1
AIPMT 2005
MCQ (Single Correct Answer)
+4
-1
H2S gas when passed through a solution of cations containing HCl precipitates the cations of second group of qualitative analysis but not those belonging to the fourth group. It is because
A
presence of HCl decreases the sulphide ion concentration
B
solubility product of group II sulphides is more than that of group IV sulphates
C
presence of HCl increases the sulphide ion concentration
D
sulphides of group IV cations are unstable in HCl.
2
AIPMT 2005
MCQ (Single Correct Answer)
+4
-1
At 25oC, the dissociation constant of a base, BOH, is 1.0 $$ \times $$ 10$$-$$12. The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be
A
1.0 $$ \times $$ 10$$-$$5 mol L$$-$$1
B
1.0 $$ \times $$ 10$$-$$6 mol L$$-$$1
C
2.0 $$ \times $$ 10$$-$$6 mol L$$-$$1
D
1.0 $$ \times $$ 10$$-$$7 mol L$$-$$1
3
AIPMT 2004
MCQ (Single Correct Answer)
+4
-1
The solubility product of a sparingly soluble salt AX2 is 3.2 $$ \times $$ 10$$-$$11. Its solubility (in moles/L) is
A
5.6 $$ \times $$ 10$$-$$6
B
3.1 $$ \times $$ 10$$-$$4
C
2 $$ \times $$ 10$$-$$4
D
4 $$ \times $$ 10$$-$$4
4
AIPMT 2004
MCQ (Single Correct Answer)
+4
-1
The rapid change of pH near the stoichiometric point of an acid-base titration is the basis of indicator detection. pH of the solution is related to ratio of the concentrations of the conjugate acid (HIn) and base (In$$-$$) forms of the indicator by the expression
A
$$\log {{\left[ {I{n^ - }} \right]} \over {\left[ {HIn} \right]}} = p{K_{In}} - pH$$
B
$$\log {{\left[ {HIn} \right]} \over {\left[ {I{n^ - }} \right]}} = p{K_{In}} - pH$$
C
$$\log {{\left[ {HIn} \right]} \over {\left[ {I{n^ - }} \right]}} = pH - p{K_{In}}$$
D
$$\log {{\left[ {I{n^ - }} \right]} \over {\left[ {HIn} \right]}} = pH - p{K_{In}}$$
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