Solutions Flashcards

1
Q

Solution

A

A homogeneous mixture of two or more substances

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2
Q

Solute

A

The substance that gets dissolved

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3
Q

Solvent

A

The substance that does the dissolving

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4
Q

Aqueous Solutions

A

Solutions that have water as the solvent

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5
Q

If an ionic solute is dissolved in water →

A

conducts electricity (electrolyte)

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6
Q

If a molecular solute is dissolved in water →

A

nonconductor (non electrolyte)

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7
Q

Solubility

A

A measurement of how soluble a solute is in a specific solvent under certain conditions (ie temperature and pressure)

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8
Q

Soluble

A

CAN dissolve in solvent

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9
Q

Insoluble

A

CAN’T dissolve in solution

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10
Q

In order for solutions to occur…

A
  • The solute and solvent must be attracted to one another

- “Likes Dissolve Likes”

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11
Q

What does “Likes Dissolve Likes” mean?

A

Polar solute can dissolve in polar solvents

Non-polar solute can dissolve in non-polar solvents

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12
Q

Unsaturated

A

A solution that can still dissolve more solute

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13
Q

Saturated

A

The solvent has dissolved the maximum amount of solute possible at a given temperature and pressure

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14
Q

Supersaturated

A

A solution that contains more than could be dissolved by the solvent under normal circumstances

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15
Q

Table G

A
  • A point UNDER the line is an UNsaturated solution
  • A point ON the line is a saturated solution
  • A point ABOVE the line is a SUPERsaturated solution
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16
Q

What will increase the solubility of a gas?

A

Increasing pressure and decreasing temperature

17
Q

How do you make a real gas behave like an ideal gas?

A

Decreasing pressure and increasing temperature

18
Q

Homogeneous

A

Looks the same all throughout

19
Q

How do you see if something’s a gas on Table G?

A

If the line DECREASES

20
Q

How do you see if something’s a solid on Table G?

A

If the line goes up

21
Q

Concentration

A

amount of solute per given amount of solvent

22
Q

Molarity

A

moles of solute per liters of solution

23
Q

Molarity Equation

A

M = moles solute
———————–
liters of solution

24
Q

Units for Molarity

A

M or mol/L

25
Molarity TIPS
* Use liters in denominator (ml / 1000 = L) | * Use moles NOT grams
26
Parts per Million
ppm = mass solute --------------------- x 1 Million mass solution
27
PPM and % by Mass *TIPS*
solute / solute + solvent (solution) *not over solvent! Over solution!
28
Percent by Mass
mass solute -------------------- x 100 mass solution
29
Dilution | increasing the amount of solvent decreases concentration
M1 (V1) = M2 (V2) * M = molarity * V= volume
30
Freezing Point Depression
- Solutions have lower freezing pts than water | - More solute = lower freezing pt
31
Boiling Point Elevation
- Solutions have higher boiling points than pure water | - More solute = higher boiling pt
32
Ionic vs Covalent Compounds
Since ionic compounds dissociate into ions, they create a greater concentration of particles!
33
Factors that Affect Solubility
- Temperature - Pressure - Nature of solute/solvent
34
Temperature affects solubility
Gases -As temperature ↑, solubility ↓ Solids -As temperature ↑, solubility ↑
35
Pressure affects solubility
- ONLY AFFECTS GASES! | - As pressure ↑, solubility ↑
36
Nature of Solute/Solvent
Likes Dissolve Likes