The solubility product of silver bromide is 5.0 x 10^-13. The quantity of potassium bromide (molar mass taken as 120 g mol ⁻¹ ) to be added to 1 litre of 0.05 M solution of silver nitrate to start the precipitation of AgBr is-

1. 5.0 x 10 ⁻⁸ g

2. 1.2 x 10 ⁻¹⁰ g

3. 1.2 x 10^-9 g

4. 6.2 x 10⁻⁵ g

At 25°C, the solubility product of Mg(OH)₂ is 1.0 × 10^-11. At which pH, will Mg²⁺ ions start precipitating in the form of Mg(OH)₂ from a solution of 0.001 M Mg²⁺ ions?

The equilibrium constant at 298 K for a reaction A + B  ⇋ C + D is 100.
If the initial concentration of all the four species were 1 M each, then equilibrium concentration of D (in mol L^–1) will be :

The dissociation of HA is represented by \(\mathrm{HA} \rightleftharpoons \mathrm{H}^{+}+\mathrm{A}^{-}\). Given that the pH of a 1.0 M solution is 5, find the dissociation constant:

The K_sp for Cr(OH)₃ is 1.6x10^-30 . The molar solubility of this compound in water is :

1. $\sqrt{1.6\times {10}^{20}}$

2. $\sqrt[4]{1.6\times {10}^{-30}/27}$

3. $1.6\times {10}^{-30}/27$

4. $\sqrt[2]{1.6\times {10}^{-30}}$

The pK_a of a weak acid HA, is 4.80. The pK_b of a weak base BOH, is 4.78. The pH of an aqueous solution of the corresponding salt, BA, will be: 

1. 4.79

2. 7.01

3. 9.22

4. 9.58

For the three reactions (a, b, and c) listed below, the equilibrium constants are provided:

(a). CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g);  K₁    
(b). CH₄(g) + H₂O(g) ⇌ CO(g) + 3H₂(g); K₂    
(c). CH₄(g) + 2H₂O(g) ⇌ CO₂(g) + 4H₂(g); K₃

Which of the following relations is correct?

1. ${\mathrm{K}}_2{\mathrm{K}}_3={\mathrm{K}}_1$

2. ${\mathrm{K}}_3={\mathrm{K}}_1{\mathrm{K}}_2$

3. ${\mathrm{K}}_3{\mathrm{K}}_2^3={\mathrm{K}}_1^2$

4. ${\mathrm{K}}_1\sqrt{{\mathrm{K}}_2}={\mathrm{K}}_3$

The equilibrium constants, \(\mathrm{Kp}_1 \text { and } \mathrm{Kp}_2\) for the reactions \(\mathrm{X} \rightleftharpoons 2 \mathrm{Y} \text { and } \mathrm{Z} \rightleftharpoons \mathrm{P}+\mathrm{Q},\) are given as 1:9.
Assuming equal degrees of dissociation for both X and Z, what is the ratio of total pressures at equilibrium?

1. 1 : 1

2. 1 : 3

3. 1 : 9

4. 1 : 36

The pKa of a weak acid (HA) is 4.5. The pOH of an aqueous buffered solution of HA in which 50 % of the acid is ionized is:

1. 4.5

2. 2.5

3. 9.5

4. 7.0
 

In a saturated solution of the sparingly soluble electrolyte AgIO₃ (molecular mass = 283) the equilibrium is represented by–
${\mathrm{AgIO}}_3\left(\mathrm{(s)}\right)\rightleftharpoons {\mathrm{Ag}}^{+}\left(\mathrm{(aq)}\right)+<mspace\; width="1em"></mspace>{{\mathrm{IO}}_3}^{-}\left(\mathrm{(aq)}\right)$
If the solubility product constant K_sp of AgIO₃ at a given temperature is 1.0 × 10^-8, Calculate the mass of AgIO₃ contained in 100 ml of its saturated solution.

1. 28.3 × 10^–2 g

2. 2.83 × 10^–3 g

3. 1.0 × 10^–7 g

4. 1.0 × 10^–4 g