Ionic Equilibrium Flashcards
How to calculate pH for strong acid/ strong base?
If [H+]< 10^-6M, then [H+]net = [H+]acid + [H+]water
BUT
If [H+]≥ 10^-6M, then ph = -log10[H+]acid
pH when two stong acids are calculated
[H+]mix = (M1v1nf1 + M2v2nf2)/ v1+v2
pH when two strong bases are calculated
[OH-]mix = (M1v1nf1 + M2v2nf2)/ v1+v2
pOH = -log10[OH-]
pH = 14- pOH
pH when strong acid and strong bases are mixed
[H+]mix or [OH-]mix = (M1v1nf1 - M2v2nf2)/ v1+v2
Depending upon the value
pH when weak mono-basic acid and weak mono-acidic base
D.O.D = root ka/c
pH = [Pka - log c]/2
pH when weak polybasic acid or weak poly acidic base
pH = [Pka1 - logc]/2
pH when two weak acids and two weak bases
[H+] = root(ka1c1 + ka2c2)
pH when weak acid and strong acid/ weak bases and strong bases
[H+] = [-c2 ±root(c2^2+4ka1*c1)]/2
pH for amphiprotic species
pH = [pka1+pka2]/2
Amphiprotic Species
Species having both acid and bases charcteristic
Salt hydrolysis when weak acid and strong base are reacted
Kh = Kw/Ka
pH = 7+1/2[Pka + logc]
The pH will always be greater than 7, and will always be basic.
Salt hydrolysis when strong acid and weak base are reacted
Kh = Kw/Kb
pH = 7 - [Pkb + logc]/2
The pH will always be lesser than 7, and will always be acidic.
Salt hydrolysis when weak acid and weak base are reacted
Kh = Kw/Ka*Kb
pH = 7+[PKa-Pkb]/2
Acidic Buffer Solution and its pH
Weak Acid + Salt[Weak Acid + Strong Base]
pH = pKa + log[salt]/[acid]
Basic Buffer Solution and its pH
pOH = pKb + log[salt]/[base]
pH = 14- pOH
