The oxide that is not expected to react with sodium hydroxide is : 

1. B₂O₃           

2. CaO

3. SiO₂             

4. BeO

Equimolar solutions of the following were prepared in water separately. Which one of the solutions will record the highest pH?

(1) SrCl₂                             

(2) BaCl₂

(3) MgCl₂                           

(4) CaCl₂

The value of equilibrium constant of the reaction HI (g) $\rightleftharpoons$ $\frac{1}{2}$ H₂(g) + $\frac{1}{2}$ I₂(g) is 8.0. The equilibrium constant of the reaction

H₂(g) + I₂(g) $\rightleftharpoons$2HI(g) will be

$$\begin{gathered} 1. \frac{1}{16} \\ 2. \frac{1}{64} \\ 3. 16 \\ 4. \frac{1}{8} \end{gathered}$$

The pOH of a solution at 25$°$C that contains 1 x 10^-10 M of hydronium ions is:  

1. 7.00                               

2. 4.00

3. 9.00                                 

4. 1.00

Which one of the following ionic species has the greatest proton affinity to form stable compound?

(1) HS^-                         

(2) ${\mathrm{NH}}_2^{-}$

(3) F^-                           

(4) I^-

Given the reaction:

\(\mathrm{Cu}(\mathrm{~s})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Cu}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{~s})\) with E° = 0.46 V at 298 K,
what is the equilibrium constant for the reaction?

Which of the following pairs constitutes a buffer?

1. HNO₂ and NaNO₂

2. NaOH and NaCl

3. HNO₃ and NH₄NO₃

4. HCl and KCl

The hydrogen ion concentration of a 10^-8 M HCl aqueous solution at 298 K (K_w = 10^-14) is:

(1) 1.0×10^-6 M

(2) 1.0525 x 10^-7 M

(3) 9.525 x 10^-8 M

(4) 1.0×10^-8 M

For the chemical equilibrium, CaCO₃(s) $\stackrel{}{\rightleftharpoons }$ CaO(s) + CO₂ (g) ΔH_f° can be determined from which one of the following plots ?

(1)  

(2) 

(3) 

(4) 

Equilibrium constant for the given reaction is kc = 10²⁰ at temperature 300 K,A(s) + 2B (aq.) $\stackrel{}{\rightleftharpoons }$ 2C (s) + D (aq.)K = 10²⁰ The equilibrium conc. of B starting with mixture of 1 mole of A and 1/3 mole/litre of B at 300 K is

(1) $~4\times {10}^{–11}$

(2) $~2\times {10}^{–10}$

(3) $~2\times {10}^{–11}$

(4) $~{10}^{–10}$