Solutions & their Properties

Solutions & their Properties - Gr. 7.pptx

Jul 31, 20220 likes51 views

There are two types of mixtures: heterogeneous and homogeneous. A heterogeneous mixture contains visibly distinct components that can be separated through physical means like filtering. A homogeneous mixture appears uniform throughout and maintains a single phase. Solutions are homogeneous mixtures composed of a solvent dissolving one or more solutes. Factors like temperature, particle size, shaking, and concentration affect a solute's solubility in a solvent. Solubility is measured as the maximum amount of solute that can dissolve in a solvent at a given temperature and pressure.

Mixtures
• Mixture: a combination of two or more
substances that do not combine
chemically, but remain the same
individual substances; can be separated
by physical means.
• Two types:
– Heterogeneous
– Homogeneous

Heterogeneous Mixture
• “Hetero” means “different”
• Consists of visibly different substances or
phases (solid, liquid, gas)
• Can be separated by filtering
• Example:

Homogeneous Mixture
• “Homo” means the same
• has the same uniform appearance and
composition throughout; maintain one phase
(solid, liquid, gas)
• Commonly referred to as solutions
• Example:

Solution
• Solution: a mixture of two or more substances
that is identical throughout (homogeneous)
• can be physically separated
• composed of solutes and solvents
the substance being dissolved
the substance that dissolves the solute
Iced Tea Mix
(solute)
Water
(solvent)
Iced Tea
(solution)
Salt water is
considered a
solution. How can it
be physically
separated?

Solution
• The solvent is the largest part of the solution
and the solute is the smallest part of the
solution
Chemistry-Borders IPC-Solutions-Borders
S O L V E N T
S O L U T E

Types of Solutions
Gaseous solutions – air = Oxygen + Nitrogen
Liquid solutions – drinks = mix + water
Solid solutions – alloys = steel, brass, etc

Concentration
• the amount of solute dissolved in a
solvent at a given temperature
•described as dilute if it has
a low concentration of solute
dissolved
•described as concentrated
if it has a high concentration
of solute dissolved

Concentration
•Unsaturated - has a less than the
maximum concentration of solute
dissolved
•Saturated - has the maximum
concentration of solute dissolved
(can see solid in bottom of
solution)
•Supersaturated -contains more
dissolved solute than normally
possible (usually requires an
increase in temperature followed
by cooling)

Solubility
• the amount of solute that
dissolves in a certain amount of a
solvent at a given temperature
and pressure to produce a
saturated solution

Factors affecting solubility of solids
Temperature
increased temperature causes
solids to dissolve faster
Shaking
Note: Increasing the amount of solute
DOES NOT increase the rate of dissolving
Shaking (agitation) causes
solids to dissolve faster
Smaller particles dissolve
Faster because they have
more surface area
Particle Size

• Miscible liquids can easily dissolve in one
another.
• Immiscible liquids are not soluble in
each other.

Solutions & their Properties - Gr. 7.pptx

Mass Percent
• % by mass = mass solute x 100
mass of solution **
**Mass of solution = solute mass + solvent mass

Exercise
If a solution that has a mass of 800.0
grams contains 20.0 grams of NaCl, what
is the concentration using Percent by
Mass?

If 10.0 grams of NaCl is dissolved in 90.0
grams of water, what is the concentration
using Percent by Mass?
Exercise

A solution is made by adding 2.5 mL of
benzene to 80 mL of toluene. Solve for
the percent by volume of benzene.
Percent by volume

If 5.0 ml of alcohol is dissolved in 50.0 mL
of water, what is the concentration using
Percent by volume of the solute?
Percent by volume

This document summarizes key concepts about solutions and mixtures. It defines heterogeneous and homogeneous mixtures, and notes that solutions are homogeneous mixtures composed of solutes dissolved in solvents. Examples of different types of solutions - gaseous, liquid, and solid - are provided. The document also discusses concentration, saturation, and factors that affect the solubility of solids like temperature, shaking, particle size. It concludes by distinguishing between miscible and immiscible liquids.

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Solutions & their Properties - Gr. 7.pptx

1. Solutions

2. Mixtures • Mixture: a combination of two or more substances that do not combine chemically, but remain the same individual substances; can be separated by physical means. • Two types: – Heterogeneous – Homogeneous

3. Heterogeneous Mixture • “Hetero” means “different” • Consists of visibly different substances or phases (solid, liquid, gas) • Can be separated by filtering • Example:

4. Homogeneous Mixture • “Homo” means the same • has the same uniform appearance and composition throughout; maintain one phase (solid, liquid, gas) • Commonly referred to as solutions • Example:

5. Solution • Solution: a mixture of two or more substances that is identical throughout (homogeneous) • can be physically separated • composed of solutes and solvents the substance being dissolved the substance that dissolves the solute Iced Tea Mix (solute) Water (solvent) Iced Tea (solution) Salt water is considered a solution. How can it be physically separated?

6. Solution • The solvent is the largest part of the solution and the solute is the smallest part of the solution Chemistry-Borders IPC-Solutions-Borders S O L V E N T S O L U T E

7. Types of Solutions Gaseous solutions – air = Oxygen + Nitrogen Liquid solutions – drinks = mix + water Solid solutions – alloys = steel, brass, etc

8. Concentration • the amount of solute dissolved in a solvent at a given temperature •described as dilute if it has a low concentration of solute dissolved •described as concentrated if it has a high concentration of solute dissolved

9. Concentration •Unsaturated - has a less than the maximum concentration of solute dissolved •Saturated - has the maximum concentration of solute dissolved (can see solid in bottom of solution) •Supersaturated -contains more dissolved solute than normally possible (usually requires an increase in temperature followed by cooling)

10. Solubility • the amount of solute that dissolves in a certain amount of a solvent at a given temperature and pressure to produce a saturated solution

11. Factors affecting solubility of solids Temperature increased temperature causes solids to dissolve faster Shaking Note: Increasing the amount of solute DOES NOT increase the rate of dissolving Shaking (agitation) causes solids to dissolve faster Smaller particles dissolve Faster because they have more surface area Particle Size

12. • Miscible liquids can easily dissolve in one another. • Immiscible liquids are not soluble in each other.

13. Solubility Curves

15. Mass Percent • % by mass = mass solute x 100 mass of solution ** **Mass of solution = solute mass + solvent mass

16. Exercise If a solution that has a mass of 800.0 grams contains 20.0 grams of NaCl, what is the concentration using Percent by Mass?

17. If 10.0 grams of NaCl is dissolved in 90.0 grams of water, what is the concentration using Percent by Mass? Exercise

19. A solution is made by adding 2.5 mL of benzene to 80 mL of toluene. Solve for the percent by volume of benzene. Percent by volume

20. If 5.0 ml of alcohol is dissolved in 50.0 mL of water, what is the concentration using Percent by volume of the solute? Percent by volume

21. If 5.0 ml of alcohol is dissolved in 50.0 mL of water, what is the concentration using Percent by volume of the solute? Percent by volume

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Solutions & their Properties - Gr. 7.pptx

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Solutions & their Properties - Gr. 7.pptx