX salt and1.000 kg of water fits the expression: V = 1001.21 + 34.69( n -0.070)2 Calculate: a) the partial molar volume of the salt b) the partial molar volume of water.in a solution of molality, m (m n = 0.100 mol kg').
Q: 14. 5 kg of liquid seawater with initial temperature 0°C and salinity 3 percent (by mass) is mixed…
A: Specific heat capacity is a characteristic of a particular pure liquid. It is a minimum heat…
Q: 3) Give three examples of miscibility/immiscibility in chemistry and explain how these cases can be…
A: Miscibility and immiscibility in chemistry is popularly applicable for liquids. But it is also…
Q: Estimate the freezing point of 200 cm³ of water sweetened by the addition of 2.5 g of sucrose. Treat…
A: Given : Mass of sucrose i.e C12H22O11 = 2.5 g And volume of water = 200 cm3 = 200 mL…
Q: Meztiza, a beer cocktail, is prepared by mixing rum, beer, and cola. Compute the final…
A: Beer contains 4.50% (v/v) of ethanol. 4.50% of ethanol in 100.0 mL of beer can be given as:…
Q: A student determines the molar mass of acetone, , She found that the equilibrium temperature of a…
A: a. The depression in freezing point has the formula = initial temperature - final…
Q: One mole of a component A and two moles of a component B are mixed at 270C to form an ideal binary…
A: The no. of moles(nA) of A=1. The no. of moles(nB) of B=2. R=8.314 JK-1mol-1. The mole fraction of…
Q: A 5.17 molal aqueous nitric acid solution was prepared. (Density of nitric acid = 1.51 g/mL, density…
A: Molality = Number of moles of solute/Mass of solvent in Kg Concentration (%v/v) = 100 x Volume of…
Q: A water-carbonating plant is available for use in the home and operates by providing carbon dioxide…
A: The Henry’s constant of carbon dioxide at 298 K is 3.01 × 103 kPakg/mol. Value of 1 atm in kPa = 1 ×…
Q: Estimate the mean ionic activity coefficient of CaCl2 in a solution that is 0.010 mol kg−1 CaCl2(aq)…
A: The ionization of CaCl2 is as follows: CaCl2 (aq) →Ca+2 (aq) + 2Cl- (aq) The concentration of Ca+2…
Q: The Henry's law constant for CO2 (g) in water at 25 C is 29.4 bar M-1. Estimate the concentration of…
A: Henry's Law says:Pressure(gas)=(Henry's Law Constant)*(Molarity of the gas) (i.e. P = Kh C) we are…
Q: Consider the following reaction: NH4Cl--->NH3(g)+HCl(g). The vapor pressure after dissasociation of…
A: The given dissociation reaction of ammonium chloride is, The expression of equilibrium constant for…
Q: The excess Gibbs energy of solutions of methylcyclohexane (MCH) and tetrahydrofuran (THF) at 303.15…
A:
Q: solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in…
A: Given : Mass of solute = 40g Density = 1.000g/ml
Q: 1. The vapor pressure of pure benzene is 12.8 kPa and the vapor pressure of benzene with toluene at…
A:
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: Consider an ideal mixture of two liquids, A and B. The image below shows the mole fraction of…
A: Consider an ideal mixture of two liquids, A and B. The image below shows the mole fraction of…
Q: solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in…
A:
Q: Consider a mixture of two liquids A and B (i.e., a solution of A+B). How many degrees of freedom are…
A: Given: Mixture of liquid A and B Solution of solid A and solid B
Q: At 39.7°c, the vapour pressu re c etha nol is 13554 Tirm, and that of iso octame.is 45:9 Torr, An…
A: Given, Vapour pressure of pure ethanol = 135.4 torr Vapour pressure of isoctane = 45.9 Torr Total…
Q: Calculate the boiling point (Tbp) of an aqueous solution that is 2.222molal sucrose(aq)under…
A:
Q: The dissolution of NH4CIO4(s) in water is endothermic, with +33.5 kJ/mol. If you prepare a 1.00 m…
A: The ∆H value is 33.5kJ/mol Initial temperature (T1) is 25°C = (25+273K) = 298K Specific heat…
Q: What would (triangle) Hrxn be for this new situation with 40 ml of both 1.0 M NaOH and 1.0 M HCl,…
A: Number of moles of sodium hydroxide = 0.04 L × 1 M = 0.04 mol Number of moles of hydrochloric acid =…
Q: (h) Consider the binary phase diagram below. i. What is the eutectic composition and temperature? At…
A: 1. A eutectic mixture is a homogeneous mixture which melts at a single melting temperature , which…
Q: Describe the preparation of the following solutions: a) 500 ml of approximately 0.2M NaOH (40g/mol)…
A:
Q: The equilibrium vapour pressure for water at 25 ℃ is 0.0317 bar. If a solution of 45 g sucrose…
A:
Q: The sulfuric acid in a car battery has a density of 1.225 g/cm³ and is 3.75 M. What is the molality,…
A:
Q: The molal solubility m, of the sparingly soluble salt BaF2 in water at 25°C, following from the…
A: When a little soluble ionic compound is added to water, there will be an equilibrium between the…
Q: Alkaloids are chemical compounds containing nitrogen that can be produced by plant cells. In an…
A: The question is related to flow of heat. Thus finding out the total heat required for complete…
Q: A solution of ethanol and n-propanol behaves ideally. Calculate the chemical potential of ethanol in…
A: Given: Mole function of ethanol = 0.40 The boiling point of solution = 78.3°C…
Q: The enthalpy of fusion of solute B is 4,384.28 kJ/mol and its melting point is 870.49oC. Calculate…
A:
Q: relative to the unmixed gases of a) a mixture of 10 mol of A and 10 mol of B; b) a mixture of 10 mol…
A: Given details: The temperature of pure gas A and B = 25°C Pressure…
Q: = The vapor pressure of component A'is 300.3 torr, and that of component B is 70 torr at 35 °C. A…
A:
Q: 3. The experimental values of the partial molar volume of salt B at 298 K are found to fit the…
A:
Q: A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute,…
A: Given : Mass of solute = 40g
Q: A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute,…
A:
Q: A solution is prepared by dissolving iodine, I2, in tetrachloromethane,CCI4 at 25 °c. What are the…
A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…
Q: An aqueous solution of mass of 100 g of aqueous copper II sulfate CuSO4.xH₂O was prepared by…
A:
Q: eaction between H, SO, and LİOH in aqueous solution. Phases are
A: In the balanced chemical reaction number of atoms of each element in product side is equal to number…
Q: Given that p*(H2O)=0.02308 atm and p(H2O)=0.02238 atm in a solution in which 0.122 kg of a…
A: Activity of H2O = 0.97 Activity Coefficient of H2O = 0.98
Q: A and B form an ideal solution. At a total pressure of O.900 bar, yA = 0.450 %3D and XA = 0.650.…
A: 1- First calculate the partial pressure of B : We know that, in vapour phase of B yB = ( PB /…
Q: 9.14 The density of a methanol-water solution that is 12.000 weight percent methanol is 0.97942…
A:
Q: Calculate the OP and FP of an aqueous solution containing 15 grains of ferrous sulfate in 10mL…
A: Colligative properties are the properties of the solution that are influenced by the amount of…
Q: When 50.0 ml of 2.00 M HCL is mixed with 50.0 ml of 2.00 M NaOH at 24.5 C, the solution temperature…
A: Calculation for the above question explained as follows
Q: A solution is prepared at 25oC by mixing 20g of K2SO4 with 150mL of water. The density of water at…
A: "Since there are multiple questions and it is not mentioned that which one has to be solved so I am…
Trending now
This is a popular solution!
Step by step
Solved in 4 steps
- One mole of a component A and twomoles of a component B are mixed at270C to form an ideal binary solution. calculate the Vmix , Gmix Hmix and Smix. Assume that R=8.314 JK1mol-1 ?A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the freezing point of the solution(in C to 2 decimal places)A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the vapor pressure of the solution to 3 decimal places in atm.
- A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the osmotic pressure in atm to three decimal placesA solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the boiling point of the solution(in C to 2 decimal places)A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the following: Boiling point of solution (in °C to two decimal places) Freezing point of solution (in °C to two decimal places) Vapor pressure of the solution (in atm to three decimal places) Osmotic pressure (in atm to three decimal places)
- An excess amount of Ba(NO3)2 was added to 2 liters of water at 25 oC until the solution is saturated. Because Ba(NO3)2 is only slightly soluble in water, the excess Ba(NO3)2 was filtered out to get a solid-free mixture. The proponents of the experiment thought about using the concept of colligative properties, specifically boiling point elevation, to determine Ksp. It was observed in their experiments that the solution boils at 100.15 deg C. Kb of water = 0.51 K-kg/mol. Barium nitrate dissociates using: Solve the ff: a) Amount of Ba(NO3)2 dissolved in grams. MW of Ba(NO3)2 = 261.3 g/molb) Solubility product, Kspc) Vapor pressure of the solution in kPaA solution is prepared by dissolving 40.00 g of MgCl2 (f.w. = 95.211 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 2 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the freezing point of the solution.A solution is prepared by dissolving 40.00 g of MgCl2 (f.w. = 95.211 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 2 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the osmotic pressure in atm.
- The enthalpy of fusion of solute B is 4,384.28 kJ/mol and its melting point is 870.49oC. Calculate its ideal solubility (nB) in 8.53 moles of solvent at 143.49oC.A polymer of large molar mass is dissolved in the organic solvent m-cresol (C7H8O) at 25 °C, and the resulting solution rises to a final height of 13.4 cm above the level of the pure solvent, as solvent molecules pass through a semipermeable membrane into the solution. If the solution contains 5.24 g polymer per liter, calculate the molar mass of the polymer. Take the density of the solution to be 1.03 g cm-3.The following evidence was obtained from an experiment to determine the solubility of calcium chloride at room temperature. A sample of saturated calcium chloride solution was evaporated to dryness, and the mass of solid residue was measured.EvidenceVolume of solution (mL) = 15.0Mass of empty beaker (g) = 90.54Mass of beaker and residue (g) = 101.36The solubility of calcium chloride is g/100 mL