Question

The following information is known about commercial ammonia solutions: Formula Weight=17.03 g/mol; Density of solution=0.90 g/mL; Weight %=28.0; Molarity=14.8

a. Calculate the molality of the solution

b. Calculate the mole fraction of ammonia in the solution

Answer #1

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?

A solution consists of 18.0 g of
hydrochloric acid, HCl, and
91.0 g water and has a density of
1.08 g/mL.
(a)Calculate the weight percent of HCl, (b) the
molality of HCl, (C) the mole fraction of
HCl, and (d) the molarity of HCl
in 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

A 25.1 molal concentration of ammonia (NH3) in water has a
density of 0.982 g/ml. What are the mass percent, molarity and mole
concentration of ammonia in this solution.

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.

Toluene (C7H8, molar mass = 92.13 g/mol)
an organic compound often used as a solvent in paints is mixed with
a similar organic compound benzene (C6H6,
molar mass 78.11 g/mol). Calculate the molarity, molality,
mass percent, and mole fraction of toluene in 2.00 x
103 mL of solution that contains 75.8 g of toluene and
95.6 g of benzene. The density of solution is 0.857
g/cm3.

KCl is an ionic salt with a formula
weight of 74.54 g/mole.
A 1.417 M (mole/liter) KCl solution
has a density of 1064.5 grams/liter at 20 OC.
Use the Molarity and the formula
weight to find the mass (g) of salt in one liter.
Then, find the mass (g and kg) of
water in one liter of the solution.
Determine the molality (m), or moles
of salt per kg of water, by dividing the moles of salt in one liter...

A solution is prepared by dissolving 25.00 g of acetic
acid (CH3COOH) in 750.0 g of water. The density of the resulting
solution is 1.105 g/mL.
A) Calculate the mass percent of acetic acid in the
solution.
B) Calculate the molarity of the solution.
C) Calculate the molality of the solution.
D) Calculate the mole fraction of acetic acid in the
solution.
E) What is the concentration of acetic acid in
ppm?

A 10.69% (weight/weight) Fe(NO3)3
(241.86 g/mol) solution has a density of 1.059g solution/mL
solution. Calculate:
a.) The molar concentration of
Fe(NO3)3 in this solution.
b.) The mass in grams of Fe(NO3)3
contained in one liter of this solution.
c.) The molar concentration of NO3- in
the solution.

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?

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