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MHT-CET : Chemistry Entrance Exam

MHT - CET : Chemistry - Ionic Equilibria Formulae Page 1

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1.

Ostwald's Dilution Law

 

Weak electrolyte: K = a2 c

    

a =

 

Weak acid: Ka = a2 c

 

a =

; [H+] = a c

Weak base: Kb = a2 c

 

a =

; [OH-] = a c

 

2.

pH and pOH

 

pH = - log10 [H+]

pOH =
- log10 [OH-]

pH + pOH = 14

 

3.

Dissociation Constant for Weak Acid

 

ka =

[H+] [A- ]

[HA]

 

Weak base:

kb =

[B+] [OH-]

[BOH]

 

4.

Solubility Product

 

Ksp = [B+] [A-]
For BA B+ + A
-

 

5.

Hydrolysis of Salt: Different Formulae to be Remembered

 

Salt of weak acid and strong base:

Kh = h2.C;

    

h =

; Kh =

Kw

Ka

; [OH-] = h.c. unit = mole/dm3


Salt of strong acid and weak base:

Kh = h2.C;

    

h =

; Kh =

Kw

Kb

; [H+] = h.c. unit = mole/dm3


Salt of weak acid and weak base.

Kh = h2

    

h =

; Kh =

Kw

Ka . Kb

 

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