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MEHC U2 > Solutions > Flashcards

Solutions Flashcards

1
Q

What are the 5 types of solutions?

A 
Gas in gas 
Gas in liquid
Liquid in liquid
Solid in liquid
Solid in solid
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2
Q

What is an example of a gas in a gas?

A

Air

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3
Q

What is an example of a gas in liquid?

A

Lemonade

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4
Q

What is an example of a liquid in a liquid?

A

Diluted cordial

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5
Q

What is an example of a solid in liquid?

A

Salt water

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6
Q

What is an example of a solid in solid?

A

Brass

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7
Q

Define solvent

A

Substance present in the greater amount in a solution

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8
Q

Define solute

A

Substance that dissolves in the solvent

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9
Q

How is the solubility of a solute (solid) temperature dependent?

A

The solubility of most solids increase with an increase in temperature

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10
Q

How is the solubility of a solute (gases) temperature dependent?

A

The solubility of most gases decreases with an increase in temperature.

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11
Q

How are solutions formed?

A

When the solute-solvent attractions are stronger than the solute-solute and solvent-solvent attractions

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12
Q

How does water form strong attractions with many different substances to create a solution? What are the different substances that water can make strong attractions with?

A

As it is a polar molecule
This includes other polar molecules
Many ionic solids (solubility table)
Some non-polar molecular substances that contain H, N and O atoms with non-bonding Electron pairs

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13
Q

How does pressure changes only affect gas in liquid solutions?

A

An increase in pressure results in an increase in solubility

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14
Q

What is an unsaturated solution?

A

One in which more solute can dissolve at a given temperature and pressure

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15
Q

What is a saturated solution?

A

One in which no more solute can dissolve at a given temperature and pressure

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16
Q

What is a super saturated solution?

A

One that contains more solute than a saturated solution at the same temperature

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17
Q

How can a super saturated solution achieved?

A

It can be achieved by heating a saturated solution until all the solute dissolves and then slowly and carefully cooling the solution back to the original temp.

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18
Q

In order for a solute to dissolve what must occur?

A

The solute bonds/attractions must be broken.

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19
Q

How is a new solute formed?

A

Solvent bonds/attractions must be formed

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20
Q

How does common salt dissolve in water?

A

The attraction of the sodium ions for the chlorine ions (ionic bond) is weaker than the attractions of the (+) and (-) charged ions for the oppositely charge poles of the water molecule

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21
Q

What is the general rule for dissolving a solute in a solvent?

A

In general, a solute will dissolve in a solvent only if the electrostatic forces within the solute are similar to those within the solvent. (LIKE DISSOLVES LIKE)

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22
Q

When a solute dissolved in a solvent the resulting solution has different physical properties to the original solvent. What are the 3 significant differences that can be observed in?

A

Vapour pressure

Boiling Point

Melting Point

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23
Q

How is vapour pressure significantly different for the solution compared to the original solvent?

A

Depends on the tendency of the liquid particles to escape from the surface of the liquid.

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24
Q

How does addition of a solution decrease vapour pressure?

A

Addition of a solute decrease the proportion of ‘free’ solvent molecules at the surface of the liquid

Adding a solute decrease the vapour pressure of the solvent/solution

25
How is Boiling Point significantly different for the solution compared to the original solvent?
If a solution has a lower vapour pressure than the opure solvent, the boiling point of the solution will be higher than that of the pure solvent
26
When will a liquid boil for the boiling point of a solution, compared to the original solution.
Liquids will boil when all of the particles have a vapour pressure to or higher than the pressure of the atmosphere above the liquid. That is, adding a solute will raise the B.P of the solvent/solution
27
How is melting Point significantly different for the solution compared to the original solvent?
A solution will have a lower melting point than the pure solvent When a solute dissolves in a solvent the solute-solute attractions are stronger than the solute-solvent attractions.
28
So what occurs to the melting point when a solute is added to a solvent?
Adding a solute will depress the freezing point of the solvent/solution
29
What are 3 properties used to differ a solution from the original pure liquid solvent? (Liquid phase)
Freezing point Boiling point Vapour Pressure
30
How is freezing point different in the solution compared to the original pure liquid solvent? (Liquid phase)
Freeing point of the solutions is lower than the freezing point of the pure solvent
31
Why does the freezing point change for a pure liquid solvent when a solute is added? (Liquid phase)
Solute particles disrupt the normal pattern of the solvent particles in the solid array and a lower temp is required before a solid lattice can be achieved
32
How is boiling point different in the solution compared to the original pure liquid solvent? (Liquid phase)
Boiling point of the solution is higher than the boiling point of the solvent
33
Why does the boiling point change for a pure liquid solvent when a solute is added? (Liquid phase)
Solute-solvent attractions are stronger than the solvent-solvent attractions and therefore more energy is required to overcome them and boil the liquid
34
How is vapour pressure different in the solution compared to the original pure liquid solvent? (Liquid phase)
Vapour pressure of the solution is lower than the vapour pressure of the pure solvent due to the stronger attractions present in the liquid
35
What are precipitation reactions?
Occurs when two solutions are mixed and a reaction occur between 2 ions where the attraction of the ions for each other (solute-solute attractions) is stronger than the attraction of these ions for water molecules ion bonds form an insoluble ionic solid (precipitate)
36
What is a concentration of a solution?
Refers to the amount of solute present in a given volume of a solution
37
What are the 4 main ways of expressing the concentration of a solution?
Moles per litre Grams per litre Part per million Percentage composition by mass
38
define solution
a mixture where the particles of a solute are homogeneously spread amongst the particles of a solvent **A single phase homogenous mixture
39
Define aqueous solution
liquid solutions where the solvent is water
40
What are strong electrolytes?
when these dissolves in water they are entirely present (or at least mostly) as independent mobile ions They are fully ionised/dissociated
41
What are weak electrolytes?
When these dissolve in water they are partly present as independent mobile ions (but mostly as molecules) They are partially ionised/dissociated
42
What are non-electrolytes?
when these dissolve in water they do not produce ions they are not entirely present as molecules
43
What substances are strong electrolytes?
All ionic compounds and strong electrolytes | eg. NaCl, Ca(NO3)2
44
What substances are weak electrolytes
weak acids or bases eg. Ch3COOH, H2S, NH3 etc....
45
What substances are non-electrolytes?
Most covalent molecular substances like sugar as it does not conduct electricity when molten or in aqueous solution
46
What is dissociation?
when an ionic solid dissolves in water, the ions present within the ionic solid are released into water to form a solution of independent mobile ions IONS HAVE SEPERATED IN SOLUTION
47
What is ionisation?
When a covalent molecular substance dissolves in water, molecules of the electrolyte react with water to form ions not originally present within the substance IONS HAVE FORMED
48
Why is there sometime one arrow used in a dissociation or ionisation reaction?
shows that an ionisation or dissociation reaction is complete (case for strong electrolytes)
49
Why is there sometime double arrow used in a dissociation or ionisation reaction?
used to show the reaction does not go to completion (significant concentrations of ions and molecules are both present) (case for weak electrolytes)
50
Define electrolyte.
as a substance that conducts electricity (contains freely moving ions) When molten or when dissolved in water (aqueous solution)
51
Give an example of a dissociated reaction with NaCl
NaCl (s) --(H2O)--> Na+(aq) + Cl-(aq) ionic solid reacts with water to produce ions that re no longer bonded to each other
52
Give an example of a dissociated reaction with HCl
HCl(g) --(H2O)--> H+(aq) + Cl-(aq) Covalent bonded substance reacts with water and electron transfer occurs to form ions
53
What are 4 examples of strong electrolytes?
HCl HBr HI H2SO4
54
What are 4 examples of weak electrolytes?
HF NH3 CO2 H3PO4
55
What does electrical conductivity depend on in a solution?
The greater the concentration of ions in a solution the greater is its ability to conduct a current
56
What is the equation for moles per litre?
c=n/v C-mol L-1 n- no of moles V- volume in L of solution
57
What is the equation for grams per litre?
c=m/v c- g L-1 m- mass of solute in g v- volume in L of solution
58
What is the equation for parts per million?
Ppm= mass of solute in mg/mass of solution in Kg
59
What is the equation for percentage composition by mass?
% by mass= mass of solute in g / mass of solution in g x100

MEHC U2 (8 decks)

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