TITRATION OF STRONG ACID WITH STRONG BASE:

The titration of HCl (aq) with a standardized NaOH solution illustrated the titration of strong acid by a strong base.

The molecular and net ionic equation is.

Case (1): At the start point before any titrant has been added the receiving flask contains only 0.10 M HCl and 50 ml. Because it is strong acid so

Case (2): After starting but before equivalent point.

Case (3): At equivalent point

Case (4): Before equivalent point

TITRATION SUMMARY TABLE:

S.N.	Volume of HCl Taken	Volume of NaOH	PH
1	50.0 ml (In ml) And 0.10 M	0.0 (In ml) And 0.10M	1.0
2		10	1.17
3		20	1.36
4		30	1.60	NAVA>NBVB
5		40	1.95
6	(Vertical Over)	45	2.27
7		49	2.99
8	50.0 ml (In ml) And 0.10 M	50	7.0	NAVA=NBVB
9		51	11	NAVA<NBVB
10		60	11.95

GRAPHICAL REPRESENTATION:

ILLUSTRATIVE EXAMPLE: Find the pH of following titrations:

(A) 500 ml, 0.10 M HCl + 500 ml 0.10 M Ca(OH)₂

(B) 400 ml, M/200 Ca(OH)₂ + 400 ml M/50 HNO₃ 

 _{ANSWERS KEY:
(A): PH=12.6989  (B): PH=2.6}

Basicity of Guanidine :

Guanidine is strongest organic nitrogenous compound with the formula HNC(NH₂)₂. Guanidine is analogue of carbonic acid. That is, the C=O group in carbonic acid is replaced by a C=NH group, and each OH is replaced by a NH₂ group.

A guanidine group also appears in larger organic molecules, including on the side chain of arginine (a basic amino acid).

It is a colourless solid that dissolves in polar solvents. It is a strong base that is used in the production of plastics and explosives. It is found in urine as a normal product of protein metabolism.

Basicity of Guanidine:

Guanidine is the strongest base among neutral compounds:

The remarkable basicity of guanidine is attributed to the fact that the positive charge on

the guanidinium ion is delocalized equally over the three nitrogen atoms, as shown by

these three equivalent resonating  structures:

Basicity of nitrogen can be increased by attachment to pi-donors (NH₂) group. These two pi-donating NH₂ groups donate electron density to the (pi-accepting) C=NH. Hence, the guanidinium ion is a highly stable cation.
IIT UPDATE:
QUESTION:

SOLUTION: (B)

Related Questions:

1. How is base strength related to the availabihty of the electron-pair?
2. Amines are more basic than ammonia why?
3. What is relative basic strength order 1° amines , 2°amines and 3° amines ? Explain:
4. Give an explanation for the fact that Guanidine NH=C(CH3)2 is a stronger base than most of amines?
5. Arrange in correct order of basic Character of aniline, pyrrol, pyridine and piperidine?
6. What is correct basicity order of pyridine, pyridazine, pyrimidine and pyrazine ?
7. Give an explanation for the fact that Guanidine NH=C(CH3)2 is a stronger base than most of amines?
8. Arrange in correct order of basic Character of aniline, pyrrol, pyridine and piperidine?
9. What is correct basicity order of pyridine, pyridazine, pyrimidine and pyrazine ?
10. Why pyridine is more basic than Pyrrole?
11. Why pyrimidine is less basic than pyridine?
12. Imidazole is more basic than pyridine? Why?
13. Biological Important of Imidazole and structure:
14. Pyridine is almost 1 million times less basic than piperidine? Why?
15. Cyclohexylamine amine is the stronger base than Aniline? Why?
16. Tetrahydroquinoline amine is the stronger base than Tetrahydroisoquinoline? Why?
17. Arrange the following in the order of increasing basicity : p-Toluidine, N, N-Dimethyl-p-toluidine, p-Nitroaniline, Aniline. (I.I.T.1986)
18. Arrange the following in the increasing order of their acid strength : Methyl amine, Dimethyl amine, Aniline, N-methyl aniline (I.I.T, 1988).