CONCENTRATIONS & SOLUTIONS Flashcards

1
Q

c = kP

P is the

A

pressure of the gas over the solution

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2
Q

Each ion is surrounded by solvent molecules. If the solvent is water, the ions are []

A

hydrated

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3
Q

Low [] = Low []

A

Low P = Low C

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4
Q

What are the Intermolecular forces?

A

Dispersion Forces, H-Bonding, Dipole dipole

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5
Q

contains less solute than the solvent has the capacity to dissolve at a specific temperature.

A

unsaturated

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6
Q

c = kP

c is the

A

concentration (M) of the dissolved gas

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7
Q

c = kP

k is a

A

constant (mol/L*atm) that depends only on temperature

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8
Q

Two substances with similar [] are likely to be soluble in each other.

A

intermolecular forces

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9
Q

is electrostatically attracted to an O, N, or F atom in another molecule

A

h-bonding

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10
Q

Factors affecting Solubility

A

Nature of Solvent, Temperature, pressure

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11
Q

Enthalpy (∆H) changes with each interaction [].

A

broken or formed

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12
Q

contains the maximum amount of a solute that will dissolve in a given solvent at a specific temperature.

A

saturated

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13
Q

C2H5OH in H2O

A

polar molecules are soluble with polar solvents

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14
Q

The solubility of a gas in a liquid is proportional to the pressure of
the gas over the solution

A

Henry’s law

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15
Q

Nonpolar substances tend to dissolve in []

A

non polar solvent

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16
Q

are attractive forces between permanent dipoles of two polar molecules

A

Dipole dipole

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17
Q

occurs when hydrogen atom is bonded to O, N, or F

A

h-bonding

18
Q

Type of Force: Relative Strength: Exhibited by

London Dispersion

A

London Dispersion: Weak: All molecules

19
Q

present in polar molecules.

A

Dipole dipole

20
Q

contains more solute than is present in a saturated solution at a specific temperature.

A

supersaturated

21
Q

are very weak interactions due to the momentary changes in electron
density in a molecules.

A

Dispersion Force

22
Q

Type of Force: Relative Strength: Exhibited by

Hydrogen Bonding

A

H-Bonding: Strong: Molecules with O-H, N-H, H-F

23
Q

ionic compounds are more [] in polar solvents

A

soluble

24
Q

High [] = High []

A

High P = High C

25
Q

larger dipole moment, larger the forces.

A

dipole dipole

26
Q

Solvent molecules [] to surface ions. The ions are [] (surrounded by solvent).

A

attracted - solvated

27
Q

Henry’s Law Formula

A

c = kP

28
Q

Types of solutions

A

Saturated, Unsaturated, Supersaturated

29
Q

Type of Force: Relative Strength: Exhibited by

Dipole dipole

A

Dipole Dipole: Moderate: Molecules with net dipole

30
Q

are homogeneous mixtures of two or more pure substances.

A

Solutions

31
Q

a substance that is dissolved
in a solvent to produce a
solution.

A

Solute

32
Q

Polar substances tend to dissolve in []

A

polar solvent

33
Q

Present in covalent molecules.

A

Dispersion

34
Q

Factors Affecting Solubility

If the solution process [], then the solubility will be [] with [] temperature

A

Temperature

releases energy - decreased - increased

35
Q

Chemists use the axiom “”

A

like dissolves like

36
Q

the fraction of a solution in
which the other components
are dissolved.

A

Solvent

37
Q

NaCl in H2O or NH3(l)

A

ionic compounds are more soluble in polar solvents

38
Q

also known as Van der Waals forces and London dispersion

A

Dispersion forces

39
Q

Factors Affecting Solubility

If the solution process [], then the solubility will be [] as the temperature is []

A

Temperature

absorbs energy - increased - increased

40
Q

CCl4 in C6H6

A

non polar molecules are soluble with non polar solvents