AIPMT 2011 Mains | Ionic Equilibrium Question 33 | Chemistry

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 ?

(K_sp for AgCl = 1.8 $$ \times $$ 10^$$-$$10, K_sp for PbCl₂ = 1.7 $$ \times $$ 10^$$-$$5)

[Ag⁺] = 1.8 $$ \times $$ 10^$$-$$7 M, [Pb²⁺] = 1.7 $$ \times $$ 10^$$-$$6 M

[Ag⁺] = 1.8 $$ \times $$ 10^$$-$$11 M, [Pb²⁺] = 8.5 $$ \times $$ 10^$$-$$5 M

[Ag⁺] = 1.8 $$ \times $$ 10^$$-$$9 M, [Pb²⁺] = 1.7 $$ \times $$ 10^$$-$$3 M

[Ag⁺] = 1.8 $$ \times $$ 10^$$-$$11 M, [Pb²⁺] = 1.7 $$ \times $$ 10^$$-$$4 M

AIPMT 2011 Prelims

MCQ (Single Correct Answer)

-1

A buffer solution is prepared in which the concentration of NH₃ is 0.30 M and the concentration of NH⁺₄ is 0.20 M. If the equilibrium constant, K_b for NH₃ equals 1.8 $$ \times $$ 10^$$-$$5, what is the pH of this solution? (log 2.7 = 0.43)

9.08

9.43

11.72

8.73

AIPMT 2011 Prelims

MCQ (Single Correct Answer)

-1

Which of the following is least likely to behave as Lewis base?

H₂O

NH₃

BF₃

OH^$$-$$

AIPMT 2010 Prelims

MCQ (Single Correct Answer)

-1

If pH of a saturated solution of Ba(OH)₂ is 12, the value of its K_sp is

4.00 $$ \times $$ 10^$$-$$6 M³

4.00 $$ \times $$ 10^$$-$$7 M³

5.00 $$ \times $$ 10^$$-$$6 M³

5.00$$ \times $$ 10^$$-$$7 M³

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