Acid and Bases

K =

concentration of products over concentration of reactants

Kw =

concentration of OH- times concentration of H+

pH =

-log(concentration of H+)

pH + pOH =

14

How does temperature affect K?

Temp INC K INC because more dissociation

An acid is a

proton donor

A base is a

proton acceptor

Amphoteric

can act as acid or base

Strong means

fully dissociates in solution

Spectator cations

Li, Na, K, Rb, Cs, Ca, Sr, Ba

Spectator anions

Cl, Br, I, NO3, CIO4, CIO3

If you are left with just H+

it’s a strong acid

If you are left with just OH-

it’s a strong base

If you are left with H+ and a common anion

it’s a weak acid

If you are left with an anion

it’s a weak base

If you are left with a cation

it’s a weak acid

Weak acid when you’re left with

metal, base and H+, HA

Weak base when you’re left with 

anion, nitrogen molecule

Strong acid when you’re left with

H+

Strong base when you’re left with

OH-, H-, O2-,N3-

Calcuating pH for SB or SA

find H+ then pH = -log(H+)

or find OH- then pOH = -log(OH-) then pOH + pH = 14

Calculating pH for WA or WB

ICE table then use equilibrium constant to find x using quadratic equation or approximation

When is it acceptable to assume x is negligible

if % ionization (x amt/initial amt) is less than 5

Mixture of SA and SB

dilution then nuetralization with ICE table then find H+ then pH = -log(H+) or find OH- then pOH = -log(OH-) then pOH + pH = 14

Mixture of WA and WB

HH equation: pH = pK + log(B/A)

Mixture of one weak and one strong

dilution then neutralization with ICE table…

1. W/W use HH equation 

2. WA or WB find x using quadratic equation or approximation

3. SA or SB ind H+ then pH = -log(H+) or find OH- then pOH = -log(OH-) then pOH + pH = 14

For S/W mixtures half way to eq point

pOH = pKa