Lecture 3 (Physical properties) Flashcards

1
Q

What are the characteristics of Solutions?

A
  • Transparent to light
  • Does not separate on standing
  • Non-filterable
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2
Q

What are the characteristics of Colloids?

A
  • Murky/opaque to light
  • Does not separate on standing
  • Non-filterable
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3
Q

What are the characteristics of Heterogenous mixtures?

A
  • Murky/opaque to light
  • Separates on standing
  • Filterable
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4
Q

What is a Homogenous mixture?

A

A uniform mixture that has the same composition throughout

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5
Q

What is a solution?

A

A homogenous mixture that contains particles the size of a typical ion or small molecule

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6
Q

What is a colloid?

A

A homogenous mixture that contains particles that range in diameter from 2 to 500nm

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7
Q

Why don’t oil and water mix?

A

Because they have different intermolecular forces

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8
Q

What are Solid hydrates?

A

Ionic compounds that attract water strongly enough to hold onto water molecules even when crystalline

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9
Q

What is the difference in effect of temperature on solubility in solids and gases?

A

SOLIDS: as temperature increases, solubility INCREASES

GASES: as temperature increases, solubility DECREASES

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10
Q

Define Henry’s law

A

The solubility (or concentration) of a gas is directly proportional to the partial pressure of the gas if temperature is constant

[concentration (C) divided by pressure (P) is constant when T is constant]

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11
Q

How do you calculate Molarity (M)?

A

Moles of solute / Volume of solution

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12
Q

How do you calculate Moles of solute?

A

Molarity X Volume of solution

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13
Q

How do you calculate Volume of solution?

A

Moles of solute / Molarity

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14
Q

What is a way of expressing percent concentration of a solution?

A

Weight/volume percent concentration

W/V% concentration = Mass of solute (g) / Volume of solution (mL) X 100

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15
Q

What is a way of expressing a volume of solute as a % of the volume of final solution?

A

Volume/volume percent concentration

V/V% concentration = Volume of solute (mL) / Volume of solution (mL) X 100

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16
Q

What is the Dilution factor?

A

The ratio of the initial and final solution volumes (V1/V2)

17
Q

What is the difference between electrolytes and non-electrolytes?

A

ELECTROLYTES = dissolve in water and separate into ions forming solutions that are able to conduct electricity

NON-ELECTROLYTES = dissolve in water but as molecules not as ions -> solutions don’t conduct electricity

18
Q

What is the difference between a strong electrolyte, weak electrolyte and a non-electrolyte?

A

Strong electrolyte = completely dissociates into ions in an aqueous solution

Weak electrolyte = forms mostly molecules and a few ions in an aqueous solution

Non-electrolyte = dissolves as molecules in an aqueous solution

19
Q

What are the physical properties of solutions?

A
  • VAPOR PRESSURE is lower for a solution than for a pure solvent
  • BOILING POINT is higher for a solution than for a pure solvent
  • FREEZING POINT is lower for a solution than for a pure solvent
  • OSMOSIS occurs when a solution is separated from a pure solvent by a semipermeable membrane
20
Q

What is osmolarity?

A

The sum of the molarities of all dissolved particles in 1.0 liter of solution

21
Q

When are two liquids called Isotonic?

A

When they have the same osmolarity

22
Q

How is dialysis linked to osmosis?

A

In dialysis, the membrane allows the passage of solvent and small dissolved molecules but prevents passage of proteins and larger particles -> used to remove metabolic waste products from blood

23
Q
A