Solubility Equilibria of Sparingly Soluble Salts
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CHXI07:EQUILIBRIUM

314952 The product of ionic concentration in a saturated solution of an electrolyte at a given temperature is constant and is known as

1 Ionic product of the electrolyte
2 Solubility product
3 Ionization constant
4 Dissociation constant
CHXI07:EQUILIBRIUM

314970 Consider the following sparingly soluble salts having same solubility product in their saturated solution in water:
(A) \({\text{XY}}\)
(B) \(\mathrm{X}_{2} \mathrm{Y}\)
(C) \(\mathrm{XY}_{3}\)
The correct order of increasing solubility of these salts in water will be

1 A \( < \) B \( < \) C
2 C \( < \) B \( < \) A
3 B \( < \) A \( < \) C
4 B \( < \) C \( < \) A
CHXI07:EQUILIBRIUM

314953 What is the minimum volume of water required to dissolve \(1 \mathrm{~g}\) of calcium sulphate at \(298 \mathrm{~K}\) ? (For calcium sulphate, \({{\rm{K}}_{{\rm{sp}}}}\) is \(9.1 \times 10^{-6}\) )?

1 \(5.43 \mathrm{~L}\)
2 \(2.43 \mathrm{~L}\)
3 \(8.43 \mathrm{~L}\)
4 \(7.43 \mathrm{~L}\)
CHXI07:EQUILIBRIUM

314954 The correct representation for solubility product of \(\mathrm{SnS}_{2}\) is

1 \(\left[\mathrm{Sn}^{4+}\right]\left[\mathrm{S}^{2-}\right]^{2}\)
2 \(\left[\mathrm{Sn}^{4+}\right]\left[\mathrm{S}^{2-}\right]\)
3 \(\left[\mathrm{Sn}^{4+}\right]\left[2 \mathrm{~S}^{2-}\right]\)
4 \(\left[\mathrm{Sn}^{4+}\right]\left[2 \mathrm{~S}^{2-}\right]^{2}\)
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CHXI07:EQUILIBRIUM

314952 The product of ionic concentration in a saturated solution of an electrolyte at a given temperature is constant and is known as

1 Ionic product of the electrolyte
2 Solubility product
3 Ionization constant
4 Dissociation constant
CHXI07:EQUILIBRIUM

314970 Consider the following sparingly soluble salts having same solubility product in their saturated solution in water:
(A) \({\text{XY}}\)
(B) \(\mathrm{X}_{2} \mathrm{Y}\)
(C) \(\mathrm{XY}_{3}\)
The correct order of increasing solubility of these salts in water will be

1 A \( < \) B \( < \) C
2 C \( < \) B \( < \) A
3 B \( < \) A \( < \) C
4 B \( < \) C \( < \) A
CHXI07:EQUILIBRIUM

314953 What is the minimum volume of water required to dissolve \(1 \mathrm{~g}\) of calcium sulphate at \(298 \mathrm{~K}\) ? (For calcium sulphate, \({{\rm{K}}_{{\rm{sp}}}}\) is \(9.1 \times 10^{-6}\) )?

1 \(5.43 \mathrm{~L}\)
2 \(2.43 \mathrm{~L}\)
3 \(8.43 \mathrm{~L}\)
4 \(7.43 \mathrm{~L}\)
CHXI07:EQUILIBRIUM

314954 The correct representation for solubility product of \(\mathrm{SnS}_{2}\) is

1 \(\left[\mathrm{Sn}^{4+}\right]\left[\mathrm{S}^{2-}\right]^{2}\)
2 \(\left[\mathrm{Sn}^{4+}\right]\left[\mathrm{S}^{2-}\right]\)
3 \(\left[\mathrm{Sn}^{4+}\right]\left[2 \mathrm{~S}^{2-}\right]\)
4 \(\left[\mathrm{Sn}^{4+}\right]\left[2 \mathrm{~S}^{2-}\right]^{2}\)
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CHXI07:EQUILIBRIUM

314952 The product of ionic concentration in a saturated solution of an electrolyte at a given temperature is constant and is known as

1 Ionic product of the electrolyte
2 Solubility product
3 Ionization constant
4 Dissociation constant
CHXI07:EQUILIBRIUM

314970 Consider the following sparingly soluble salts having same solubility product in their saturated solution in water:
(A) \({\text{XY}}\)
(B) \(\mathrm{X}_{2} \mathrm{Y}\)
(C) \(\mathrm{XY}_{3}\)
The correct order of increasing solubility of these salts in water will be

1 A \( < \) B \( < \) C
2 C \( < \) B \( < \) A
3 B \( < \) A \( < \) C
4 B \( < \) C \( < \) A
CHXI07:EQUILIBRIUM

314953 What is the minimum volume of water required to dissolve \(1 \mathrm{~g}\) of calcium sulphate at \(298 \mathrm{~K}\) ? (For calcium sulphate, \({{\rm{K}}_{{\rm{sp}}}}\) is \(9.1 \times 10^{-6}\) )?

1 \(5.43 \mathrm{~L}\)
2 \(2.43 \mathrm{~L}\)
3 \(8.43 \mathrm{~L}\)
4 \(7.43 \mathrm{~L}\)
CHXI07:EQUILIBRIUM

314954 The correct representation for solubility product of \(\mathrm{SnS}_{2}\) is

1 \(\left[\mathrm{Sn}^{4+}\right]\left[\mathrm{S}^{2-}\right]^{2}\)
2 \(\left[\mathrm{Sn}^{4+}\right]\left[\mathrm{S}^{2-}\right]\)
3 \(\left[\mathrm{Sn}^{4+}\right]\left[2 \mathrm{~S}^{2-}\right]\)
4 \(\left[\mathrm{Sn}^{4+}\right]\left[2 \mathrm{~S}^{2-}\right]^{2}\)
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CHXI07:EQUILIBRIUM

314952 The product of ionic concentration in a saturated solution of an electrolyte at a given temperature is constant and is known as

1 Ionic product of the electrolyte
2 Solubility product
3 Ionization constant
4 Dissociation constant
CHXI07:EQUILIBRIUM

314970 Consider the following sparingly soluble salts having same solubility product in their saturated solution in water:
(A) \({\text{XY}}\)
(B) \(\mathrm{X}_{2} \mathrm{Y}\)
(C) \(\mathrm{XY}_{3}\)
The correct order of increasing solubility of these salts in water will be

1 A \( < \) B \( < \) C
2 C \( < \) B \( < \) A
3 B \( < \) A \( < \) C
4 B \( < \) C \( < \) A
CHXI07:EQUILIBRIUM

314953 What is the minimum volume of water required to dissolve \(1 \mathrm{~g}\) of calcium sulphate at \(298 \mathrm{~K}\) ? (For calcium sulphate, \({{\rm{K}}_{{\rm{sp}}}}\) is \(9.1 \times 10^{-6}\) )?

1 \(5.43 \mathrm{~L}\)
2 \(2.43 \mathrm{~L}\)
3 \(8.43 \mathrm{~L}\)
4 \(7.43 \mathrm{~L}\)
CHXI07:EQUILIBRIUM

314954 The correct representation for solubility product of \(\mathrm{SnS}_{2}\) is

1 \(\left[\mathrm{Sn}^{4+}\right]\left[\mathrm{S}^{2-}\right]^{2}\)
2 \(\left[\mathrm{Sn}^{4+}\right]\left[\mathrm{S}^{2-}\right]\)
3 \(\left[\mathrm{Sn}^{4+}\right]\left[2 \mathrm{~S}^{2-}\right]\)
4 \(\left[\mathrm{Sn}^{4+}\right]\left[2 \mathrm{~S}^{2-}\right]^{2}\)
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