Equilibrium Quick Flashcards

If Q greater than K

Shift left

Q less than K

Shift right

Raising temp in exothermic

Shift left

Raising temp in endothermic

Shift rightI

If a solution is satuated?

Concentrations are at their maximum

Increasing pressure

Shifts equilibrium to the side with fewer moles of gas.

AgCl(s)⇌Ag+(aq)+Cl−(aq) (Ksp=?)

[Ag+][Cl−]

What is Ksp?

The equilibrium constant for the dissolution of a slightly soluble ionic compound.

Includes only aqueous ions, not solids.

What does a larger Ksp mean?

The compound is more soluble.

How do coefficients affect Ksp? Example:

CaF₂ ⇌ Ca²⁺ + 2F⁻

They become exponents. Ksp​=[Ca2+][F−]2

How do you use Q vs Ksp?

Q < Ksp → no precipitate

Q = Ksp → equilibrium

Q > Ksp → precipitate forms

What is the common ion effect?

Adding an ion already present shifts equilibrium left, decreasing solubility.

What happens when you add a common ion?

Increases ion concentration

Makes Q > Ksp

Shifts left

More solid forms

Does adding a common ion increase or decrease solubility?

Decreases solubility

Why does precipitation occur when Q > Ksp?

There are too many ions, so the system forms a solid to return to equilibrium.

sp​=[Ca2+][F−]2 (how would yo uwrite out with x)

ksp=(x)(2x)²