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SCH4U - Chem > 7.6 Solubility Equilibria > Flashcards

7.6 Solubility Equilibria Flashcards

1
Q

What is solubility

A
  • Quantity of solute that dissolves in a quantity of a solvent at a particular temperature
  • Concentration of a saturated solution at a particular temperature
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2
Q

Example of solubility

A

How much sugar can dissolve in water at 100 degrees celcius

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3
Q

What is the purpose of consuming barium sulfate + water before an x-ray

A
  • Its low solubility allows it to remain a solid in one’s body, and the solid (undissolved) crystals create a clear image of the digestive tract
  • Barium ions are toxic if dissolved, so knowing its poor solubility helps us know its safe to consume
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4
Q

What do ionic compounds form when placed into water

A

A dynamic equilibrium

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5
Q

What happens to an ionic compound like AgI in water

A

Since it has low solubility, its ions remain tightly packed in a crystal lattice

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6
Q

How does water try to dissolve an ionic compound (ex. AgI)

A

The charged ends of polar water molecules orient themselves around opposite charged ions to pull them into solution (ex. Partial negative oxygen orients around positive silver ions)

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7
Q

What are the forward and reverse reactions of
AgI (s) → Ag+ (aq) + I- (aq)

A

Forward: Dissolution
Reverse: Precipitation

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8
Q

When a solution is saturated, it has reached…

A

Equilibrium

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9
Q

Define saturation

A

When a solvent contains the max amount of solute at a certain temperature and pressure, and concentrations remain constant

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10
Q

Define solubility equilibrium

A

A dynamic equilibrium between a solute and a solvent in a saturated solution in a closed system

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11
Q

Is a solubility equilibrium heterogenous or homogenous

A

Heterogenous: Between a solid ionic compound and its aqueous ions

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12
Q

Why can AgI (s) be ignore in the equilibrium law equation

A

It’s a solid, has constant concentrations

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13
Q

What is Ksp

A

The solubility product constant from the equilibrium law equation of a saturated solution at a certain temperature

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14
Q

When does the solubility of an ionic compound vary

A

Depending on the ions it contains

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15
Q

How do highly charged anions and cations do and why

A

They make a compound less soluble because it takes more energy for the solvent to break its crystal lattice

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16
Q

Compare solubility of divalent to monovalent ions

A

Divalent ions such as calcium and carbonate are less soluble than monovalent ions such as nitrate and sodium

17
Q

What happens when 2 aqueous solutions mix

A

They can form an ionic compound with low solubility that precipitates out of the solution

18
Q

What happens if you pair a cation with an anion vs another cation

A

Cations + anions: Might be soluble
Cations + Cations: Insoluble

19
Q

A precipitate forming depends on…

A

Concentrations of the ions

20
Q

What is the trial ion product

A

Product of concentrations of ions raised to powers of coefficients to determine if precipitation occurs

21
Q

If Q > Ksp…

A

Rxn shifts left and precipitation occurs

22
Q

If Q < Ksp…

A

Rxn shifts right and no precipitation occurs

23
Q

If Q = Ksp…

A

Solution is at equilibrium, no precipitation occurs

24
Q

What is the common ion effect

A

By adding a common ion that it’s in ionic compound to a dissolution system, you can make the reaction shift left and form a precipitate

25
Q

A precipitate will only form after the common ion effect if..

A

The new concentrations of aqueous ions push the equilibrium past the solubility limit represented by Ksp

26
Q

What kind of solutions can the common effect occur in

A

Any in between solutions of low and high solubility

27
Q

Would silver acetate be more or less soluble in silver nitrate or water

A

Since silver nitrate has a common ion, it will make silver acetate less soluble than in water due to the common ion effect

28
Q

Define phase equilibrium

A

Equilibrium between different physical states
Ex. Bromine equilibrium

29
Q

What happens when a dissolving substance reaches equilibrium

A

It stops dissolving

30
Q

Do highly soluble compounds form an equilibrium

A

No

SCH4U - Chem (9 decks)

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