Chem Exam 2 Key Points

Volume increases, Pressure decreases

side with more moles is favored

Volume decreases, Pressure increases

side with less moles is favored

relationship used to convert between the two common types of equilibrium constants: Kp (pressure-based) and Kc (concentration-based).

For the reaction where [n = -1]…what happens after an increase in volume?

Q > K, so the reaction shifts left

For the rection where [n=0]…what happens after an increase in volume?

Q = K the reaction does not shift

For the reaction where [n = +1]… what happens after an increase in volume?

Q < K, the product shifts towards the product

pH =

-log(H+)

pOH =

-log(OH-)

pH + pOH = 14

Kw =

[H+] * [OH-]

[H+] =

10 ^ -pH

[OH-] =

10 ^-pOH

In pH scale… if number lower than 7

Acid = [H+] > [OH-]

In pOH scale… if number lower than 7…

Basic = [OH-] [H+]

In pH scale… if number bigger than 7…

Basic = [OH-] [H+]

In pOH scale…if number bigger than 7…

Acid = [H+] [OH-]

HF ← → H+ + F-

Ka = [H+] [F-] \ [HF]

Ka * Kb = Kw

The relationship between the acid dissociation constant (Ka), base dissociation constant (Kb), and the water ionization constant (Kw).

Strong Acid, Strong Base

Neutral

Strong base, Weak Acid

Basic

Strong Acid, Weak Base

Acidic

The stronger the acid, the lower the pKa

Highly electronegative atoms, such as Chlorine, stabilize the conjugate base, making ionization occur more readily. The stronger the acid, the lower the pKa. Increasing the number if Cl atoms further lowers pKa, as does decreasing the distance between the Cl atoms and the site of ionization.

• Reverse → flip (1/K)

• Multiply coefficients → power (Kⁿ)

• Add reactions → multiply Ks

Manipulating K