Solubility of Ca(OH)₂ is s mol L^-1 . The solubility product (K_sp) under the same condition is : 

1. 4s³ 

2. 3s⁴

3. 4s² 

4. s³

The species, among the following, that act as both Brönsted acid and base is/are:

1. \(H_2PO^-_2 \) 

2.  \(HPO^{2-}_3\)

3. \(HPO^{2-}_4\)

4. All of the above

An aqueous solution of 1M NaCl and 1M HCl is : 

1. not a buffer but pH < 7 

2. not a buffer but pH >7 

3. a buffer with pH <7 

4. a buffer with pH >7 

For the following reaction in gaseous phase \(\mathrm{CO}+\frac{1}{2} \mathrm{O}_{2} \longrightarrow \mathrm{CO}_{2} ; \quad \dfrac {K_{c}}{K_{p}} \text { is : }\)

One of the following equilibria is not affected by change in volume of the flask. The correct option is: 

\(1. \mathrm{PCl}_{5}(g) \rightleftharpoons \mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g)\\ 2. \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)\\ 3. \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g)\\ 4. \mathrm{SO}_{2} \mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{SO}_{2}(g)+\mathrm{Cl}_{2}(g)\)

Find the pH of a 0.005 M solution of calcium acetate, Ca(CH₃COO)₂.
Given: pKa of CH₃COOH = 4.74

Consider the reaction equilibrium :  \(2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{SO}_{3}(g) ; \quad \Delta H^{\circ}=-198 \mathrm{~kJ} \)

On the basis of Le-Chatelier's principle, the condition favorable for the forward reaction is : 

1. lowering of temperature as well as pressure 

2. increasing temperature as well as pressure 

3. lowering the temperature and increasing the pressure 

4. Any value of temperature and pressure 

For the gaseous equilibrium reaction:
\({N_2O_4 (g) \rightleftharpoons 2NO_2 (g)}\), the equilibrium concentrations of \(\mathrm{N_2O_4}\) and \(\mathrm{NO_2}\)​ are \(4.8 \times 10^{-2}\) and \(1.2 \times 10^{-2}\), respectively.

Calculate the value of the equilibrium constant \(K_c\)​ for the reaction:

1. 3.3 \(\times\) 10²  mol L^-1
2. 3 \(\times\) 10^-1  mol L^-1
3. 3 \(\times\) 10^-3  mol L^-1
4. 3 \(\times\) 10³ mol L^-1

The solubility in water of a sparingly soluble salt AB₂ is 1.0 \(\times\) 10^-5 mol L^-1 . Its solubility product will be:

1.   4 \(\times\)10^-15  

2.  4  ^\(\times\) 10^-10  

3.  1 ^\(\times\) 10^-15  

4.  1.0 \(\times\) 10^-10

Which one of the following statements is not true :