ertain substance X has a normal boiling point of 95.4 °C and a molal boiling point elevation constant K, = 0.82 °C-kg•mol A solution is prepared by dissolving some urea NH,) CÓ) in 250. g of X. This solution boils at 96.1 °C. Calculate the mass of urea that was dissolved. pund your answer to 1 significant digit.
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- The active ingredient in many commercial antifreezes is ethylene glycol (C2H6O2). If you wish to protect your radiator down to –25°F, how many grams of ethylene glycol should you add to each liter of water? First convert the temperature to degrees Celsius, use the Kfvalue of 1.853°C/molal for water, and recall that the density of water is 1.00 g/mL. ` ` Adding a solute to a pure solvent not only causes a decrease in the freezing point of the result- ing solution, it also causes an increase in the boiling point of the resulting solution compared to the pure solvent. Thus, ethylene glycol also protects your radiator from boiling over in hot summer months. Using the antifreeze solution prepared in question 2 above, calculate the boiling point of the solution in degrees Fahrenheit. Use the following equation: ΔTb= (Kb) x (molalitysolution) where Kb= 0.52°C/molal Note: ΔTb = BP solution - BP solvent H2OThe normal boiling point of a certain liquid X is 110.00°C, but when 26.1g of iron(III) nitrate (FeNO33) are dissolved in 450.g of X the solution boils at 110.5°C instead. Use this information to calculate the molal boiling point elevation constant Kb of X.Round your answer to 1 significant digit. =Kb⋅°CkgmolYou have a container of 17.42 M conc. acetic acid (CH3COOH(aq)) with density 1.05 g/mL, find the molality of a 150ml sample of the solution. molality = moles solute/Kg solvent moles solute = (0.150 L)(17.42 mol/L) = 2.613 mol CH3COOH molar mass of CH3COOH = 60.06 g/mol grams of solution = (150mL)(1.05 g/mL) = 157.5 g solution grams of solute = (2.613 mol)(60.06 g/mol) = 156.9 g CH3COOH so the total grams of water in this solution would be: g H2O = g solution - g CH3COOH = 157.5g - 156.9 g = 0.6g H2O 0.6g H2O = 0.0006 Kg H2O so molality = (2.613 mol CH3COOH) /(0.0006 kg H2O) = 4355 molal this seems rather high to me but if its 'concentrated' acetic acid, I know that you can get it to about 98% as glacial acetic acid so perhaps there is 4355 moles of acetic acid per kg of water. Did I do this correctly? I know that typically the solvent is the larger component of a solution but the fact that it gives me CH3COOH(aq) would imply that H2O is the solvent still in this situation, I have…
- Osmosis is the process responsible for carrying nutrients and water from groundwater supplies to the upper parts of trees. The osmotic pressures required for this process can be as high as 18.1 atm . What would the molar concentration of the tree sap have to be to achieve this pressure on a day when the temperature is 35 ∘C ? Express your answer to three significant figures and include the appropriate units.In the determination of molar mass of an unknown substance by ebullioscopic constant, 30 mL of acetone (C3H6O) was placed in a test tube with thermometer and glass tubing and subjected to water bath. Upon boiling, the temperature reads 56 deg C. For the boiling point of unknown-acetone solution, you prepared the solution by mixing 1.60 g of unknown solute in the 30 mL acetone and subjected it again to water bath. The boiling temperature of the solution is 56.68 deg C. The density of acetone = 0.9849 g/mL and the Kb of acetone = 1.67 degC/kgIn the determination of molar mass of an unknown substance by ebullioscopic constant, 30 mL of acetone (C3H6O) was placed in a test tube with thermometer and glass tubing and subjected to water bath. Upon boiling, the temperature reads 56 deg C. For the boiling point of unknown-acetone solution, you prepared the solution by mixing 1.60 g of unknown solute in the 30 mL acetone and subjected it again to water bath. The boiling temperature of the solution is 56.68 deg C. The density of acetone = 0.9849 g/mL and the Kb of acetone = 1.67 degC/kg What is the value for delta Tb or the change in boiling temperature (in degrees Celsius)?
- In the determination of molar mass of an unknown substance by ebullioscopic constant, 30 mL of acetone (C3H6O) was placed in a test tube with thermometer and glass tubing and subjected to water bath. Upon boiling, the temperature reads 56 deg C. For the boiling point of unknown-acetone solution, you prepared the solution by mixing 1.60 g of unknown solute in the 30 mL acetone and subjected it again to water bath. The boiling temperature of the solution is 56.68 deg C. The density of acetone = 0.9849 g/mL and the Kb of acetone = 1.67 degC/kg What is the value for delta Tb or the change in boiling temperature (in degrees Celsius)? Final answer must be rounded off to 2 decimal places, and shall NOT have any unit.In the determination of molar mass of an unknown substance by ebullioscopic constant, 30 mL of acetone (C3H6O) was placed in a test tube with thermometer and glass tubing and subjected to water bath. Upon boiling, the temperature reads 56 deg C. For the boiling point of unknown-acetone solution, you prepared the solution by mixing 1.60 g of unknown solute in the 30 mL acetone and subjected it again to water bath. The boiling temperature of the solution is 56.68 deg C. The density of acetone = 0.9849 g/mL and the Kb of acetone = 1.67 degC/kg - What is the value for delta Tb or the change in boiling temperature (in degrees Celsius)? Final answer must be rounded off to 2 decimal places, and shall NOT have any unit. - How many moles of solute is present in the solution given in the video? Final answer must be rounded off to 2 decimal places, and shall NOT have any units. - What is the molal concentration of the solution? Final answer must be rounded off to 2 decimal places, and shall NOT…An investigation was carried out to determine which of three antibacterial soaps is most effective. Four petri dishes labeled A, B, C, and D were set up. The same amount and type of bacteria was added to each dish. Next, 2 mL of a different brand of soap were added to dishes B, C, and D. Then, 2mL of water was added to dish A, instead of soap. The dishes were incubated at 37o C for 24 hours. At the end of the investigation, the amount of bacteria in each dish was determined. Dish D had the least bacteria. It was concluded that the soap in dish D was the most effective soap to use against bacteria. Which statement best describes the validity of this conclusion?
- a stock solution of sodium chloride solution was prepared ( at 25C) by dissolving 250 mg of sodium chloride ( 58.44 g/mol) in enough water (18.015 g/ mol) to make a total volume of 50 mililiters. density of sodium chloride ( at 25C) = 2.17 g/mL. 1. what is the concentration (w/v%) of the saline solution? 2. what is the molar concentration of the saline solution? 3. what is the normality of the saline solution? 4. what is the mole fraction of the solute? 5.what os the molality of a solution hen 12 g of NH3( 17.031g/mol) is dissolved in 250g water? 6. what is the factor of calcium chlorideOsmotic pressures are often reported in units of atmospheres or mm Hg. The latter impliesthat the height of a column of liquid can be used as a measure of pressure. This is, in fact, thebasis of the torricellian barometer from which the units of “torr” come. The pressure, P, isrelated to the height of the column by:P = ρghwhere ρ is the density of the liquid, g is the acceleration due to gravity and h is the height. Whatwill be the height (in mm) of a column of aqueous solution with a density of 0.9987 g/mL, if theosmotic pressure of the solution at 25 °C is 1.4 mm Hg? The density of mercury at thistemperature is 13.8 g/mLThe boiling point of a solution containing 7.51 g of a nonvolatile hydrocarbon in 102.2 g of acetone is 57.08oC. What is the molecular weight of the hydrocarbon? For acetone, Tb = 55.95oC and Kb = 1.71 oC/m