Question

Calculate the molarity, molality, and mole fraction of a solution created by mixing 500.0 mL of ethanol (C2H6O / d = 0.789 g/mL) with 4.267 g of benzene (C6H6 / d = 0.876 g/mL). Assume the density of the solution is the same as ethanol.

Answer #1

Calculate the molality, molarity, and mole fraction of FeCl3 in
a 23.0 mass % aqueous solution (d = 1.230 g/mL). molality=____m
molarity=____M mole fraction=___

Calculate the molality, molarity, and mole fraction of FeCl3 in
a 29.5 mass % aqueous solution (d = 1.280g/mL)

1. The mole fraction of an aqueous solution of lithium sulfate
is 0.297. Calculate the molarity (in mol/L) of the lithium sulfate
solution, if the density of the solution is 1.39 g mL-1.
2. Determine the mole fraction of potassium permanganate in a
6.65 M aqueous solution of potassium permanganate. The density of
the solution is 1.39 g mL-1.

A solution is prepared by mixing 25 mL pentane (C5H12, d = 0.63
g/cm3) with 30 mL hexane (C6H14, d = 0.66 g/cm3). Assuming that the
volumes add on mixing, calculate the mass percent, mole fraction,
molality, and molarity of the pentane.

A sodium hydroxide solution is made by mixing 13.64 g NaOH with
100 g of water. The resulting solution has a density of 1.131
g/mL.
a. What is the molarity of this solution?
b. What is the molality of the solution?
c. What is the mass fraction of NaOH in the solution?
d. What is the mole fraction of NaOH in the solution?

If 0.125 L of aqueous solution with a density of 0.810 g/mL
contains 13.7 µl of ethanol, epress the concentration of ethanol in
ppm, ppb, molarity, molality, and vol%. Pure ethanol has a density
of 0.789 g/mL

Calculate the mole fraction of solute in the following aqueous
solutions (a) 0.112 M C6H12O6
(glucose solution, p = 1.006 g/mL; (b) 3.20% ethanol
(CH3CH2OH) by volume (p = 0.993 g/mL; pure
ethanol, p = 0.789 g/mL)

the mole fraction of sucrose in an aqueous solution is 0.100.
Calculate the molality of sucrose in the solution. the molar mass
of sucrose is 342.3 g/mol

1. Calculate Molarity and molality of 50% solution, by volume,
of ethanol (d=.789g/mL) in water (d=1.00g/mL).
2.
A. What volume of 6M nickel (II) chloride is needed to make 5.0L
of .3m solution?
B. What mass of solid nickel (II) chloride is needed to make the
same 5.0L of a 3m solution?

Calculate the molarity and the molality of
C3H8O2 for a solution of 20.0 g of
C3H8O2 (molar mass 76.09 g/mol) in
80.0 g of water (molar mass 18.02 g/mol). The density of the
solution is 1.016 g/mL.

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