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 $$\mathrm{AgCl}=10^{-10}$$ )
1. $$10^{-4}$$
2. $$10^{-6}$$
3. $$10^{-9}$$
4. $$10^{-5}$$
Subtopic:  Solubility Product |
From NCERT
NEET - 2024
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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:
1. $$2.0 \times 10^{-8} M$$
2. $$0.5 \times 10^{-8} M$$
3. $$1.5 \times 10^{-8} M$$
4. $$1.0 \times 10^{-8} M$$

Subtopic:  Solubility Product |
81%
From NCERT
NEET - 2022
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Given that the ionic product of $\mathrm{Ni}{\left(\mathrm{OH}\right)}_{2}$ is 2 × .
The solubility of $\mathrm{Ni}{\left(\mathrm{OH}\right)}_{2}$ in 0.1 M NaOH is ;

 1 2 × ${10}^{-8}$ M 2 1 × ${10}^{-13}$ M 3 1 × ${10}^{8}$ M 4 2 × ${10}^{-13}$ M
Subtopic:  Solubility Product |
69%
From NCERT
NEET - 2020
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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 molar solubility of ${\mathrm{CaF}}_{2}$ $\left({\mathrm{K}}_{\mathrm{sp}}=5.3$ $\mathrm{×}$ ${10}^{-11}\right)$ in 0.1 M solution of NaF will be:

 1 $5.3$ $\mathrm{×}$ ${10}^{-11}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$ 2 $5.3$ $\mathrm{×}$ ${10}^{-8}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$ 3 $5.3$ $\mathrm{×}$ ${10}^{-9}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$ 4 $5.3$ $\mathrm{×}$ ${10}^{-10}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$
Subtopic:  Solubility Product |
65%
From NCERT
NEET - 2019
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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 concentration of Ag+ ions in a saturated solution of Ag2C2Ois 2.2 × 10–4 mol L–1.
The solubility product of Ag2C2O4 is:

 1 2.66×10–12 2 4.5×10–11 3 5.3×10–12 4 2.42×10–8
Subtopic:  Solubility Product |
60%
From NCERT
NEET - 2017
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The solubility of AgCl (s) with solubility product 1.6×1010 in 0.1 M NaCl solution would be?

 1 1.26 × 10–5 M 2 1.6 × 10–9 M 3 1.6 × 10–11 M 4 zero
Subtopic:  Solubility Product |
82%
From NCERT
NEET - 2016
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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 Ksp 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 ${\mathrm{AgNO}}_{3}$ solution is added to the solution containing equal moles of NaCl, NaBr, Nal, and Na2CrO4?

1. Agl

2. AgCl

3. AgBr

4. Ag2CrO4

Subtopic:  Solubility Product |
52%
From NCERT
NEET - 2015
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