Find "gamma"+/- for CuSO4 in an aqueous solution at 25oC that has CuSO4 molality of 0.040 mol/kg and MgCl2 molality of 0.080 mol/kg. Use Davies equation
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Find "gamma"+/- for CuSO4 in an aqueous solution at 25oC that has CuSO4 molality of 0.040 mol/kg and MgCl2 molality of 0.080 mol/kg.
Use Davies equation
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- At a certain temperature, the solubility of zinc(I) chromate is (7.6x10^-5) M. What is the Ksp? Report your answer to 2 sig figs. Note: Your answer is assumed to be reduced to the highest power possibleA 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 osmotic pressure in atm to three 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 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)If you know that sodium bicarbonate has a solubility of 8.4 g in 100g water at 18 °CI. Calculate (a) the molarity and (b) the molality of 8.4 g of Sodium bicarbonate in water II. if you had 200 mls of water, what is the minimum amount of Sodium bicarbonate that you will require to achieve supersaturation? III. If 150 mls of a stock solution of sodium bicarbonate having a concentration of 0.5 M was diluted to 300 mls. What will be the final concentration of the diluted 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 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.In 1.00 atm of pure oxygen, the solubility of O2 (g) in water is 1.26*10-3 M at 25.0oC. The mole fraction of oxygen in air is 0.210. If the atmospheric pressure is 0.979 atm, what is the solubility of oxygen in air at 25oC? Answer is suppose to be 2.59*10-4 M, please show step by step.
- The Henry's law constant for CO2 (g) in water at 25 C is 29.4 bar M-1. Estimate the concentration of dissolved CO2 (g) in a carbonated soft drink pressurized with 1.80 bar of CO2 (g).In a lab test, a student in CHEM 2102 was provided with a solution of compound B (0.16 mol of B was dissolved in 100.0 mL of solvent A, the density of solvent A was 1.20 g/mL). He observed that the boiling point of the solution is 201.0 C. The students search for the molal boiling point elevation constant of the compound B and he found it to be 0.15 C. Kg/mol. Interestingly, while he was searching he found the heat of vaporization of the solvent A is 5.5 KJ/mol. Can the student use the given information to find SSurr for boiling process of solvent A. If yes, calculate the numerical value. Explain your answer.Compute for the molality of her disinfectant if she dissolved 5Tbsp of NaClO in 3.8 Liters of H20
