For the reaction equilibrium,

2NOBr(g) $\rightleftharpoons$2NO(g) + Br₂(g), if $P_{\mathit{B}{\mathit{r}}_{\mathit{2}}}$ = P/9 at equilibrium and P is total pressure. The ratio of K_p/P is equal to:

1. 1/9               

2. 1/81

3. 1/27               

4. 1/3

In the system, CaF₂(s) $\rightleftharpoons$Ca²⁺ (aq) + 2F^-(aq), increasing the concentration of Ca²⁺ ions 4 times will cause the equilibrium concentration of F^- ions to change to:

1. 1/4 of the initial value

2. 1/2 of the initial value

3. 2 times of the initial value

4. none of the above

The addition of HCl does not suppress the ionization of:

KMnO₄ can be prepared from K₂MnO₄ as per reaction,

 $3{\mathrm{MnO}}_4^{2-}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>2{\mathrm{H}}_2\mathrm{O}<mspace\; width="1em"></mspace>\rightleftharpoons <mspace\; width="1em"></mspace>2{\mathrm{MnO}}_4^{-}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{MnO}}_2<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>4{\mathrm{OH}}^{-}$

The reaction can go to completion by removing OH^- ions by adding             

1. HCl

2. KOH

3. CO₂

4. SO₂

The increasing order of basic strength of Cl^-, ${\mathrm{CO}}_3^{2-}<mspace\; width="1em"></mspace>$, CH₃COO^-, OH^-, F^- is:

1. Cl^-<F^-<CH₃COO^-<${\mathrm{CO}}_3^{2-}<mspace\; width="1em"></mspace>$<OH^-

2.  Cl^-<F^-< ${\mathrm{CO}}_3^{2-}<mspace\; width="1em"></mspace>$<CH₃COO^-<OH^-

3. CH₃COO^-<Cl^-<F^-<${\mathrm{CO}}_3^{2-}<mspace\; width="1em"></mspace>$<OH^-

4. None of the above

If the pressure is applied to the following equilibrium, Liquid $\rightleftharpoons$ Vapour. The boiling temperature of the liquid:

1. will decrease                                 

2. will increase

3. may not change                           

4. will not change

Which of the following statements is not true?

1. The pH of 10^-8 N HCl is 8.

2. 96500 coulomb of electricity is passed through a CuSO₄ solution deposit 1g of equivalent of Cu at cathode.

3. The conjugate base of H₂P${\mathrm{O}}_4^{-}$ is HP${\mathrm{O}}_4^{2-}$.

4. pH + pOH = 14 for all aqueous solution.

In which of the following will the solubility of AgCl be the minimum?

Which of the following salts will give the highest pH in the water?                   

1. KCl           

2. NaCl         

3. Na₂CO₃     

4. CuSO₄

The aqueous solution having the lowest pH:

1. NaOH                 

2. NH₄Cl

3. Na₂CO₃             

4. NaCl