Properties of
Solutions!
WATER!
Solution: a homogenous mixture (s, l, g)
-solute: the substance that is dissolved
in the solution (lesser amount)
-solvent: the substance that dissolves
the solute ( greater amount)
Liquid Solutions:
• are homogenous mixtures.
• do not disperse light.
• may have color.
• will not settle.
• pass through a filter.
Solubility Factors
Nature of Solute and Solvent:
Polar dissolves polar and ionic.
Non-polar dissolves non-polar.
Temperature:
Liquid & Solid: The higher the temperature, the more
soluble.
Gas: Opposite
Pressure:
Has no effect on liquids & solids.
As the pressure increases, the solubility of gas
increases.
• A solution is saturated when it contains
the maximum amount of solute it is able
to dissolve at a given Temp.
• It’s unsaturated when it has less than
the maximum amount of solute.
• It’s supersaturated when it has more
than the maximum amount of solute.
Crystals may form, unstable, given
Temp.
https://www.youtube.com/watch?
v=xy56zzVAaJc
Solubility Curve
Solubility
Solution A is unsaturated
because it falls below
the line.
B
C
A
D
Temperature
Solutions B and D are
saturated because it
falls on the line.
Solution C is
supersaturated because
it falls above the line.
Use Reference Table F
To figure out which ions are soluble in water!
https://www.youtube.com/watch?v=9aYLonML69w
HTTPS://WWW.YOUTUBE.COM/WA
TCH?V=XDEDXFHCPWO
Molarity
The relationship between the moles of solute
and the volume of solution.
Mol solute
L solution
M=
Ex: What is the molarity of a 10.0 L solution
containing 25 moles of solute?
M=
25 mol
10.O L
=2.5 mol/L
molality
The relationship between moles of solute to
kilograms of solvent.
Mol
solute
m=
kg solvent
Ex: What is the molality of a solution
containing 25 moles of solute and 10 grams of
25 m
solvent?
m=
0.010O Kg
m=250.0
Parts Per Million
The relationship between the mass of
solute and the total mass for very dilute
solutions.
ppm =
grams of solute
grams of solution
(whole)
X 10^6
June 2007.
Part C
Answer all questions in this part.
Directions (64–82): Record your answers in the spaces provided in your answer booklet. Some questions may require the use of the Reference
Tables for Physical Setting/Chemistry.
Base your answers to questions 64 through 66 on the information below.
Scientists who study aquatic ecosystems are often interested in the concentration of
dissolved oxygen in water. Oxygen, O2, has a very low solubility in water, and therefore
its solubility is usually expressed in units of milligrams per 1000. grams of water at
atmosphere. The graph below shows a solubility curve of oxygen in water.
atmosphere. The graph below shows a solubility curve of oxygen in water.
64 A student determines that 8.2 milligrams of oxygen is dissolved in a 1000.-gram sample
of water at 15°C and 1.0 atmosphere. In terms of saturation, what type of solution is
this sample? [1]
65 Explain, in terms of molecular polarity, why oxygen gas has low solubility in water. Your
response must include both oxygen and water. [1]
66 An aqueous solution has 0.0070 gram of oxygen dissolved in 1000. grams of water. In
the space in your answer booklet, calculate the dissolved oxygen concentration of this
solution in parts per million. Your response must include both a correct numerical
setup and the calculated result. [2]
Percent by Mass
The percent of solute present in a
solution.
% Mass=
Mass of part
Mass of whole
X 100
http://www.nysedregents.org/Chemistry/
Archive/20070620exam.pdf
PartC
#66
Base your answers to questions 65 through 68 on the information below.
In a laboratory, a student makes a solution by completely dissolving 80.0
grams of KNO3(s) in 100.0 grams of hot water. The resulting solution has a
temperature of 60.°C.
The room temperature in the laboratory is 22°C.
65 Classify, in terms of saturation, the type of solution made by the student.
[1]
66 Compare the boiling point of the solution at standard pressure to the
boiling point of water at standard pressure. [1]
67 Describe the direction of heat flow between the solution made by the
student and the air in the laboratory. [1]
68 Describe a laboratory procedure that can be used to recover the solid
solute from the aqueous solution
June 2010.
Icy Road
• http://mortonmelters.com/#/for-yourhome/basic/
http://www.nysedregents.org/C
hemistry/112/chemexam112w.pdf
#70-71