1
MCQ (Single Correct Answer)

AIPMT 2002

Reaction BaO2(g) $$\rightleftharpoons$$ BaO(s) + O2(g); $$\Delta $$H = +ve. In equilibrium condition, pressure of O2 depends on
A
increase mass of BaO2
B
increase mass of BaO
C
increase temperature on equilibrium
D
increase mass of BaO2 and BaO both.

Explanation

For the reaction

BaO2(g) $$\rightleftharpoons$$ BaO(s) + O2(g); H = +ve.

At equilibrium Kp = PO2

[For solid and liquids concentration term is taken as unity]

Hence, the value of equilibrium constant depends only upon partial pressure of O2. Further on increasing temperature formation of O2 increases as this is an endothermic reaction.
2
MCQ (Single Correct Answer)

AIPMT 2002

Solubility of MX2 type electrolytes is 0.5 $$ \times $$ 10$$-$$4 mole/lit., then find out Ksp of electrolytes.
A
5 $$ \times $$ 10$$-$$12
B
25 $$ \times $$ 10$$-$$10
C
1 $$ \times $$ 10$$-$$13
D
5 $$ \times $$ 10$$-$$13

Explanation

MX2 Ag2+ + 2X-
s s 2s


Ksp = [M2+] [X]2 = (S)(2S)2 = 4S3

$$ \Rightarrow $$ Ksp = 4(0.5 × 10–4)3 = 5 × 10–13
3
MCQ (Single Correct Answer)

AIPMT 2001

Correct relation between dissociation constants of a dibasic acid is
A
Ka1 = Ka2
B
Ka1 > Ka2
C
Ka1 < Ka2
D
Ka1 = $${1 \over {{K_{{a_2}}}}}$$

Explanation

In polyprotic acids the loss of second proton occurs much less readily than the first. Usually the Ka values for successive loss of protons from these acids differ by at least a factor of 10–3.

$$ \therefore $$ Ka1 > Ka2
4
MCQ (Single Correct Answer)

AIPMT 2001

Solubility of M2S salt is 3.5 $$ \times $$ 10$$-$$6 then find out solubility product.
A
1.7 $$ \times $$ 10$$-$$6
B
1.7 $$ \times $$ 10$$-$$16
C
1.7 $$ \times $$ 10$$-$$18
D
1.7 $$ \times $$ 10$$-$$12

Explanation

M2S ⇌ 2M+ + S2–

Ksp = [M+]2[S2–] = (2s)2(s) = 4s 3

Ksp = 4(3.5 × 10–6)3 = 1.7 × 10–16

EXAM MAP

Joint Entrance Examination

JEE Advanced JEE Main

Medical

NEET

Graduate Aptitude Test in Engineering

GATE CSE GATE ECE GATE ME GATE PI GATE EE GATE CE GATE IN