4 gm of NaOH is dissolved in 1000 ml of water. The ${\mathrm{H}}^{+}$ ion concentration will be -

The solubility product of a sparingly soluble salt AX₂ is 3.2 ×10^–11. It's solubility (in moles/litre) is:-

A compound BA₂ has \(K_{sp} = 4\times 10^{-12}\)$$; solubility of this compound will be :

For a reaction , ${\mathrm{BaO}}_2\left(\mathrm{s}\right)\rightleftharpoons \mathrm{BaO}\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)$; ∆H = + ve.
At equilibrium condition, pressure of O₂  depends on : -

The compound with highest pH among the following is : -

Solution of 0.1 N NH₄OH and 0.1 N NH₄Cl has pH 9.25. Then pk_b of NH₄OH is : -

A compound among the following that can be classified as not a protonic acid,is  :

The volume of the container containing a liquid and its vapours at a constant temperature is suddenly increased. The effect of the change on vapour pressure would be :

For the following reaction, 

2SO₂(g) + O₂(g) $\leftrightharpoons$2SO₃(g)

The value of K_c at equilibrium with a concentration of [SO₂]= 0.60M,[O₂] = 0.82M and [SO₃] = 1.90M

would be:

Pure liquids and solids are ignored while writing the expression for the equilibrium constant because 

 For a given reaction, 2N_{2 (g)} + O_{2 (g)}  $\leftrightharpoons$2N₂O _(g), if a mixture of 0.482 mol N₂ and 0.933 mol of O₂ is placed in a 10 L vessel and allowed to form N₂O at a temperature for which K_c= 2.0 × 10^–37 L mol^-1, the concentration of N₂O at equilibrium will be -

For a reaction, 2NO _(g) + Br_{2 (g)}  $\leftrightharpoons$2NOBr _(g)

When 0.087 mol of NO and 0.0437 mol of Br₂ are mixed in a closed container at a constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. The concentration of NO and Br₂ at equilibrium will be:

For the reaction: H_{2 (g)} + I_{2 (g)}  $\rightleftharpoons$2HI _(g) ; K_c = 54.8 at 700K .

If 0.5 mol L^–1 of HI_(g) is present at equilibrium at 700 K, the concentration of H_2(g) and I_2(g)  would be:

When the initial concentration of ICl is 0.78 M, what will be the equilibrium concentration of ICl?

2ICl_(g) $\leftrightharpoons$I_2(g) + Cl_2(g); K_c = 0.14

Given the reaction: CH₃COOH _(l) + C₂H₅OH _(l)  $\leftrightharpoons$CH₃COOC₂H_{5 (l)} + H₂O _(l)

At 293 K, if one starts with 1.00 mol of acetic acid and 0.18 mol of ethanol, there is 0.171 mol of ethyl acetate in the final equilibrium mixture. The equilibrium constant of the reaction will be-

(a) PCl_{5 (g)} $\leftrightharpoons$ PCl_{3 (g)} + Cl_{2 (g)}

(b) CaO _(s) + CO_{2 (g)} $\leftrightharpoons$  CaCO_{3 (s)}

(c) 3Fe _(s) + 4H₂O _(g) $\leftrightharpoons$ Fe₃O_{4 (s)} + 4H_{2 (g)}

The effect of an increase in the volume on the number of moles of products in the above-mentioned reactions would be, respectively:

Consider the following reactions.

(i) COCl_{2 (g)}  $\leftrightharpoons$CO _(g) + Cl_{2 (g)}

(ii) CO_{2 (g)} + C _(s) $\leftrightharpoons$ 2CO _(g)

(iii) 2H_{2 (g)} + CO _(g) $\leftrightharpoons$ CH₃OH _(g)

Which reaction(s) shift in a backward manner when the pressure is increased?

Given an endothermic reaction:

CH_{4 (g)} + H₂O _(g)  $\leftrightharpoons$CO _(g) + 3H_{2 (g)}

If the temperature is increased, then 

For the given reaction: 

PCl_{5 (g)}  $\leftrightharpoons$PCl_{3 (g)} + Cl_{2 (g)}, ∆_rH° = 124.0 kJ mol^–1 and K_c = 8.3 $\times$ 10^-3 mol L^-1 at 473 K

The effect on K_c if (i) pressure is increased  and (ii) the temperature is increased will be, respectively-