Unit 8- Solutions Flashcards

1
Q

Describe the difference between solvation and solubility.

A

Solvation is a process where solute particles separate and become associated with solvent molecules. Solvation also includes the creation of a solvent shell around the solute. Solvation is a kinetic process unlike solubility. Solubility is a measured amount of solute dissolved in a given amount of solvent where the rate of dissolution equals the rate of precipitation.

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2
Q

Describe the solution process of NaCl in water.

A

The crystal lattice structure has to break down the Na+ and Cl- ions; therefore, they dissociate (break apart). Water molecules surround each of those and then face different directions depending upon the charge of the ion. Then, we have the solvent shell completely forming.

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3
Q

What are the equations for Heat of Solution?

A

Delta H Solution= Delta H1+ Delta H2+ Delta H3; Delta H Solution= Delta H Lattice+ Delta H Hydration

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4
Q

Describe everything about Delta H1

A

Separating solute into individual components of solute; this is Delta H Lattice= Always +

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5
Q

Describe everything about Delta H2

A

Overcoming intermolecular forces to make room for solute; Always +

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6
Q

Describe everything about Delta H3

A

Interaction of solute/solvent to form solution; Always -

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7
Q

Describe everything about Delta H Hydration

A

Delta H2+ Delta H3= Delta H Hydration; it is ALWAYS -; it is dependent on the distance between ion and dipole (closer=stronger attraction)—> More Negative- Charge on ion (greater charge=stronger attraction)- Polarity of solvating molecule (greater magnitude= stronger attraction)

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8
Q

What is the formula for molarity?

A

M= moles solute/ Liters Solution

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9
Q

What is the formula for molality?

A

Molality= moles solute/ kg solvent

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10
Q

What is the formula for mole fraction?

A

Mole Fraction= moles solute/ moles total

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11
Q

What is the formula for % Mass?

A

% Mass= (moles solute/moles total)x100

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12
Q

What are the factors that affect solubility?

A

Temperature- Pressure- Relative structures of solute and solvent TPS (Temperature- Pressure- Structure)

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13
Q

What is the relationship between solubility and temperature?

A

In liquids, they have a direct relationship; in gases, they have an inverse relationship

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14
Q

Define Colloids

A

particles of intermediate size (1-1000nm) inside a dissolving medium.

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15
Q

Describe everything about Colloids

A

Smaller Particles= Solution; Large Particles= Suspension; Particles do not settle: particles are in their own phase independent of the medium- layers of ions/charges around the large particles prevents coagulation/precipitation. Intermediate and medium sized particles scatter light: can identify colloids using scattering light (Tyndall Effect); Examples include paint and fog; Particles are large enough to scatter light like a suspension, but small enough to not be seen with the naked eye.

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16
Q

Describe everything about the Tyndall Effect.

A

If you can’t see the light being passed through, it’s a solution. If you can see the light being passed through, it’s a colloid.

17
Q

Describe everything about prevention of aggregation of colloid.

A

Electrostatic Stabilization: repulsion of charges around colloid particle; Steric Stabilization: covering particles in polymers.

18
Q

Describe everything about prevention of sedimentation of colloid.

A

Similar densities of solvent and particle prevents settling; colloids coagulate (settle out) overtime by adding a salt that disrupts the repulsion forces- would become a suspension.

19
Q

What is meant by miscible and immiscible?

A

whether or not two solvents can dissolve in one another.