What is the pH of the NaOH solution when 0.04 g of it dissolved in water and made to 100 mL solution?

• 2

• 1

• 13

• 12

Which one of the following is correct with respect to basic character?

• P(CH₃)₃ > PH₃

• PH₃ > P(CH₃)₃

• PH₃ > NH₃

• PH₃ = NH₃

If the ionc product of Ni(OH)₂ is 1.9× 10^-15, the molar solubility of Ni(OH)₂ in 1.0 M NaOH

• 1.9 × 10^-18 M

• 1.9 × 10^-13 M

• 1.9 × 10^-15 M

• 1.9 × 10^-15 M

40 mL of x M KMnO₄ solution is required to react completely with 200 mL of 0.02 M oxalic acid solution in acidic medium. The value of x is

• 0.04

• 0.01

• 0.03

• 0.02

At 400 K, in a 1.0 L vessel, N₂O is allowed to attain equilibrium, N₂O₄ (g) $\rightleftharpoons$ 2NO₂ (g)

At equilibrium, the total pressure is 600 mm Hg, when 20% of N₂O₄ is dissociated. The value of K_P for the reaction is

• 50

• 100

• 150

• 200

In which of the following salts, only cationic hydrolysis is involved?

• CH₃COONH₄

• CH₃COONa

• NH₄Cl

• Na₂SO₄

The slope of the graph drawn between ln k and $\frac{1}{\mathrm{T}}$ as per Arrhenius equation gives the value (R = gas constant; E_a = Activation energy)

• $\frac{\mathrm{R}}{{\mathrm{E}}_{\mathrm{a}}}$

• $\frac{{\mathrm{E}}_{\mathrm{a}}}{\mathrm{R}}$

• $-\frac{{\mathrm{E}}_{\mathrm{a}}}{\mathrm{R}}$

• $\frac{-\mathrm{R}}{{\mathrm{E}}_{\mathrm{a}}}$

$$\begin{gathered} \left(\mathrm{i}\right) {\mathrm{H}}_3{\mathrm{PO}}_4\left(\mathrm{aq}\right) \rightleftharpoons {\mathrm{H}}^{+} \left(\mathrm{aq}\right) + {\mathrm{H}}_2{\mathrm{PO}}_4^{-}\left(\mathrm{aq}\right) \\ \left(\mathrm{ii}\right) {\mathrm{H}}_2{\mathrm{PO}}_4^{-}\left(\mathrm{aq}\right) \rightleftharpoons {\mathrm{H}}^{+} \left(\mathrm{aq}\right) + {\mathrm{HPO}}_4^{2-} \left(\mathrm{aq}\right) \\ \left(\mathrm{iii}\right) {\mathrm{HPO}}_4^{2-} \left(\mathrm{aq}\right) \rightleftharpoons {\mathrm{H}}^{+}\left(\mathrm{aq}\right) + {\mathrm{PO}}_4^{3-}\left(\mathrm{aq}\right) \end{gathered}$$

The equilibrium constants for the above reactions at a certain temperature are K₁, K₂ and K₃ respectively. The equilibrium constant for the reaction ${\mathrm{H}}_3{\mathrm{PO}}_4\left(\mathrm{aq}\right) \rightleftharpoons 3{\mathrm{H}}^{+}\left(\mathrm{aq}\right) + {\mathrm{PO}}_4^{3-} \left(\mathrm{aq}\right)$ in terms of K₁, K₂ and K₃ is 

• K₁+ K₂ + K₂

• $\frac{{\mathrm{K}}_1}{{\mathrm{K}}_2+{\mathrm{K}}_3}$

• $\frac{{\mathrm{K}}_3}{{\mathrm{K}}_1{\mathrm{K}}_2}$

• K₁K₂K₃

The equilibrium constant (K_c) for the following equilibrium $2{\mathrm{SO}}_2\left(\mathrm{g}\right) + {\mathrm{O}}_2\left(\mathrm{g}\right) \rightleftharpoons 2{\mathrm{SO}}_3\left(\mathrm{g}\right)$ at 563 K is 100. At equilibrium, the number of moles of SO₃ in the 10 litre flask is twice the number of moles of SO₂ , then the number of moles of oxygen is

• 0.4

• 0.3

• 0.2

• 0.1

The relation between K_p and K_c is correctly shown as

• K_c = K_p (RT)${}^{∆{\mathrm{n}}_{\mathrm{g}}}$

• K_p = K_c (RT)${}^{-∆{\mathrm{n}}_{\mathrm{g}}}$

• K_p = K_c (RT)${}^{∆{\mathrm{n}}_{\mathrm{g}}}$

• K_c = K_p (RT)${}^{-∆{\mathrm{n}}_{\mathrm{g}}}$