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**Question 1: The Ksp of Ag _{2}CrO_{4 }is 1.1 ×10^{–12} at 298K. The solubility (in mol/L) of Ag_{2}CrO_{4} in a 0.1M AgNO_{3} solution is (IIT-JEE- 2013)**

Ag

Let the concentration of CrO

K

or

1.1´10

or

X = 1.1×10

Hence, the correct option is B.

**Question 2: Solubility product constant (K _{SP}) of salts of type MX, MX_{2} and M_{3}X at temperature “T” are 4.0×10^{-8}, 3.2×10^{-14} and 2.7×10^{-15}, respectively. Solubilities (mol dm^{-3}) of the salts at temperature ‘T’ are (IIT JEE -2008)**

(b) M

(c) MX

(d) MX >M

MX → M

Ksp = [M

Here [M

So, Ksp =[M

or

[M

MX

Ksp = [M

Here 2[M

So, Ksp =4[M

or

[M

M

Ksp = [M

Here [M

So, Ksp =27[X

or

[X

or

[X

So, order of the solubilies is

MX >M

Hence, the correct option is D.

**Question 3: In the following equilibrium, N _{2}O_{4}(g)↔ NO_{2}(g) When 5 moles of each are taken, the temperature is kept at 298 K the total pressure was found to be 20 bar. Given that**

(i) Given that, P total = P (N

But at equilibrium, P (N

So, P (N

Now

For the equilibrium reaction,

N

Q = [P (NO

Now,

ΔG

So,

ΔG = ΔG

= -5706 J = -5.706 kJ

(ii) Negative value of ΔG indicates that reaction is spontaneous one and it will shift in forward direction.

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