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![Numarically representation
• 0.001m Nacl �+= 1 �−=1
• I=
1
2
�����
2
• I=
1
2
[(0.001× 12
)+(0.001× 12
)]
• I=
1
2
[0.001+0.001]
• I=
1
2
(0.oo2)
• I=0.001](https://image.slidesharecdn.com/debyehuckellimitinglaw1-210908050359/75/Debye-huckel-limiting-law-1-7-2048.jpg)
![• 0.002m Nacl �+=1 �− = 1
• I=
1
2
[0.002× (1)2 +0.002× (1)2]
• I=
1
2
(0.004)
• I=0.002
• �=0.04472
• log�−
+
=-0.509(1×1)×0.4473
• = -0.02276
• �−
+
= 0.9489](https://image.slidesharecdn.com/debyehuckellimitinglaw1-210908050359/75/Debye-huckel-limiting-law-1-9-2048.jpg)
Debye huckel limiting law 1
- 1. Presentation Debye huckel limitinglaw Writen By Ameer Hamza Ghazi University Dera Ghazi Khan
- 2. Explain • 1923 peterDebye and Erich Huckel • This law says about quantitative approach for the calculation of mean ionic activity of stronge electrolyte • γ± of S.E • L.L.E = log �+ _ =− �(�+�−) �
- 3. • D.H.L.L.E • Relationbetween ionic strength or mean activity • �− + ≠ I • i change (1) valancy (2) concentration • non ideal a< � ← �− + → a> � non idel • a=c ideal
- 4. • • log�− + =-A(�+�−) � •A= constant • �+�_= charge on electrolyte • I= ionc strength
- 5.
- 6. • log�− + =-A �( 1:1) Nacl • log�_ + =-A2 � (2:1) Mgcl2 • log�_ + = _A3 � (3:1) Agcl3
- 7. Numarically representation • 0.001mNacl �+= 1 �−=1 • I= 1 2 ����� 2 • I= 1 2 [(0.001× 12 )+(0.001× 12 )] • I= 1 2 [0.001+0.001] • I= 1 2 (0.oo2) • I=0.001
- 8. • � =0.03162 •log�− + =-0.509(1×1)×0.3162 • log�− + =-0.001865 • �− + =0.9957
- 9. • 0.002m Nacl�+=1 �− = 1 • I= 1 2 [0.002× (1)2 +0.002× (1)2] • I= 1 2 (0.004) • I=0.002 • �=0.04472 • log�− + =-0.509(1×1)×0.4473 • = -0.02276 • �− + = 0.9489
- 10. • so thati ↑ �− + ↓ • 0.001m Mgcl2 �+=2 �−=1 • I=0.003 • �− + = -0.05575
- 11.
- 12. • log�− + = -A(�+�−)� C.I Now we proved that I depend upon concentration and valency and ionic activity coefficient change due to change in ionic strenth
- 13. Assumptions (1) 100 %Dissociation (2) Dilute (0.01m) (3) Two Forces (a) Asymetric force (b) viscous∖ Drag force
- 14.