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 :

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

The first and second dissociation constants of an acid H₂A are 1.0 × 10^–5 & 5.0 × 10^–10 respectively. The overall dissociation constant of the acid will be :

In aqueous solution, the ionization constants for carbonic acid are
\(K_{1} = 4.2 \times 10^{- 7}\) and \(K_{2} = 4.8 \times 10^{- 11}\)
The correct statement for a saturated 0.034 M solution of the carbonic acid is:

The standard Gibbs energy change at 300 K for the reaction $2\mathrm{A}\rightleftharpoons \mathrm{B}+\mathrm{C}$ is 2494.2 J. At a given time, the composition of the reaction mixture is $\left[\mathrm{A}\right]=\frac{1}{2},<mspace\; width="1em"></mspace>\left[B\right]=2<mspace\; width="1em"></mspace>and<mspace\; width="1em"></mspace>\left[C\right]=\frac{1}{2}$. The reaction proceeds in the:[assume R=8.314 J/K/mol; e^-1 = 0.37]

A vessel at 1000 K contains CO₂ with a pressure of 0.5 atm. Some of the CO₂ is converted into CO on the addition of graphite. If the total pressure at equilibrium is 0.8 atm, the value of K is :

1. 1.8 atm

2. 3 atm

3. 0.3 atm

4. 0.18 atm

The amount of water in litres that must be added to 1 litre of an aqueous solution of HCl with a pH of 1 to create an aqueous solution with pH of 2, is:

If the equilibrium constant \(\left(K_c\right)\) for the reaction \(\mathrm{N}_2(\mathrm{g})+\mathrm{O}_2(\mathrm{g}) \rightarrow 2 \mathrm{NO}(\mathrm{g})\) at temperature \(T\) is \(4 \times10^{-4}\) then what will be the value of \(K_c\) for the reaction, \(\mathrm{NO}(\mathrm{g}) \rightarrow \frac{1}{2} \mathrm{N}_2(\mathrm{g})+\frac{1}{2} \mathrm{O}_2(\mathrm{g})\) ?

1. \(2.5 \times10^{2}\)
2. \(4 \times10^{-4}\)
3. \(50.0\)
4. \(0.02\)