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chem - chloe > solutions part 1 > Flashcards

solutions part 1 Flashcards

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1
Q

——– is formed when one substance dispersed uniformly throughout another

A

solution

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2
Q

other name for solution

A

homogeneous mixture

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3
Q

2 components of homogeneous mixture

A

solute and solution

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4
Q

meaning its components are not visible to the naked eye

A

homogeneous in nature,

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5
Q

TRUE OR FALSE

A Solution scatters in a light beam.

A

false

A Solution does not scatter a light beam because there are no particles to obstruct the light.

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6
Q

The ——–, which is the scattering of light by particles in a mixture, occurs in suspensions, not in solutions.

A

Tyndall effect

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7
Q

where does the Tyndall effect occur?

A

in suspensions

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8
Q

true or false

Components of a solution can be separated using simple mechanical filtration.

A

false

Components of a solution cannot be separated using simple mechanical filtration.

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9
Q

——— is the liquid then ——- is the particles na nag settle down or also known as precipitate.

A
  1. Supernatant
  2. residue
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10
Q

The maximum amount of a substance that can be dissolved in a given volume of solvent.

A

solubility

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11
Q

when a substance can be dissolved in a solvent.

A

Soluble

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12
Q

when a substance cannot be dissolved in a solvent.

A

Insoluble

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13
Q

Two liquids that are soluble in each other.

A

Miscible

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14
Q

Two liquids that are not soluble in each other.

A

immiscible

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15
Q

The solubility of a substance depends on the —- of both the solute and the solvent.

A

polarity

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16
Q

true or false

substances with similar polarities dissolve well in each other. The greater the difference in polarity, the lower the solubility.

A

true

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17
Q

factors affecting solubilty (3)

A

polarity

temp

pressure

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18
Q

—- is when an entity contains two distinct and opposite poles that can either attract or repel each other

A

Polarity

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19
Q

true or false

increasing the temp decreases the solubility of the solute in the solvent

A

false

increasing the temp increases the solubility

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20
Q

For —- solutes, the effect of pressure on solubility is negligible,
meaning it has little to no effect.

A

solid

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21
Q

true or false

The solubility of a gas in a liquid is directly proportional to the applied pressure.

A

true

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22
Q

a physical or chemical situation where a system can take no more of a substance

A

saturation

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23
Q

When equilibrium is reached the rates of dissolution and precipitation are equal, there is some dissolved and some undissolved solute. this state indicates that the solvent has dissolved as much solute as possible, and any additional solute will remain undissolved.

A

dynamic equilibrium

24
Q

Contains the maximum amount of a
given solvent at a specific temperature

A

Unsaturated Solution

25
Q

Contains less solute than it has the
capacity to dissolve

A

Saturated Solution

26
Q

Contains more solute than is present
in a saturated solution

A

Supersaturated Solution

27
Q

are often formed by heating the solvent to dissolve more solute than it normally would at lower temperatures. As the solution cools, the excess solute remains dissolved until disturbed.

A

Supersaturated Solution

27
Q

These are the forces of attraction between molecules of the solute and solvent.

A

INTERMOLECULAR ATTRACTIONS

28
Q

These forces determine how well the solute and solvent interact to form a solution. For a solution to form, the —————-between the solute and solvent must be compatible, meaning the polarity of both should be similar for effective interaction.

A

intermolecular forces

28
Q

forces within the molecules themselves. Before the solute and solvent can interact, the —— holding the solute particles together and those holding the solvent molecules together must be overcome.

A

intramolecular forces

29
Q

true or false

breaking of bonds is not necessarry to allow the solute and solvent to mix

A

false

breaking of internal bonds allows the solute and solvent to mix.

30
Q

Solvent particles surround solute particles, effectively coating them and leading to the dissolution of the solute in the solvent. When water is the solvent, the process is called ————-.

A

hydration

31
Q

As solvation occurs, the solvent particles form a cage-like structure around the solute particles, trapping them within this ——

A

“solvent cage.”

32
Q

Dissolution overall can be either —- or —–

A

endothermic or exothermic

33
Q

true or false

Whether the dissolution is endothermic or exothermic depends on the balance between the energy required to break the initial bonds (in the solute and solvent) and the energy released when new bonds are formed during solvation. If more energy is required, the process is exothermic if more energy is released, it is endothermic

A

false

if more energy is required, the process is endothermic; if more energy is released, it is exothermic.

34
Q

Energy is released, meaning the
formation of new bonds between the solute and solvent releases more energy than is needed to break the original bonds. This results in an increase in temperature.

  • more energy released in mkaing bonds
A

exothermic

35
Q

Energy is absorbed, which means
more energy is required to break the bonds within the solute and solvent than is released when new bonds are formed between them. This results in a DECREASE in temperature.

A

endothermic

36
Q

steps of solution (3)

A

solvent solvent

solute solute

solute solvent

37
Q

step?

The forces holding the solute
particles together must be overcome for the solute to dissolve.

A

solvent solvent (1)

38
Q

step?

After the solute andsolvent
molecules are separated, new interactions (or bonds) form between them. This is crucial for the formation of a solution.

A

solute solute (2)

39
Q

step?

Thesearetheinteractionsthatoccur
between solute and solvent molecules once the solute has been dispersed. The strength of these interactions determines whether the solute will stay dissolved or precipitate out of the solution.

A

solute solvent (3)

40
Q

types of imf

weakest to strongest (5)

A

LONDON dispersion

dipole induced

dipole dipole

h bonding

ion dipole

41
Q

IMF:

Weakest, occurs between all molecules, especially nonpolar ones.

A

london dispersion

42
Q

imf: Occurs when a polar molecule induces a dipole in a nonpolar molecule.

A

dipole induced

43
Q

imf: Occurs between two polar molecules.

A

dipole dipole

44
Q

imf: Occurs when hydrogen is bonded to highly electronegative atoms like oxygen, nitrogen, or fluorine.

A

H bonding

45
Q

imf: Strongest, occurs between an ion and a polar molecule.

A

ion dipole

46
Q

true or false

hotter temperatures are more ideal for dissolving gases in a solvent.

A

false
, lower temperatures are more ideal for dissolving gases in a solvent.

47
Q

true or false

Heating up the solution makes the solid solute dissolve more easily.

A

true

48
Q

this states that the solubility of gases is directly proportional to the partial pressure of the gas above the liquids

A

henry’s law

49
Q

t or f

When pressure increases over the solvent, it allows the molecules of gases to interact more with the solvent

A

true

50
Q

t or f

Increasing the pressure compresses gas particles, bringing them closer to the solvent molecules, which enhances solubility. Conversely, decreasing the pressure results in lower solubility as gas particles spread out.

A

t

51
Q

a solutiion can be —- or —-

A

dilute or concentrated

52
Q

Solution contains less solute than solvent.

A

dilute

53
Q

Solution contains more solute than solvent.

A

concentrated

chem - chloe (2 decks)

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