Equilibrium Tes...

For the following equilibrium
$${\text{N}}{{\text{H}}_{\text{4}}}{\text{HS}}\left( {\text{s}} \right) \rightleftharpoons {\text{N}}{{\text{H}}_{\text{3}}}\left( {\text{g}} \right){\text{ + }}{{\text{H}}_{\text{2}}}{\text{S}}\left( {\text{g}} \right)$$; partial pressure of $${\text{N}}{{\text{H}}_{\text{3}}}$$ will increase

For $$N{H_4}H{S_{\left( s \right)}} \to N{H_{3\left( g \right)}} + {H_2}{S_{9\left( g \right)}},{K_p} = 100\,at{m^2}$$, equilibrium pressure equals to:

The correct order of equilibrium constant for the reactions is:
$$H_2CO+H_2O\quad \begin{matrix} { K }_{ 1 } \\ { \rightleftharpoons  } \end{matrix}\quad H_2C(OH)_2$$

 Which buffer solution has maximum $$pH?$$ 

At 298 K $$0.01 M\ { NH }_{ 4 }OH$$ solution is $$4.3\%$$ ionised.The ionization constant of $${ NH }_{ 4 }OH $$ is :

Solubility of silver cyanide is maximum in

At $$100^\circ C$$, value of $$K_{w}$$ is 

$$As_2S_3$$ solution has negative charge, capacity to precipitate is highest in:

If the pressure of $$N_2/H_2$$ mixture in a closed apparatus is 100 atm and 20% of the mixture reacts,then the pressure at same temperature would be:

Calculate the degree of ionization of 0.04M HOCl solution having ionization constant $$1.25\times { 10 }^{ -4 }$$?