The pH of an ammonium phosphate solution, if the pK_a of phosphoric acid and the pK_b of ammonium
hydroxide are 5.23 and 4.75 respectively, is:

1.	8	2.	6
3.	7	4.	10

The \(p K_a\) of a weak acid (HA) and \(p K_b\) of a weak base (BOH) are 3.2 and 3.4, respectively.
The pH of their salt (AB) solution is:

1. 7.0

2. 1.0

3. 7.2

4. 6.9

The equilibrium constant (K_c) for the reaction N₂(g) + O₂(g) → 2NO(g) at temperature T is 4 × 10^–4.
The value of K_c for the reaction, 
$\mathrm{NO}\left(\mathrm{g}\right)\to \frac{1}{2}{\mathrm{N}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)$ is:

1. 2.5 × 10²

2. 4 × 10^–4

3. 50.0

4. 0.02

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:

1. 2.0 L

2. 9.0 L

3. 0.1 L

4. 0.9 L

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 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]

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 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 :