Given below are two statements:

Assertion (A):	When Cu (II) and sulphide ions are mixed, they react together extremely quickly to give a solid.
Reason (R):	The equilibrium constant of Cu2+(aq) + S2- (aq) ⇋ CuS(s) is high because the solubility product is low.

 

1.	Both (A) and (R) are True and (R) is the correct explanation of (A)
2.	Both (A) and (R) are False.
3.	(A) is True but (R) is False.
4.	Both (A) and (R) are True but (R) is not the correct explanation of (A)

An acidic buffer is obtained on mixing :
1. 100 mL of 0.1 M CH₃COOH and 100 mL of 0.1 M NaOH.
2. 100 mL of 0.1 M HCl and 200 mL of 0.1 M NaCl.
3. 100 mL of 0.1 M HCl and 200 mL of 0.1 M CH₃COONa.
4. 100 mL of 0.1 M CH₃COOH and 200 mL of 0.1 M NaOH.

If the equilibrium constant for $\mathrm{A}<mspace\; width="1em"></mspace>\rightleftharpoons <mspace\; width="1em"></mspace>\mathrm{B}<mspace\; width="1em"></mspace>+\hspace{0.17em}\mathrm{C}<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{eq}}^{\left(1\right)}$ and that of $\mathrm{B}\hspace{0.17em}+\hspace{0.17em}\mathrm{C}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>\rightleftharpoons <mspace\; width="1em"></mspace>\mathrm{P}<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{eq}}^{\left(2\right)}$, the equilibrium constant for $A<mspace\; width="1em"></mspace>\leftrightharpoons <mspace\; width="1em"></mspace>P$ is: 

1. ${\mathrm{K}}_{\mathrm{eq}}^{\left(2\right)}<mspace\; width="1em"></mspace>-<mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{eq}}^{\left(1\right)}$

2. ${\mathrm{K}}_{\mathrm{eq}}^{(1)\hspace{0.17em}}\times <mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{eq}}^{\left(2\right)}$

3. ${\mathrm{K}}_{\mathrm{eq}}^{\left(1\right)}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{eq}}^{\left(2\right)}$

4. ${\mathrm{K}}_{\mathrm{eq}}^{\left(2\right)}<mspace\; width="1em"></mspace>/<mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{eq}}^{\left(1\right)}$

100 mL of 0.1 M HCl is taken in a beaker and to it 100 mL of 0.1 M NaOH is added in steps of 2 mL and the pH is continuously measured. Which of the following graphs correctly depicts the change in pH?

1.		2.
3.		4.

Consider the following reaction 
\(\mathrm{N}_2 \mathrm{O}_4(g) \rightleftharpoons 2 \mathrm{NO}_2(g) ; \Delta H^0=+58 \mathrm{~kJ}\)
${}_{}$Also, consider the following stimuli on the above equilibrium.

For each of the above cases (I, II), the direction in which the equilibrium shifts is:
1. (I) Towards reactant, (II) No change.
2. (I) Towards product, (II) Towards reactant.
3. (I) Towards product, (II) No change.
4. (I) Towards reactant, (II) Towards product.

For a reaction; $X<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>Y<mspace\; width="1em"></mspace>\leftrightharpoons <mspace\; width="1em"></mspace>2Z$, 1.0 mol of X, 1.5 mol of Y and 0.5 mol of Z were taken in a 1 L vessel and allowed to react. At equilibrium, the concentration of Z was 1.0 mol L^–1 . The equilibrium constant of the reaction is $\frac{x}{15}$. The value of x is:

1. 24

2. 13

3. 16

4. 19

The solubility of Ca(OH)₂ in water is: 

[Given: K_sp Ca(OH)₂ in water = 5.5 × 10^–6]

1. 1.77 × 10^–6

2. 1.11 × 10^–6

3. 1.11 × 10^–2

4. 2.77 × 10^–2

At 1990 K and 1 atm pressure, there are an equal number of Cl₂ molecules and Cl atoms in the reaction mixture.
The value of K_P for the reaction ${\mathrm{Cl}}_{2\left(\mathrm{g}\right)}\rightleftharpoons 2{\mathrm{Cl}}_{\left(\mathrm{g}\right)}$ under the above conditions is x × 10^–1. The value of x is:

1. 4

2. 8

3. 5

4. 10

For the reaction A_(g)$\to$(B)_(g), the value of the equilibrium constant at 300 K and 1 atm is equal to 100.0. The value of $∆$_rG for the reaction at 300 K and 1 atm in J mol^–1 is – xR, where x is:
(R = 8.31 J mol^–1 K^–1 and ln 10 = 2.3)

1. 1400

2. 1380

3. 1360

4. 1340

An aqueous solution contains 0.10 M H₂S and 0.20 M HCl. If the equilibrium constant for the formation of HS^– from H₂S is 1.0 × 10^–7 and that of S^2– from HS^– ions is 1.2 × 10^–13 then the concentration of S^2– ions in aqueous solution will be:

1. 5 × 10^–8 M

2. 3 × 10^–20 M

3. 6 × 10^–21 M

4. 5 × 10^–19 M