Given that the equilibrium constant for the reaction,
2SO2(g) + O2(g) $$\rightleftharpoons$$ 2SO3(g) has a value of 278 at a particular temperature. What is the value of the equilibrium constant for the following reaction at the same temperature ?
SO3(g) $$\rightleftharpoons$$ SO2(g) + $${1 \over 2}$$ O2(g)
Given the reaction between 2 gases represented by A2 and B2 to give the compound AB(g),
A2(g) + B2(g) $$\rightleftharpoons$$ 2AB(g)
At equilibrium, the concentration of
A2 = 3.0 $$ \times $$ 10$$-$$3 M, of B2 = 4.2 $$ \times $$ 10$$-$$3 M, of AB = 2.8 $$ \times $$ 10$$-$$3 M
If the reaction takes place in a sealed vessel at 527oC, then the value of Kc will be
Equimolar solutions of the following substances were prepared separately. Which one of these will record the highest pH value ?
A
BaCl2
B
AlCl3
C
LiCl
D
BeCl2
Explanation
All of the given salts have same anion i.e., Cl
which on hydrolysis gives HCl which is a strong
acid.
Now, among the salts which have cation that
gives a strongest base on hydrolysis of salt have
the highest pH value. As Ba form Ba(OH)2 which
is a stronger base thus, it results in the highest pH
value.
4
AIPMT 2012 Prelims
MCQ (Single Correct Answer)
pH of a saturated solution of Ba(OH)2 is 12. The value of solubility product (Ksp) of Ba(OH)2 is
A
3.3 $$ \times $$ 10$$-$$7
B
5.0 $$ \times $$ 10$$-$$7
C
4.0 $$ \times $$ 10$$-$$6
D
5.0$$ \times $$ 10$$-$$6
Explanation
Ba(OH)2
⇌
Ba2+
+
2OH
At equilibrium
x
2x
pH = – log[H+]
12 = – log [H+]
$$ \Rightarrow $$ [H+] = 10–12
As, [H+][OH–
] = 10–14
10–12 [OH–
] = 10–14
$$ \Rightarrow $$ [OH–
] = 10–2
As [OH–
] = 2x = 10–2 then x = 5.0 × 10–3
Now, Ksp = [Ba2+][OH–
]2
Ksp = (5 × 10–3) (10–2)2
= 5.0 × 10–7
Questions Asked from Equilibrium
On those following papers in MCQ (Single Correct Answer)
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