A solution of mannitol
(C6H14O6) in
water is 12.00 % mannitol by
mass. Its density is 1.0412 g cm-3 at
20 °C. Compute its molarity, mole fraction, and molality at this
temperature.
Molarity
C6H14O6 = M
Mole fraction
C6H14O6 =
Molality C6H14O6
= m
A solution of mannitol (C6H14O6) in water is 12.00 % mannitol by mass. Its density is...
A solution of fructose (C6H12O6) in water is 18.00 % fructose by mass. Its density is 1.0728 g cm-3 at 20 °C. Compute its molarity, mole fraction, and molality at this temperature.
A solution of iron(III) chloride (FeCl3) in water is 6.000 % iron(III) chloride by mass. Its density is 1.0493 g cm-3 at 20 °C. Compute its molarity, mole fraction, and molality at this temperature. Molarity FeCl3 = M Mole fraction FeCl3 = Molality FeCl3 = m
A solution of copper (II) sulfate (CuSO_4) in water is 11.00% copper (II) sulfate by mass. Its density is 1.1186 g cm^3 at 20 degree c. Compute its molarity, mole fraction, and molality at this temperature. Molarity CuSO_4 = M Mole fraction CuSO_4 = Molality CuSO_4 = m.
An aqueous antifreeze solution is 31.0 % ethylene glycol (C2 H4 O2) by mass. The density of the solution is 1.05 g/cm3. Calculate the molality, molarity and mole fraction of the ethylene glycol Molality mol/kg Molarity mol/L Mole fraction
A student makes a solution for analysis by mixing 5.86 grams of Cu2SO4 into 283.2 grams of water. The density of water at the temperature of the lab at the time the solution was made is 0.9926 g/mL. Calculate the molarity, molality, mole fraction, and mass percent of the copper I sulfate. • The molarity of the solution is: 0.09 * • The molality of the solution is: 0.09 * • The mole fraction of the solution is: 0.001269* •...
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.)
An aqueous NaCl solution contains 1.343x10* ppm NaCl. The density of water is 1.000g/ml. The density of the solution is 1.08 g/mL. The molar mass of NaCl is 58.44g/mol. Keep the correct number of significant figures. a) What is the molality of NaCl? b) What is the molarity of NaCl? c) What is the (mass/volume)% is unit of (kg/L)%? d) What is mass percent? e) What is mole fraction of NaCl?
a.) Salt solution is 12.0% NaCl by mass, with a density of 1.023 g/mL. What are the molarity, molality, and mole fraction of this solution? b.) How many grams of salt would you need to add to 500 mL of this solution to raise its mole % to 5.00?
An aqueous solution of glucose is 17.5% C6H12O6 by mass and has a density of 1.10 g/mL. What is the molarity and molality of the solution? What is the mole fraction of glucose?
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