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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When equal volumes of 0.002 M solutions of sodium iodate and cupric chlorate are mixed together (Ksp  (cupric iodate) = 7.4 × 10–8 ), from the following, the correct observation would be :

 1 Precipitation will occur 2 Precipitation will not occur 3 There are 50 % chances of precipitation 4 Data is not sufficient to make any conclusive observation

Subtopic:  Solubility Product |
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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 |
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The maximum concentration of equimolar solutions, of ferrous sulphate and sodium sulphide, so that when mixed in equal volumes, there is no precipitation of iron sulphide, will be:

(For iron sulphide, Ksp = 6.3 × 10–18).

$1.$ $5.02$ $×{10}^{-9}$ $\mathrm{M}$

$2.$ $5.02$ $×$ ${10}^{9}$ $\mathrm{M}$

$3.$ $2.$ $25$ $×$ ${10}^{-13}$ $\mathrm{M}$

$4.$ $\mathrm{Can}\text{'}\mathrm{t}$ $\mathrm{predict}$

Subtopic:  Solubility Product |
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If the solubility product of CuS is 6 × 10–16, the maximum molarity of CuS in an aqueous solution will be:
1. 1.45 × 10−8 mol L−1
2. 3.45 × 10−8 mol L−1
3. 2.45 × 10−8 mol L−1
4. 4.25 × 10−8 mol L−1

Subtopic:  Solubility Product |
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The ionization constant of benzoic acid is 6.46×105 and Ksp for silver benzoate is 2.5×10–13. Silver benzoate is x times more soluble in a buffer of pH 3.19 compared to its solubility in pure water. The value of x will be:

1. 6.8

2. 16.8

3. 33.3

4.  3.3

Subtopic:  Solubility Product |
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The solubility product of silver chromate is $1.1×{10}^{-12}$. The solubility of silver chromate will be:

1. $6.5×{10}^{-5}\mathrm{mol}$ ${\mathrm{L}}^{-1}$

2. $6.5×{10}^{-6}\mathrm{mol}$ ${\mathrm{L}}^{-1}$

3. $5.5×{10}^{-5}\mathrm{mol}$ ${\mathrm{L}}^{-1}$

4. $5.5×{10}^{-6}\mathrm{mol}$ ${\mathrm{L}}^{-1}$

Subtopic:  Solubility Product |
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The solubility product of mercurous iodide is $4.5×{10}^{-29}$. The solubility of mercurous iodide will be:

1. $6.5×{10}^{-7}\mathrm{mol}$ ${\mathrm{L}}^{-1}$

2. $4.09×{10}^{-8}\mathrm{mol}$ ${\mathrm{L}}^{-1}$

3. $4.09×{10}^{-7}\mathrm{mol}$ ${\mathrm{L}}^{-1}$

4. $6.5×{10}^{-8}\mathrm{mol}$ ${\mathrm{L}}^{-1}$

Subtopic:  Solubility Product |
61%
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