1
AIPMT 2012 Prelims
MCQ (Single Correct Answer)
+4
-1
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
2
AIPMT 2012 Prelims
MCQ (Single Correct Answer)
+4
-1
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
3
AIPMT 2012 Prelims
MCQ (Single Correct Answer)
+4
-1
Buffer solutions have constant acidity and alkalinity because
A
these give unionised acid or base on reaction with added acid or alkali
B
acids and alkalies in these solutions are shielded from attack by other ions
C
they have large excess of H+ or OH$$-$$ ions
D
they have fixed value of pH
4
AIPMT 2011 Mains
MCQ (Single Correct Answer)
+4
-1
In qualitative analysis, the metals of group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains Ag+ and pb2+ at a concentration of 0.10 M. Aqueous HCl is added to this solution until the Cl$$-$$ concentration is 0.10 M. What will the concentrations of Ag+ and Pb2+ be at equilibrium ?

(Ksp for AgCl = 1.8 $$ \times $$ 10$$-$$10, Ksp for PbCl2 = 1.7 $$ \times $$ 10$$-$$5)
A
[Ag+] = 1.8 $$ \times $$ 10$$-$$7 M, [Pb2+] = 1.7 $$ \times $$ 10$$-$$6 M
B
[Ag+] = 1.8 $$ \times $$ 10$$-$$11 M, [Pb2+] = 8.5 $$ \times $$ 10$$-$$5 M
C
[Ag+] = 1.8 $$ \times $$ 10$$-$$9 M, [Pb2+] = 1.7 $$ \times $$ 10$$-$$3 M
D
[Ag+] = 1.8 $$ \times $$ 10$$-$$11 M, [Pb2+] = 1.7 $$ \times $$ 10$$-$$4 M
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