The solubility product for a salt of type AB is $4×{10}^{-8}$.  The molarity of its standard solution will be:
1. $2×{10}^{-4}$ $\mathrm{mol}/\mathrm{L}$

2. $16×{10}^{-16}$ $\mathrm{mol}/\mathrm{L}$

3. $2×{10}^{-16}$ $\mathrm{mol}/\mathrm{L}$

4. $4×{10}^{-4}$ $\mathrm{mol}/\mathrm{L}$

Subtopic:  Solubility Product |
80%
From NCERT
NEET - 2020
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The solubility of $\mathrm{Ni}{\left(\mathrm{OH}\right)}_{2}$ in 0.1 M NaOH is:

Ksp ($\mathrm{Ni}{\left(\mathrm{OH}\right)}_{2}$)= 2x ${10}^{-15}$

1. 2 x ${10}^{-8}$ M.

2. 1 x ${10}^{-13}$ M

3. 1 x ${10}^{8}$

4. 2 x ${10}^{-13}$

Subtopic:  Solubility Product |
69%
From NCERT
NEET - 2020
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At room temperature, MY and NY3, two nearly insoluble salts, have the same Ksp values of 6.2 × 10-13. The true statement regarding MY and NY3 is:

 1 The molar solubility of MY in water is less than that of NY3. 2 The salts MY and NY3 are more soluble in 0.5 M KY than in pure water. 3 The addition of the salt of KY to a solution of MY and NY3 will have no effect on their solubilities. 4 The molar solubilities of MY and NY3 in water are identical.

Subtopic:  Solubility Product |
68%
From NCERT
NEET - 2016
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The minimum volume of water required to dissolve 1g of calcium sulphate at 298 K is

(For CaSO4Ksp is 9.1 × 10–6)

1. 1.22 L

2. 0.69 L

3. 2.44 L

4. 1.87 L

Subtopic:  Solubility Product |
67%
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The solubility of BaSO4 in water is $2.42$ $×$ ${10}^{-3}$ g/ litre at 298 K. The value of the solubility product will be: (Molar mass of BaSO4 = 233 gmol–1)

 1 1.08 × 10–10 mol2 L–2 2 1.08 × 10–12 mol2 L–2 3 1.08 × 10–14 mol2 L–2 4 1.08 × 10–8 mol2 L–2
Subtopic:  Solubility Product |
61%
From NCERT
NEET - 2018
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The Ksp of Ag2CrO4 and AgBr is 1.1 × 10–12 and 5.0 × 10–13 respectively.

The molarity ratio of saturated solutions of Ag2CrO4 and AgBr will be:

 1 91.9 2 108.6 3 56.9 4 76.9
Subtopic:  Solubility Product |
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