4 mole of an ideal gas having γ = 1.67 are mixed with 2 mole of another ideal gas having γ = 1.4. Find the equivalent value of γ for the mixture.

Answer key:  γ= 1.54

Titration of Weak acid Vs Strong base:

 (II):  Titration of Weak acid Vs Strong base:

Titration of a weak acid by strong base is a bit more complex than both acid and base are strong this is because we have consideration the equilibrium involving the weak acid and its conjugate base.

Titration Table and curve:

S.N	Acid (0.1M)	Base (0.1M )	pH	Nature	Case
1		0  ml	2.85	WA	pH=1/2(Pka –logC)
2	Volume	5 ml	4.22	ABS	pH=(Pka +log [S]/[A]
3	Taken	10 ml	4.7	ABS	pH=Pka Best Buffer
4	20.0 ml	15 ml	5.17	ABS	pH=(Pka +log [S]/[A]
5	Ka for	19 ml	5.98	ABS	pH=(Pka +log [S]/[A]
**6	CH3COOH	20 ml	8.7	SH	pH=7+1/2(Pka+logC)
7	2* 10^-10	21 ml	11.39	SB	NbVb - NaVa=NrVr
8		25 ml	12.04	SB	[OH-]= Nr
9		30 ml	12.3	SB	Strong base
10					Remains present

 

In titration of any weak acid with strong base, The pH at equivalent point will be greater than “7”

TITRATIONS OF DIPROTIC ACID WITH STRONG BASE:

The thermodynamics equilibrium constant Kp for the homogeneous gaseous reaction is 10^-3. The standard Gibb's free energy change ∆G° for the reaction at 27°C. (Use R= 2 cal K ^−1 mol ^−1) is :

Calculate the pH of 1.0×10^−3 M sodium phenolate NaOC6​H5​ . Ka​ for C6​H5​OH is 1×10^−10 .

ΔG^ o at 25^°C for the reaction 1/2N2(g) + 3/2H2(g) ⇋ 2NH3(g) is -11.392 kj mole^-1. Hence thermodynamics equilibrium constant is : he equilibrium constant for reaction is 10. (Use R=8.3 JK ^−1 mol ^−1)

Answer key : 10^2