Reaction quotient for the reaction, ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$ is given by , $\mathrm{Q}$ $=$ $\frac{{\left[{\mathrm{NH}}_3\right]}^2}{\left[{\mathrm{N}}_2\right]{\left[{\mathrm{H}}_2\right]}^3}$ .The reaction will proceed from right to left if K_c value is:

1.	Q<Kc	2.	Q=0
3.	Q>Kc	4.	Q=Kc

The ratio of \({{K_{P}}\over{K_{C}}}\) for the reaction

$\mathrm{CO}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{CO}}_2\left(\mathrm{g}\right)$ $\mathrm{is:}$

The pair that represents a buffer solution among the following pairs is?

1. ${\mathrm{HNO}}_3$ and ${\mathrm{NH}}_4{\mathrm{NO}}_3$

2. $\mathrm{HCl}$ and $\mathrm{KCl}$

3. ${\mathrm{HNO}}_2$ and ${\mathrm{NaNO}}_2$

4. $\mathrm{NaOH}$ and $\mathrm{NaCl}$

The mixture that can act like a buffer is:

1. ${\mathrm{CH}}_3\mathrm{COOH} + {\mathrm{CH}}_3\mathrm{COONa}$

2. ${\mathrm{NH}}_4{\mathrm{NO}}_3+{\mathrm{NH}}_4\mathrm{OH}$

3. $50 \mathrm{ml} 0.1 \mathrm{m} \mathrm{NaCN}+30 \mathrm{ml} 0.1 \mathrm{m} \mathrm{HCl}$

4. All of the above

An acid buffer solution can be prepared by mixing the solutions of:

1. Sodium chloride and sodium hydroxide

2. Sulphuric acid and sodium sulphate

3. Ammonium chloride and ammonium nitrate

4. Ammonium acetate and acetic acid

A buffer solution can be prepared from a mixture of:

I. Sodium acetate and acetic acid in water

II. Sodium acetate and hydrochloric acid in water

III. Ammonia and ammonium chloride in water

IV. Ammonia and sodium hydroxide in water.

1. I, III, IV

2. III, IV

3. I, II, IV

4. I,  III

The basic buffer solution among the following is: 

1. ${\mathrm{NH}}_4\mathrm{Cl}+{\mathrm{NH}}_4\mathrm{OH}$

2. $\mathrm{NaCl}+\mathrm{NaOH}$

3. ${\mathrm{NH}}_4\mathrm{Cl}+{\mathrm{CH}}_3\mathrm{COOH}$

4. ${\mathrm{CH}}_3\mathrm{COONa}+{\mathrm{CH}}_3\mathrm{COOH}$

Conjugate base of hydrazoic acid is: 

1. \({HN_3}^-\)${}_{}^{}$

2. \(N_2^-\)   ${\mathrm{}}_{}^{}$

3. \(N_3^-\) 
4. \({N^3}^-\)

Out of ${\mathrm{Ca}}^{2+},\hspace{0.17em}{\mathrm{Al}}^{3+},\hspace{0.17em}{\mathrm{Cr}}^{3+}, {\mathrm{Mg}}^{2+}, \mathrm{and} {\mathrm{Zn}}^{2+},$ the reagents ${\mathrm{NH}}_4\mathrm{Cl}$ and aqueous ${\mathrm{NH}}_3$ will precipitate

1. ${\mathrm{Ca}}^{2+},\hspace{0.17em}{\mathrm{Al}}^{3+}$

2. ${\mathrm{Al}}^{3+}, {\mathrm{Cr}}^{3+}$

3. ${\mathrm{Bi}}^{3+}, {\mathrm{Mg}}^{2+}$

4. ${\mathrm{Mg}}^{2+}, {\mathrm{Zn}}^{2+}$

The pH of 0.1 M solution of the following compounds increases in the order of -

1. $\mathrm{NaCl}<{\mathrm{NH}}_4\mathrm{Cl}<\mathrm{NaCN}<\mathrm{HCl}$

2. $\mathrm{HCl}<{\mathrm{NH}}_4\mathrm{Cl}<\mathrm{NaCl}<\mathrm{NaCN}$

3. $\mathrm{NaCN}<{\mathrm{NH}}_4\mathrm{Cl}<\mathrm{NaCl}<\mathrm{HCl}$

4. $\mathrm{HCl}<\mathrm{NaCl}<\mathrm{NaCN}<{\mathrm{NH}}_4\mathrm{Cl}$