Question

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

Answer #1

**Molarity = number of moles of solute/per L of
solution**

**=> 2.498 *10^(-4)/0.125 = 1.9984 * 10^(-3)
M**

**Molality = number of moles of solute/per Kg of
solvent**

**Mass of solvent = 810 gm/L * 0.125L = 101.25
gms**

**Mass of ethanol = 789 gm/L * 13.7 * 10^(-6) L =
0.0108093 gms**

**molar mass of ethanol = 46 gm/mol**

**number of moles of ethanol = 0.0108093/46 = 2.498 *
10^(-4) moles**

**molality = 2.498 * 10^(-4)/(101.25/1000) = 0.00232
m**

**Volume Percentage = 13.7 * 10^(-6)/0.125 * 100 = 1.0960
* 10^(-2)%**

**ppm = mg/L = 10.8093/0.125 = 86.4744 ppm**

**ppb = mg/uL = 86474.4 ppb**

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 15 μL of this
alcohol in a 40 wt% solution of Ethanol in water. The final volume
of the solution is 25 mL. Assume that the density of the ethanol
solution does not change upon dissolution of the butanol. Use the
correct number of significant figures!

If an aqueous solution of Pb2+ has a concentration of
125 ppb, and the density of the solution is 0.9997 g/mL, then what
is the Molarity of the solute at 25.0 ºC?

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.

A solution is 40% ethanol (density = 0.789 g/mL) by volume and
60% water (density = 1.00 g/mL). If Tom Titan has 750.0 mL of the
solution, what is the mass of ethanol in solution?

A water solution contains 40.0% ethylene glycol (C2H6O2) by mass
and has a density of 1.05 g/mL.
1.) how many grams of ethylene glycol are there in 1.250 L of
solution?
2.) What is the mass of 1.250 L of this solution (grams)?
3.) What is the concentration of this solution in ppm?
4.) What is the molality of the C2H6O2 solution?

At 25 degrees Celcius, the density of a 30% aqueous solution by
weight of glycerol (C6H8O3) is
1.071 g/mL. What is the concentration of glycerol in this solution
in units of molarity, molality, and mole fraction?

Concentrated aqueous HCl has a molarity of 11.7 mol/L and a
density of 1.20 g/cm3. What is the molality of HCl in
the solution?

An aqueous NaCl solution is made using 113 g of NaCl diluted to
a total solution volume of 1.25 L .
A.) Calculate the molarity of the solution.
B.) Calculate the molality of the solution. (Assume a density of
1.08 g/mL for the solution.)
C.) Calculate the mass percent of the solution. (Assume a
density of 1.08 g/mL for the solution.)

An aqueous solution is 5.50% by mass
ammonia, NH3, and has
a density of 0.975 g/mL.
The molality of ammonia in the solution is _______
m

An aqueous solution is 8.00% ammonium chloride, NH4Cl, by mass.
The density of the solution is 1.023 g/mL. What are the molality,
mole fraction, and molarity of NH4Cl in the solution?

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 8 minutes ago

asked 17 minutes ago

asked 22 minutes ago

asked 36 minutes ago

asked 36 minutes ago

asked 48 minutes ago

asked 59 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago