Question

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.

Answer #1

Molality of the solution = 25.1 molal

This means 25.1 moles of NH3 are present in 1000 g water.

Molar mass of NH3 = 17 g/mol

Mass of NH3 = 17 * 25.1 = 426.7 g

Total mass of the solution = 1000 + 426.7 = 1426.7 g

Mass percent of ammonia in the solution = 426.7 / 1426.7 * 100

**= 29.91 %**

Density of solution = 0.982 g/ml

Volume of solution = Mass / Density

= 1426.7 / 0.982

= 1452.85 mL

= 1.45 L

Molarity of solution = 25.1 / 1.45

**= 17.3 M**

Mole concentration of ammonia = Moles of ammonia / Volume of solution

25.1 / 1.45

**= 17.3 M**

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

The density of a 1.22 M aqueous sucrose soluton
(C12H22O11) is 1.25 g/mL.
Calculate the molal concentration, mole fraction (sucrose) and the
mass percent (sucrose) of the solution. What volume (mL) of the
solution would contain 100 g of sucrose?

What is the molal and molarity concentration of a 98.0 mass
percent aqueous sulfuric acid solution. The density of the solution
is 1.83 g/mL.

20.0% by mass NH3(aq) has a density of 0.8951 g/mL. What is the
molar concentration of this solution?

A.) A solution of H2SO4(aq) with a molal concentration of 3.58 m
has a density of 1.200 g/mL. What is the molar concentration of
this solution?
B.) What is the mole fraction of solute in a 3.79 m aqueous
solution?
C.) An aqueous sodium acetate, NaC2H3O2, solution is made by
dissolving 0.155 moles of NaC2H3O2 in 0.650 kg of water. Calculate
the molality of the solution.

A solution of H2SO4(aq) with a molal concentration of 6.25 m has
a density of 1.300 g/mL. What is the molar concentration of this
solution?

A solution of H2SO4(aq) with a molal concentration of 6.80 m has
a density of 1.318 g/mL. What is the molar concentration of this
solution?

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

2. A solution of NH3 in water has a concentration of 4.48%. Calculate
the molality of the solution.
3. What is the molality of NaCl in a solution that is 4.000
M NaCl, with a density of 1.55 g mL-1?

5.97M glycerol (C3H8O3, 92.095g/mol) has a density of 1.10g/mL.
What is the molal concentration of glycerol?

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 3 minutes ago

asked 16 minutes ago

asked 26 minutes ago

asked 52 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago