NEET Solubility Product Practice Questions With Solutions

NEET Chemistry Solubility Product Practice Questions

Question 1.

The ratio of solubility of $\mathrm{AgCl}$ in $0.1~ \mathrm{M} ~\mathrm{KCl}$ solution to the solubility of $ \mathrm{Ag} \mathrm{Cl}$ in water is:
(Given: Solubility product of $\mathrm{AgCl}=10^{-10}$ )

A$10^{-4}$

B$10^{-6}$

C$10^{-9}$

D$10^{-5}$

Question 2.

The solubility product of $\mathrm{BaSO_4}$ in water is $1.5 \times 10^{-9} $. The molar solubility of $\mathrm{BaSO_4}$ in 0.1 M solution of Ba(NO₃)₂ in:

A$2.0 \times 10^{-8} M$

B$0.5 \times 10^{-8} M$

C$1.5 \times 10^{-8} M$

D$1.0 \times 10^{-8} M$

Question 3.

The molar solubility of

{CaF}_{2}

(K_{sp} = 5.3

\times

10^{- 11})

in 0.1 M solution of NaF will be:

5.3

\times

10^{- 11}

mol

L^{- 1}

5.3

\times

10^{- 8}

mol

L^{- 1}

5.3

\times

10^{- 9}

mol

L^{- 1}

5.3

\times

10^{- 10}

mol

L^{- 1}

Question 4.

The solubility of BaSO₄ in water is

2.42

\times

10^{- 3}

g/ litre at 298 K. The value of the solubility product will be: (Molar mass of BaSO₄ = 233 gmol^–1)

A1.08 × 10^–10 mol² L^–2

B1.08 × 10^–12 mol² L^–2

C1.08 × 10^–14 mol² L^–2

D1.08 × 10^–8 mol² L^–2

Question 5.

The concentration of Ag⁺ ions in a saturated solution of Ag₂C₂O₄is 2.2 × 10^–4 mol L^–1.
The solubility product of Ag₂C₂O₄ is:

A2.66×10^–12

B4.5×10^–11

C5.3×10^–12

D2.42×10^–8

Question 6.

At room temperature, MY and NY₃, two nearly insoluble salts, have the same K_sp values of 6.2 × 10^-13. The true statement regarding MY and NY₃ is:

AThe molar solubility of MY in water is less than that of NY₃.

BThe salts MY and NY₃ are more soluble in 0.5 M KY than in pure water.

CThe addition of the salt of KY to a solution of MY and NY₃ will have no effect on their solubilities.

DThe molar solubilities of MY and NY₃ in water are identical.

Question 7.

The solubility of AgCl (s) with solubility product 1.6×10^–¹⁰ in 0.1 M NaCl solution would be?

A1.26 × 10^–5 M

B1.6 × 10^–9M

C1.6 × 10^–11 M

Dzero

Question 8.

The K_sp of Ag₂CrO₄, AgCl, AgBr, and Agl are respectively, 1.1 × 10^–12, 1.8 × 10^–10, 5.0 × 10^–13, 8.3 × 10^–17. Which one of the following salts will precipitate last if

{AgNO}_{3}

solution is added to the solution containing equal moles of NaCl, NaBr, Nal, and Na₂CrO₄?

AAgl

BAgCl

CAgBr

DAg₂CrO₄

Question 9.

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 concentration of Ag⁺and Pb²⁺ at equilibrium?

(K_sp for AgCl = 1.8 × 10^-10)

(K_sp for PbCl₂ = 1.7 × 10^-5)

$[A g^{+}] = 1.8 \times 10^{- 11}$ $M;$

$[P b^{2 +}] = 1.7 \times 10^{- 4} M$

$[{Ag}^{+}] = 1.8 \times 10^{- 7}$ $M;$

$[P b^{2 +}] = 1.7 \times 10^{- 6} M$

$[{Ag}^{+}] = 1.8 \times 10^{- 11}$ $M;$

$[P b^{2 +}] = 8.5 \times 10^{- 5} M$

$[A g^{+}] = 1.8 \times 10^{- 9}$ $M;$

$[P b^{2 +}] = 1.7 \times 10^{- 3} M$

Question 10.

A saturated solution of Ba(OH)₂ has a pH of 12. The value of its K_sp will be:

4.00 \times 10^{- 6}

M^{3}

4.00 \times 10^{- 7}

M^{3}

5.00 \times 10^{- 6}

M^{3}

5.00 \times 10^{- 7}

M^{3}

Question 1.

The solubility product of a sparingly soluble salt AX₂ is 3.2 ×10^–11. Its solubility (in moles/litre) is:

A3.1×10^–4

B2 × 10^–4

C4 × 10^–4

D5.6 × 10^–6

Question 2.

The solubility product of AgI at 25 ºC is 1.0 × 10^–16 mol² L^–2. The solubility of AgI in 10^–4 N solution of KI at 25 ºC is approximately (in mol L^–1):

1.0 \times 10^{- 16}

1.0 \times 10^{- 12}

1.0 \times 10^{- 10}

1.0 \times 10^{- 8}

Question 3.

If the solubility of MX₂ – type electrolytes is 0.5 × 10^–4 Mole/lit. then K_sp of electrolytes will be:

5 \times 10^{- 12}

25 \times 10^{- 10}

1 \times 10^{- 13}

5 \times 10^{- 13}

Question 4.

If the solubility of a

M_{2} S

salt is

3.5

\times

10^{- 6}

mol litre^-1 , then the solubility product of

M_{2} S

will be:

1.7

\times

10^{- 6}

mol³litre^-3

1.7

\times

10^{- 16}

mol³ litre^-3

1.7

\times

10^{- 18}

mol³ litre^-3

1.7

\times

10^{- 12}

mol³ litre^-3

Question 5.

A compound BA₂ has $K_{sp} = 4\times 10^{-12}$

.

Solubility of this compound will be:

A10^-3

B10^-4

C10^-5

D10^-6

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NEET Solubility Product Practice Questions With Solutions

NEET Chemistry Solubility Product Practice Questions

Question 1.

Question 2.

Question 3.

Question 4.

Question 5.

Question 6.

Question 7.

Question 8.

Question 9.

Question 10.

Question 1.

Question 2.

Question 3.

Question 4.

Question 5.

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