The solubility product of Pbl₂ is 8.0 × 10^–9 . The solubility of lead iodide in 0.1 molar solution of lead nitrate is x × 10^–6 mol/L. The value of x is:

(Rounded off to the nearest integer)$\text{\hspace{0.17em}[Given:\hspace{0.17em}}\sqrt{2}=1.41\text{\hspace{0.17em}]\hspace{0.17em}}$

1.	154	2.	423
3.	282	4.	141

Arrange the following solution in the decreasing order of pOH :

(A). 0.01 M HCl

(B). 0.01 M NaOH

(C). 0.01 M ${\mathrm{CH}}_3\mathrm{COONa}$

(D). 0.01 M NaCl

1. (B) > (C) > (D) > (A)

2. (A) > (C) > (D) > (B)

3. (B) > (D) > (C) > (A)

4. (A) > (D) > (C) > (B)

The correct expression for the following reaction is:

Fe₂N_(s) + \(\frac{3}{2}\)H_2(g) \(\leftrightharpoons \) 2Fe_(s) + NH_3(g)

The variation of the equilibrium constant with temperature is given below :

Temperature               Equilibrium Constant

${\mathrm{T}}_1=25°\mathrm{C}$                   ${\mathrm{K}}_1=100$

${\mathrm{T}}_2=100°\mathrm{C}$                 ${\mathrm{K}}_2=100$

The values of $∆\mathrm{H}°,<mspace\; width="1em"></mspace>∆\mathrm{G}°<mspace\; width="1em"></mspace>\mathrm{at}<mspace\; width="1em"></mspace>{\mathrm{T}}_1<mspace\; width="1em"></mspace>\mathrm{and}<mspace\; width="1em"></mspace>∆\mathrm{G}°<mspace\; width="1em"></mspace>\mathrm{at}<mspace\; width="1em"></mspace>{\mathrm{T}}_{2<mspace\; width="1em"></mspace>}\left(\mathrm{in}<mspace\; width="1em"></mspace>\mathrm{kJ}<mspace\; width="1em"></mspace>{\mathrm{mol}}^{-1}\right)$ respectively are close to: [use R=8.314 ${\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1}$]

1. 28.4, -7.14 and -5.71

2. 0.64, -7.14 and -5.71

3. 0.64, -5.71 and -14.29

4. 28.4, -5.71 and -14.29

Given that the equilibrium constant (K_C) at 800 K for the reaction \(N_2(𝑔)+3H_2(𝑔)⇋2NH_3(𝑔)\) is 64. What is the equilibrium constant K_C at the same temperature for the reaction \(NH_3(g) ⇌ \dfrac{1}{2}N_2(g) + \dfrac{3}{2}H_2(g)\)?

Find the molar solubility of AB₂ in pure water, given:

Kₛₚ = 3.20 × 10⁻¹¹

Assume that neither ion reacts with water.

1. 2 × 10^-4 mol L^-1

2. 4 × 10^-4 mol L^-1

3. 6 × 10^-4 mol L^-1

4. 8 × 10^-4 mol L^-1

The pH of an ammonium phosphate solution, if the pK_a of phosphoric acid and the pK_b of ammonium
hydroxide are 5.23 and 4.75 respectively, is:

The \(p K_a\) of a weak acid (HA) and \(p K_b\) of a weak base (BOH) are 3.2 and 3.4, respectively.
The pH of their salt (AB) solution is:

1. 7.0

2. 1.0

3. 7.2

4. 6.9

Given that the pH of a 0.1 M solution of acid HQ is 3, the ionization constant \(K_a\) of the acid is:

If the equilibrium constant \(\left(K_c\right)\) for the reaction \(\mathrm{N}_2(\mathrm{g})+\mathrm{O}_2(\mathrm{g}) \rightarrow 2 \mathrm{NO}(\mathrm{g})\) at temperature \(T\) is \(4 \times10^{-4}\) then what will be the value of \(K_c\) for the reaction, \(\mathrm{NO}(\mathrm{g}) \rightarrow \frac{1}{2} \mathrm{N}_2(\mathrm{g})+\frac{1}{2} \mathrm{O}_2(\mathrm{g})\) ?

1. \(2.5 \times10^{2}\)
2. \(4 \times10^{-4}\)
3. \(50.0\)
4. \(0.02\)