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Chemistry > Solutions and Solubility > Flashcards

Solutions and Solubility Flashcards

1
Q

What are solutions?

A

Solutions are homogenous mixtures of two or more substances.

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2
Q

What is the composition of a solution?

A

Solute+ Solvent

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3
Q

What is a solute?

A

Solids, liquids or gases dissolved in a solvent in small quantities.

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4
Q

What is a solvent?

A

Solids, liquids or gases present in large quantities in which a solute in dissolved.

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5
Q

______ solvents are present in the most common solutions.

A

Liquid

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6
Q

What is an aqueous solution?

A

Solution with water as solvent.

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7
Q

Why is water an important solvent?

A
  1. Most important solvent to dissolve inorganic solute.
  2. Common pharamceutical solvent.
  3. Important biological solvent.
  4. Makes around 60% of our body.
  5. Largely due to its structure.
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8
Q

Give an example of a solution with a gas as a solvent.

A

Air
Solvent- Nitrogen

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9
Q

Give an example of a solution with solid as a solvent.

A

Alloys
Solvent- Metal

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10
Q

What do the properties of liquid solutions depend on?

A
  1. The type of solute added in the solution.
  2. The amount of solute added in the solution.
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11
Q

What is the difference between clear and colorless solutions?

A

Clear solutions- Only one state of matter can be deciphered from the solutions. Solute particles are not seen.
Colorless solutions- Absence of color.

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12
Q

On what basis are solutions classified into?

A
  1. On the basis on conduction of electricity.
  2. On the basis of particle size.
  3. On the basis of solubility.
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13
Q

What is the difference betwenn electrolytic and non-electrolytic solutions?

A

Electrolytic solution:
* Conduct electricty
* Solutions of solids, bases and salts.
* Used in hospitals for replacement therapy to treat the imbalance of ions.

Non-electrolytic solution:
* Does not conduct electricity.

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14
Q

What are the characteristics of true solutions?

A
  1. Have small particle size.
  2. Homogenous.
  3. Do not settle over time.
  4. Cannot be separated through filtration.
  5. Distinguished from pure substances through chemical analysis.
  6. Do not scatter light.
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15
Q

What are the characteristics of colloids?

A
  1. Particle size of colloids> true solutions (1-1000nm)
  2. Not truly homogenous.
  3. Does not settle over time.
  4. Shows tyndall effect.
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16
Q

What are the characteristics of suspensions?

A
  1. Particle diameter> 1000nm
  2. Heterogenous (not a true solution, neither a precipitate)
  3. Settles over time.
  4. Eg. Blood
17
Q

What is the particle diameter of blood?

A

> 1 micrometer

18
Q

____________ is a way to speed up settling of particles in a suspension.

A

Centrifugation

19
Q

What are the characteristics of unsaturated solutions?

A
  1. Solute concentration is less than equilibrium solubility.
  2. All the solute is dissolved.
  3. As the solute is not in equilibrium with the solution yet, there is room for more solute.
20
Q

What are the characteristics of saturated solutions?

A
  1. The solute concentration is equal to equilibrium solubility.
  2. All the solute that could be dissolved by the solution at that temperature is dissolved.
  3. As the dissolved and undissolved solute are in equilibrium, there is no room for more.
21
Q

What are the characteristics of super-saturated solutions?

A
  1. The solute concentration is way more than equilibrium solubility.
  2. All the solute is not dissolved.
22
Q

What is solubility?

A

Solubility is the ability of the solute to dissolve in the solvent.

23
Q

What are the conditions in our body caused due to undissolved substances?

A
  1. Gout- Accumulation of uric acid crystals in soft tissues, cartilage and tendons
  2. Kindney stones- calcium oxalate of calcium phosphate in the urinary tract, bladder, urethra or kidneys.
24
Q

What is hyperuricemia?

A

High levels of uric acid in the blood.

25
Q

Uric acid is a product of ____________________.

A

Purine degradation

26
Q

What are three solubility trends?

A
  1. Polarity
  2. Temperature
  3. Pressure
27
Q

How is ammonia soluble in water?

A
  • Ammonia is a polar solute and water is a polar solvent.
  • They are soluble because of intermolecular forces.
  • Partial negative charge and partial positive charges of both molecules interact.
28
Q

Why is oil insoluble in water?

A
  • Oil is a non-polar solute and water is a polar solvent.
  • Oil has carbon and hydrogen atoms that do not carry any charge.
  • Water molecules attract themselves but not oil.
29
Q

Why does increase in temperature increase solubility in solutions where the solute is solid or liquid?

A

Dissolution reuires breaking of intermolecular forces amongst the solute particles and amongst the solvent particles which requires energy.
Energy is released in the formation of new intermolecular bonds between solute and solvent molecules.

30
Q

Why does solubility of gases decrease with increase in temperature?

A

Solubility of gases in liquids is in liquid phase. This is similar to the phenomenon of condensation. As condensation is an exothermic process, increase in temperature decreases solubility.

31
Q

Why is pressure insignificant to the solubility ofliquids and solids in liquids?

A

Because the volume of liquids and solids stays constant.

32
Q

Why does solubility of gases increase with increase in pressure?

A

Due to Henry’s Law.
Henry’s Law- Mole fraction of gases dissolved in solution increases with increase in partial pressure of the gas over the solution.

33
Q

How is solubility related to equilibrium?

A
  • When a solute is added to a solvent, it dissolves in it and this continues till the the dissolved and undissolved solute are in equilibrium with eachother.
  • At this stage the process of dissolution and crystalisation accur at the same rate.
34
Q

What is degree of solubility?

A
  • It is a quantitative measure of solubility.
  • It is the amount of solute that can be dissolved in a given amount of solvent.
  • It is achieved by solubility product constant.

Chemistry (11 decks)

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