Solubility Pr...

Solubility Product

Trending Questions

Q. The solubility of

P b C l_{2}

in water is

0.01 M a t 25^{\circ} C

. Its maximum concentration in

0.1 M N a C l

will be:

$2 \times 10^{- 3} M$
$1 \times 10^{- 4} M$
$1.6 \times 10^{- 2} M$
$4 \times 10^{- 4} M$

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Q. Enthalpy of solution of

N a O H

(solid ) in water is

- 41.6 k J m o l^{- 1}

. When

N a O H

is dissolved in water, the temperature of water

Decreases
Does not change
Fluctuates indefinitely
Increase

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Which is the correct representation of the solubility product constant

$A g_{2} C r O_{4}$ of

[Ag⁺]² [CrO₄^2-]
[Ag⁺] [CrO₄^2-]
[2Ag⁺] [CrO₄^2-]
[2Ag⁺]² [CrO₄^2-]

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Q. The

p H

of a solution obtained by mixing

100 m L

0.2 M

C H_{3} C O O H

with

100 m L

0.2 M N a O H

will be: (

p K_{a} f o r C H_{3} C O O H = 4.74

)

4.74
8.87
9.1
8.87

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Q. Equal volume of

0.02 M

A g N O_{3}

and

0.02 M H C N

were mixed. Calculate

[A g^{+}]

at equilibrium assuming no cynao-complex formation.
Given :

K_{s p} (A g C N) = 2.2 \times 10^{- 16}, K_{a} (H C N) = 6.2 \times 10^{- 10} .

$2.64 \times 10^{- 4} M$
$3.69 \times 10^{- 8} M$
$5.9 \times 10^{- 5} M$
$4.64 \times 10^{- 2} M$

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A X_{2}

is a sparingly soluble salt. The solubility product of

A X_{2}

3.2 \times 10^{- 11} .

Find the value of solubility

(s)

m o l L^{- 1}

$2 \times 10^{- 8}$
$2 \times 10^{- 4}$
$8 \times 10^{- 12}$
$2 \times 10^{- 11}$

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Q. A solution which is

10^{- 3} M

each in

M n^{2 +}, F e^{2 +}

and

H g^{2 +}

is treated with

10^{- 16} M

sulphide ion, If

K_{s p}

M n S, F e S, Z n S a n d H g S

are

10^{- 15}, 10^{- 25}, 10^{- 20}

and

10^{- 54}

respectively, which one will precipitate first?

$F e S$
$M n S$
$H g S$
$Z n S$

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Q. Consider a sparingly soluble salt, zirconium phosphate

[Z r_{3} (P O_{4})_{4}]

. If molar solubility of zirconium phosphate is denoted by

s

and its solubility product by

K_{s p}

, then which of the following relationship holds true?

$s = {(\frac{K_{s p}}{144})}^{\frac{1}{7}}$
$s = {(\frac{K_{s p}}{144})}^{7}$
$s = {(\frac{K_{s p}}{6912})}^{\frac{1}{7}}$
$s = {(\frac{K_{s p}}{6912})}^{7}$

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Q. Solubility product

(K_{s p})

values of the following sparingly soluble salts at

25^{\circ} C

is :

Salts

K_{s p}

A g C l 1.8 \times 10^{- 10} A g I 1.1 \times 10^{- 16} P b C r O_{4} 1.8 \times 10^{- 14} A g B r 3.3 \times 10^{- 13}

The least soluble and the most soluble salts respectively are:

$P b C r O_{4}$ and $A g C l$
$A g I$ and $A g C l$
$A g I$ and $P b C r O_{4}$
$A g I$ and $A g B r$

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Q. 32. OCH3 Is electron withdrawing or electron releasing

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Q. If the solubility of

C a F_{2}

in water at

18^{\circ} C

2.05 \times 10^{- 4} m o l L^{- 1}

. Calculate its solubility product at the given temperature.

$3.45 \times 10^{- 11}$
$4.45 \times 10^{- 12}$
$5.45 \times 10^{- 10}$
$6.66 \times 10^{- 9}$

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Q. Which is odd electron specie?(1) CO2(2) NO2(3) SO2(4) SiO2

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Q. Solubility product constant (

K_{s p}

) of salts of types MX,

M X_{2}

and

M_{3} X

at temperature 'T' are

4.0 \times 10^{- 8}, 3.2 \times 10^{- 14}

and

2.7 \times 10^{- 15},

respectively. Solubilities (mol

d m^{- 3}

) fo the salts at temperature 'T' are in the order

$M X > M X_{2} > M_{3} X$
$M_{3} X > M X_{2} > M X$
$M X_{2} > M_{3} X > M X$
$M X > M_{3} X > M X_{2}$

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K_{s p}

C d S = 8 \times 10^{- 27}

K_{s p}

Z n S = 1 \times 10^{- 21}

K_{a}

H_{2} S = 1 \times 10^{- 21}

.
When

Z n S

starts precipitating, what concentration of

C d^{2 +}

is left?

$8 \times 10^{- 7} M$
$0.1 M$
$4 \times 10^{- 10} M$
$2 \times 10^{- 9} M$

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Q. Find the

[H^{+}]

that must be maintained in a saturated

H_{2} S (0.1 M)

to precipitate

C d S

not

Z n S

[C d^{2 +}] = [Z n^{2 +}] = (0.1 M)

initially.

K_{s p} (C d S) = 8 \times 10^{- 27} K_{s p} (Z n S) = 1 \times 10^{- 21} K_{s p} (H_{2} S) = 1.1 \times 10^{- 21}

0.589 M
0.105 M
0.500 M
0.877 M

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Q. Equal volumes of 0.2 M CH3COOH and 0.2 M HCl are mixed. Concentration of CH3COOH in the solution is

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Calculate the solubility of A₂X₃ in pure water, assuming that neither kind of ion reacts with water. The solubility product of A₂X₃, K_sp = 1.1 × 10^-23

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Q. The ionic product of water does not change with temperature.

False
True

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Q. Electron dot structure of P4O7

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Q. How chemical equilibrium is attained?

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Q. What will be the solubility of

C d (C N)_{2}

0.05 M N a C N

solution if the

K_{s p}

1.0 \times 10^{- 8} {mol}^{3} L^{- 3}

C d (C N)_{2} ⇌ C d^{2 +} + 2 C N^{-} N a C N \to N a^{+} + C N^{-}

$1.0 \times 10^{- 6}$
$1.0 \times 10^{- 8}$
$2 \times 10^{- 8}$
$4 \times 10^{- 6}$

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The solubility product of $M g (O H)_{2}$ at $25^{\circ} C$ is $1.4 \times 10^{- 11}$ . The solubility of $M g (O H)_{2}$ in gm per litre is:

$1.4 \times 10^{- 3}$
$2.8 \times 10^{- 3}$
$1.11 \times 10^{- 6}$
$8.7 \times 10^{- 3}$

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Q. Consider a sparingly soluble salt

A B

having solubility as

s m o l L^{- 1}

. What will be the value of

K_{s p}

for

A B

salt.

$s m o l L^{- 1}$
$\sqrt[3]{s} (m o l L^{- 1})^{\frac{1}{3}}$
$\sqrt{s} (m o l L^{- 1})^{0.5}$
$s^{2} (m o l L^{- 1})^{2}$

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Q. If the concentration of

A^{+}

ions in a solution of a sparingly soluble salt,

A B

10^{- 3} M .

Find the concentration of

B^{-}

ions at which the precipitation of

A B

starts.
Given : Solubility product of AB is

1.0 \times 10^{- 8}

$< 10^{- 8} M$
$> 10^{- 5} M$
Between $10^{- 8} M t o 10^{- 7} M$
Between $10^{- 7} M t o 10^{- 8} M$

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$K_{s p} M g (O H)_{2}$ is $4.0 \times 10^{- 12}$ . The number of moles of $M g^{2 +}$ ions in one litre of its saturated solution in 0.1 M NaOH is :

$4.0 \times 10^{- 10}$
$1.0 \times 10^{- 4}$
$2.0 \times 10^{- 6}$
$8.0 \times 10^{- 6}$

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Q. 46. what is 2s2p mixing in MOT does it is the reason due to which above 14 electron sigma 2pz is written before pi

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Q. 15 mL of 0.05 M

A g N O_{3}

is mixed with 45 mL of 0.03 M

K_{2} C r O_{4}

. Then, which of the following is correct regarding

A g_{2} C r O_{4}

K_{s p}

A g_{2} C r O_{4} = 1.9 \times 10^{- 12} .

Precipitation occurs
Precipitation does not occur
Can't be determined from given data
None of these

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Q. Which of the following is

T R U E

$\frac{Q}{K_{s p}} > 1 \Rightarrow$ The solution is unsaturated.
$\frac{Q}{K_{s p}} < 1 \Rightarrow$ The solution is saturated.
$\frac{Q}{K_{s p}} = 1 \Rightarrow$ The solution is saturated.
Both b and c

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Q. If the solubility product of a sparingly soluble salt

L i_{3} P O_{4}

2.7 \times 10^{- 9}

. The concentration

(m o l L^{- 1})

L i^{+}

ions in the saturated solution of the salt is:
Given :

(100)

^{\frac{1}{4}} = 3.16

$3.78 \times 10^{- 9} m o l L^{- 1}$
$2.7 \times 10^{- 9} m o l L^{- 1}$
$3.16 \times 10^{- 3} m o l L^{- 1}$
$9.48 \times 10^{- 3} m o l L^{- 1}$

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Q. The solubility product

(K_{s p})

of the following compounds are given at

25^{\circ} C

. The compound most soluble and least soluble coumpounds are:
Compounds

K_{s p}

A g C l 1.1 \times 10^{- 10} A g I 1.1 \times 10^{- 16} P b C r O_{4} 4.0 \times 10^{- 14} A g_{2} C O_{3} 8.0 \times 10^{- 12}

$A g C l a n d P b C r O_{4}$
$A g_{2} C O_{3} a n d P b C r O_{4}$
$A g_{2} C O_{3} a n d A g I$
$A g C l a n d A g_{2} C O_{3}$

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