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Chemistry Honors > Solutions Unit > Flashcards

Solutions Unit Flashcards

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1
Q

What is a solution?

A

A homogeneous mixture

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2
Q

What is a mixture?

A

A combination of 2 or more substances, not chemically combined

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3
Q

How can mixtures be seperated?

A

Some by filtration if the particles are big enough, others by evaporation or distillation (if the boiling points are different)

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4
Q

What is a homogeneous mixture?

A

It is a mixture that is the same all throughout

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5
Q

What is a heterogeneous mixture?

A

A mixture that is not uniform

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6
Q

What is a solute?

A

The dissolved substance in the solution (or the part in lesser amount)

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7
Q

What is a solvent?

A

The part of a solution in which the solute is dissolved (or the part in greater amount)

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8
Q

What is an aqueous solution?

A

A solution in which water is the solvent

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9
Q

What are the properties of a solution?

A
  • homogeneous
  • dissolved particles will not come out of the solution if left standing
  • clear and transparent
    the solute and solvent cannot be separated by filtration
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10
Q

What are the types of solution?

A

Gas (ex air), liquid (ex NaCl aq), solids (ex metals, amalgams and alloys)

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11
Q

What is concentration?

A

A ratio of solute to solvent

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12
Q

What is a concentrated solution?

A

One which has a large amount of solute dissolved per unit of solvent

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13
Q

What is a dilute solution?

A

One which has a small amount of solute dissolved per unit of solvent

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14
Q

What is solubility?

A

How much solute can dissolve in a particular solvent under given conditions of temperature and pressure.

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15
Q

What is a saturated solution?

A

One which the solvent has dissolved all the solute it can hold at given conditions.

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16
Q

What is an unsaturated solution?

A

One which the solvent has not yet dissolved all the solute it can hold

17
Q

What are the factors that affect solubility?

A

Temperature: for ionic substances (salts) an increase in temperature will increase the solubility. For gases, an increase in temperature lowers solubility.

Nature of the solute and solvent: like dissolves like, polar dissolves polar (and ionic), non-polar dissolves non-polar.

Pressure (for gases only): The higher the pressure the greater the solubility

18
Q

What conditions are gases most soluble at?

A

High pressure and lower temperature.

19
Q

What are the factors affecting rate of solution?

A
  • Size of the particles
  • Stirring
  • How much of the solute is already dissolved
  • Temperature
20
Q

What is a precipitate?

A

A solid that forms suddenly in a solution as a result of a chemical reaction or a change in solubility.

21
Q

What are colligative properties?

A

Properties that depend on the number of particles in a solution (not on the identity of the solute).

22
Q

What do colligative properties include?

A

Freezing point depression and boiling point elevation.

23
Q

What is freezing point depression?

A

Adding a solute to a solvent lowers the freezing point of the solution. (the solution has a lower freezing point than the pure solution)

24
Q

What is the relationship between number of particles and freezing point?

A

The higher number of particles, the lower the freezing point.

25
Q

What is molality?

A

Another method of calculating concentration.
moles of solute/kg of solvent

26
Q

Formula for calculating freezing point depression:

A

∆Tf = Kf x m

27
Q

What is Kf for water?

A

1.86 1.86 C/molal

28
Q

What are non electrolytes?

A

Substances which dissolve but do NOT dissociate in water.

29
Q

Why is this?

A

Because they do not produce ions i solution, they do not conduct electricity.

30
Q

What are electrolytes?

A

Substances which dissociate in water. They produce ions in a solution and DO conduct electricity. They are mostly ionic compounds.

31
Q

What will one mole of a electrolyte produce?

A

More than one mole of ions/particles.

32
Q

What will one mole of a non-electrolyte produce?

A

One mole of particles in a solution.

33
Q

What is the formula for freezing point depression for electrolytes?

A

∆Tf = Kf x m x number of mole of particles/ions in the solution.

34
Q

Of the following, which is an example of an electrolyte?

C6H12O6
(NH4)3PO4

A

(NH4)3PO4 because it is ionic.

35
Q

How do you calculate ppm?

A

ppm = mass of solute/mass of solution x 1000000

36
Q

How do you solve dilution problems?

A

Use the formula (Vi)(Mi) = (Vf)(Mf) and remember to subtract.

Chemistry Honors (11 decks)

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