
190 proof ethanol is (assume) 95% by weight ethanol. The other 5% is water. The density...
A solution is prepared by mixing 1.15 g of ethanol (CH3CH2OH) with 100. g of water. Calculate: (a) the percent by mass, (b) mole fraction, (c) molality, and (d) molarity of this solution. Assume that the density of the solution is 1.00 g/mL
Assume you dissolve 41.4 g of camphor (C10H16O) in 449 mL of ethanol, C2H5OH. Calculate the molality, mole fraction, and weight percent of camphor in this solution. (The density of ethanol is 0.785 g/mL.)
If 36.17 g of ethanol, C2H6O, are mixed with 73.81 g of water, what is the molality of the ethanol in the solution? Assume the mixture is at 20 oC. The density of ethanol at 20 oC is 0.7893 g/mL; the density of water at 20 oC is 1.0000 g/mL. (Enter your answer to the hundredth place.)
3. (3 pts) Formaldehyde (H2CO) is sold as a 37.0% by weight solution in water. a. Write out both the mathematical definition of weight percent and the mathematical definition of molality, below. How are they similar? How are they different? b. What is the molality of formaldehyde in this solution? c. If the density of the solution if 1.09 g/mL, what is the molarity of formaldehyde? d. You dilute 10.0 mL of the concentrated formaldehyde solution to 200.0 mL with...
The density of an aq solution containing 10.0 percent ethanol by mass is 0.984g/ml. Calculate the molality if this solution. b.) Calculate its molarity. c.) What volume of the solution would contain 0.125 mole of ethanol?
12. Calculate the vapor pressure of ethanol over 80 proof (40.0% ethanol by volume) at 19°C. The vapor pressure of pure ethanol at this temperature is 40.0 Torr. The density of ethanol is 0.79 g/mL and the density of water is 1.00 g/mL.
An aqueous solution of ethanol is prepared by dissolving 19.00 g of ethanol, C2H5OH, in 100.0 g of water. What is the molality of the ethanol solution? The formula mass of ethanol is 46.07 g/mol, and assume the density of water to be 1.000 g/mL
The density of a 40 wt% solution of ethanol in water is 0.937 g/mL. The density of n-butanol is 0.810 g/mL. What is the concentration of n-butanol in ppm if you dissolve 25.0 μL of this alcohol in a 40 wt% solution of Ethanol in water. The final volume of the solution is 50.0 mL. Assume that the density of the ethanol solution does not change upon dissolution of the butanol. Use the correct number of significant figures! Hint: to...
115 grams of KCl is dissolved in 750 ml of water (assume density = 1.005 g/ml). What are the molality, molarity, mole fraction, mole percent, % mass, ppm by mass? What would be the freezing point and boiling point of that solution assuming the Kf of water is 1.86 oC/m and Kb is 0.512 oC/m (assume that KCl fully dissociates with no pairing of ions)?
Consider 99.5 g sucrose (C12H22011) in 300.0 mL of water. Assume 1.00 g/mL as the density of water and of sucrose. Calculate the following: 7. a. Molarity b. Molality c. Mole fraction d. Mole percent Percent by mass, as well as parts per million (ppm) and parts per billion (ppb) e. f. Percent by volume