12.2 Solubility and Factors Affecting Solubility

12.2 Solubility and Factors Affecting Solubility Dr. Fred Omega Garces Chemistry 200 Miramar College 1 Solubility January 13 Properties of Solu...
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12.2 Solubility

and Factors Affecting Solubility

Dr. Fred Omega Garces Chemistry 200 Miramar College

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Solubility

January 13

Properties of Solution Characteristics: • Distribution of particles is uniform • Components in solution do not separate upon standing • Components cannot be separated by filtration. • Solute / Solvent mixes in ratios - up to the solubility limit. • Solution is almost always transparent. • Compounds of solution may be separated by other methods i.e., distillation or chromatography.

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Solubility

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Suspended in Solution: Solubility Process Solubility - The process in which substances dissolve at the molecular level. Solubility - The maximum mass of solute capable of dissolving in a given amount of solvent at a given temperature.

Unsaturated

A solution that has the capacity to dissolve more solute.

Saturated

A solution that contains the maximum solute it can dissolve. (There are no residue)

A solution that contains more solute (in dissolved form) than the solubility limit

Immiscible - When two liquids are not soluble in each other

Miscible - When two liquids are soluble in all proportion.

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supersaturated

Solubility

January 13

1) Nature of Solute and Solvent Dissolving Process: Why is water soluble in alcohol yet water is insoluble in oil ? Solubility Factor: Solute and Solvent characteristic: • In aqueous solution, water will form strong intermolecular forces with only other polar molecules (the dissolution process) • Oil is a nonpolar substance and therefore will only form strong IMF with other nonpolar substances such as organic compounds.

An oil layer floating on water. For a substance to dissolve, the water-water hydrogen bonds must be broken to make a “hole” for each solute particle. However, the water-water interactions will break only if they are replaced by similar strong interactions with the solute.

• The result is the immisciblity of water and oil. (Later the Energetics of this process will be discuss)

Organic Chemist saying “Like Dissolves Like”

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Solubility

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Dissolution of Solid Solute What is the driving force which causes solutes to dissolve to form solutions? Covalent versus Ionic solute 1. Covalent solutes dissolve by H-bonding to water or by 2. Ionic solutes dissolve by dissociation into their ions.

LDF

Ionic

Covalent

Picture of Ethanol and NaCl dissolving 5

Solubility

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Dissolving at the molecular Level: Ionic Compounds Ionic substances NaCl, MgCl2, AgCl

The salt; NaCl or the ionic compound is a 3-D lattice.

The Na+ and Cl- are arranged in 3-D alternating ion lattice

The negative Cl- attracts the (δ+) of hydrogen in H2O while the positive Na+ attracts the (δ -) of oxygen in H2O. Occurs due to coulombic (opposite) attracts.

The solvent (H2O) interaction to the ion is the Hydration process

H2O literally pulls the lattice arrangement of the solid salt apart because of the attraction between the δ+ or δ - of water to the - or + ions. Consider: 1) M+ & X- (i.e., Na+ and Cl - ) 2) M+ to δ- oxygen of H2O & X- to δ + hydrogen of H2O

If (1) is favorable (lattice energy) then solute does not dissolve (insoluble) i.e., AgCl if (2) is favorable then hydration, solute does dissolve (soluble). NaCl 6

Solubility

January 13

Equilibrium: Dissolution = Crystallization Observe: After some time, no change in amount of solid precipitate at the bottom of the beaker. Concentration of the solution is maintained

[Solute]

D Solid

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[Solute]

Solution Solubility

At the molecular level: Amount of salt dissolving into solution equals to amount of salt recrystalizing January 13

Dynamic Equilibrium Equilibrium Situation in which changes occur at equal rates so there is no apparent net change.

LeChatelier Principle A change (stress) on a system at equilibrium will cause the system to self adjust itself to reduce the stress until a new equilibrium is re-established.

Example: Traffic at a toll bridge Vapor Pressure Sugar dissolving 13_07

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Solubility

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Ionic Vs Covalent Compounds: Electrolyte Vs. Nonelectrolyte Substance when dissolve can break-up to ions or stay intact. i.e., NaCl and sugar. Type:

% ionization:

Solubility (in H2O)

Electrolyte: conducts electricity. Strong electrolyte

100 % ionization

Weak electrolyte

less 100% ionization

very soluble slightly to very soluble

Nonelectrolyte: Do not conduct electricity no conduction

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0 % ionization

Solubility

insoluble or soluble

January 13

Dissolution at the molecular level? Spontaneity of dissolving process:

Consider the Spontaneity due to Gravity: Object drops and impact floor spontaneously. The driving force is gravity. High Energy Objects spontaneously fall because of the tendency for systems to be at a lower energy state.

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When systems proceed to a lower energy state, the process is exothermic: Energy is released. (Tends to be spontaneous) Low Energy Solubility

January 13

Driving Force for Dissolution Reaction exothermic ΔH (-) Downhill g ∴ Spontaneous Reaction exothermic ΔH (+) Uphill g Spontaneous ???

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Solubility

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Dissolution at the molecular level? Consider the dissolution of NaOH in H2O

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Solubility

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Exothermic: Dissolution Process Solution process as indicated by the enthalpy heat of solution: Dissolution via ΔHsoln can be thought of as the sum of three enthalpy changes; ΔHsolvent, ΔHsolute and ΔHmix. The result is ΔHsolution. Note, If ΔHsoln < O, Then it is a downhill, Spontaneous

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Solubility

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ΔHmix or ΔHhydration Closer Look, ΔHmix: ΔHhydr is

always negative

based on Columb’s Law. E = k |Q1•Q2| d Trends in ionic heats of hydration. Heats of hydration (ΔHhydr) are always negative because ions and water attract each other and release heat. Values for the Group 1A(1), 2A(2), and 7A(17) ions are shown as descending posts, with the ionic radius on top. The ΔHhydr values depend on charge density smaller down a group as ionic size increases and larger from Group 1A(1) to Group 2A(2) as ionic charge increases. 14

Solubility

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Consider the Dissolution of NH4Cl In the dissolution of ammonium chloride,NH4Cl, the system feels cold, indicating an Endothermic process.

An uphill process that is spontaneous. How is this possible ?

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Solubility

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Endothermic, Dissolution Process ΔHmix small, ΔHsoln (+)

Down hill (Exothermic) vs. up hill (Endothermic)

Will an unfavorable process (uphill) proceed spontaneously ? Will a substance dissolve if ΔHsoln g (+) When a solute and solvent mixes, the magnitude of three ΔH processes will determine if the dissolution process is exothermic, or endothermic. Factors determining spontaneity will be determine by thermodynamic factors and not only by enthalpies value 16

Solubility

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Second Law of Thermodynamics Why does ink spread or gas expand or your room gets chaotic? Greater probability of disorder than order.

One of the Basic Law of Nature 2nd Law of Thermodynamics: Process in which disorder increases occur spontaneously

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Solubility

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Enthalpy Diagram for Series of Dissolution Processes NaCl in H2O

NaOH in H2O

NH4NO3 in H2O

Enthalpy diagrams for dissolving three ionic compounds in water. The enthalpy diagram for dissolving an ionic compound in water includes the negative of the ΔHlattice (ΔHsolute; always positive) and the heat of hydration (ΔHhydr; always negative). A, For NaCl, the magnitude of ΔHlattice is slightly greater than that of ΔHhydr, so ΔHsoln is small and positive. B, For NaOH, ΔHhydr dominates, so ΔHsoln is large and negative. C, For NH4NO3, ΔHlattice dominates, so ΔHsoln is large and positive.

NaCl in Heptane

Hexane in Heptane

Enthalpy diagrams for dissolving NaCl and octane in hexane. A, Since attractions between ions and hexane molecules are weak, ΔHmix is much smaller than ΔHsolute. Thus ΔHsolute is so positive that NaCl does not dissolve in hexane. B, Intermolecular forces in octane and in hexane are so similar that ΔHsolute is very small. Octane dissolves in hexane because the solution has greater entropy (more disorder) than the pure components.

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Solubility

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Factors Affecting Solubility 1. Nature of Solute / Solvent. - Like dissolves like (IMF) 2. Temperate Factor i) Solids/Liquids- Solubility increases with Temperature Increase K.E. increases motion and collision between solute / solvent.

ii) gas - Solubility decreases with Temperature Increase K.E. result in gas escaping to atmosphere.

3. Pressure Factor i) Solids/Liquids - Very little effect Solids and Liquids are already lose together, extra pressure will not increase solubility.

ii) gas - Solubility increases with Pressure. Increase pressure squeezes gas solute into solvent. 19

Solubility

January 13

2 i) Temperature on Solubility: Solids & Liquids Temperature -

(Solid and Liquid)

Consider the extent in which sugar or NaCl dissolves in water. What are the conditions which will increase the solubility of sugar or salt in water.

[Solute]

D

Solid

[Solute] Solution

As the temperature increase, both solute and solvent will be moving faster, this will result in the mixing of both substance to be more effective.

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Solubility

January 13

Equilibrium Revisited [Solute]

D

Solid

[Solute]

Solution

Observe: After some time, no change in amount of solid precipitate at the bottom of the beaker. Concentration of the solution is maintained Equilibrium Situation in which changes occur at equal rates so there is no apparent net change. LeChatelier Principle A Change (i.e., stress) on a system at equilibrium will cause the system to self adjust itself to reduce the stress until a new equilibrium is re-establish. 21

Solubility

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LeChatelier Principle Teeter•Tooter At Equilibrium

Stress applied Self Adjust

Re-establish Equilibrium 22

Solubility

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Equilibrium: Stress / Relief on Reactant Stress on Reactant, Rxn shift right

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Relief on Reactant, Rxn shift left

Solubility

January 13

Equilibrium: Stress / Relief on Stress on Product, Rxn shift left

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Product

Relief on Product, Rxn shift right

Solubility

January 13

Exothermic Heats of Solution R

Energy +

P

Exothermic Process. Energy is a product

P

Heating a solution in which the ΔHsoln is exothermic (Energy is a product) results in a shift of the reaction to the left or more solute precipitating out of solution.

Temp increase

R + Energy

R 25

Energy +

P

Solubility

January 13

Endothermic Heats of Solution R+

P

Energy

Temp increase

P R

R 26

+ Energy

+ Energy

P Solubility

Endothermic Process Energy is a reactant Heating a solution in which the ΔHsoln is endothermic (Energy is a reactant) results in a Shift of the reaction to the right or more solute dissolving in solution.

January 13

Solubilities of Solids Vs Temperature Solubilities of several ionic solid as a function of temperature. Some salts have negative enthalpy of solution, (exothermic process) i.e., Ce2(SO4)3 and they become less soluble with increasing temperature. 27

Solubility

January 13

2ii) Temperature & Solubility: Gases Temperature - (Gas)

Consider the extent in which O2 or CO2 dissolves in water. What are the conditions which will increase the solubility of gas in water. [Solute]

gas

As the temperature increase, both solute and solvent will be moving faster, the gas solute however will now have enough energy to leave the liquid interface. 28

D

Solubility

[Solute]

Solution

January 13

Gas solute; Exothermic ΔHsoln P

R

Energy +

Gas above soln

Gas in solution

Temp increase

R

As the temperature increase, both solute and solvent will be move faster. The gas solute however will now have enough energy to leave the liquid interface because IMF can be overcome

+ Energy

P

R 29

Energy +

P

Solubility

January 13

Disaster: (1700 dead) from Gas Solubility

In the African nation of Cameroon in 1986 a huge bubble of CO2 gas escaped from Lake Nyos and moved down a river valley at 20 m/s (about 45 mph). Because CO2 is denser than air, it hugged the ground and displaced the air in its path. More than 1700 people suffocated. The CO2 came from springs of carbonated groundwater at the bottom of the lake. Because the lake is so deep, the CO2 mixed little with the upper layers of water, and the bottom layer became supersaturated with CO2.

Lake Nyos in Cameroon, the site of a natural disaster. In 1986 a huge bubble of CO2 escaped from the lake and asphyxiated more than 1700 people. 30

Solubility

When this delicate situation was changed, perhaps because of an earthquake or landslide, the CO2 came out of the lake water just like it does when a can of soda is opened. January 13

3 i) Pressure on Solubility: Solids / Liquid Pressure - (Solid and Liquid) The solubility of solids and liquids are hardly affected by pressure. Solids and liquids are already very close to each other. An increase in pressure will not affect solubility

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Solubility

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3 ii) Pressure on Solubility: Gas Pressure - (Gas) Solubility of gas is greatly affected by pressure Gas solute is very sensitive to pressure. Gas particles are separated by large void space, an increase in pressure will increase these particles to come closer together thereby increasing the solubility of the gas. Divers must be careful when diving to great depth because the potential of dissolved N2 gas in blood. Clinical term is the Bends. 32

Solubility

January 13

Pressure Affect: Teeter Totter Analogy R (gas)

[Solute] D [Solute] Pressure Sensitive

P (Soln)

Pressure Sensitive

Pres increase

P R

Pressure Sensitive

R

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Pressure Sensitive

P Solubility

gas

Solution

In utilizing LeChatelier Principle to determine the direction of solubility for a gaseous solute with variation in pressure, the first thing that must be establish is which side is more sensitive to pressure. In our case the gas is more sensitive than the solution. January 13

Henry’s Law At pressure of few atmosphere or less, solubility of gas solute follows Henry Law which states that the amount of solute gas dissolved in solution is directly proportional to the amount of pressure above the solution.

c = k • P

where, c = solubility of the gas (usually molality) k = Henry’s Law Constant, (solute-solvent pair) P = partial pressure of gas over solution Henry’s Law Constant (25°C)

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Gas

k

N2 O2 CO2

8.42 •10-7 1.66 •10-6 4.48•10-5

M/mmHg

Solubility

January 13

Henry’s Law: Example The solubility of ethylene (C2H4) in water at 20°C and a pressure of 0.300 atm is 1.27•10-4 m. a) calculate the Henry’s Law constant, k in (m/torr) b) How many grams of ethylene are dissolved in one kilogram of water at 20°C at 500 torr. ? Detm’ k from c = k•P, k= c / P k= 1.27•10-4 m 0.300 atm (760torr/1atm) a) k = 5.57•10-7 m / torr

= 1.27•10-4 m 228 torr

c = k•P k is constant which depends only on T c = 5.57•10-7 m / torr • 500 torr = 2.79 •10-4 m = 2.79 •10-4 m /kg H2O b)

mass = 2.79•10-4 mol • 28.0 g / mol mass = 7.80•10-3 g

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Solubility

January 13

Summary of Pressure Temperature Affect on Solubility ΔH (s, l or g) (+) Endothermic (+) i

Temp h f React

Direction g Product i decrease

Solubility h increase

(-) Exothermic (-) Exothermic

h i

f React g Product

i decrease h increase

Pressure

Direction

Solubility

h i

g Product f React

h increase i decrease

Gas solute Gas solute

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Solubility

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