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.)
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?
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
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.
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
Calculate the mole fraction of phosphoric acid (H3PO4) in a 25.4% (by mass) aqueous solution. (Assume 750 mL of solution.) What is the molarity of the solution? What is the molality? (At 20 ° C, the density of phosphoric acid is 1.1462 g/mL and the density of water is 0.99823 g/mL.)
Calculate the molalities of some commercial reagents from the following data: (Assume 100 g of solution.) Data HCl(aq) NH3(aq) Formula weight (g/mol) 36.465 17.03 Density of solution (g/mL) 1.19 0.90 Weight % 30.2 26.4 Molarity 11.3 14.4 Molality of HCl(aq) Molality of NH3(aq)