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
2
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
