(a) Human muscle-fluid,  pH = 6.83 

(b) Human stomach fluid, pH = 1.2

(c) Human blood, pH = 7.38           

(d) Human saliva, pH = 6.4.

Out of the above mentioned biological fluids, the one with the minimum concentration of hydrogen ions is:

1.	Human blood	2.	Human muscle fluid
3.	Human stomach fluid	4.	Human saliva

The pH values of milk, tomato juice, lemon juice, and egg are 6.8, 4.2, 2.2, and 7.8 respectively.

The corresponding hydrogen ion concentration is maximum in: 

The ionization constant of propanoic acid is 1.32 × 10^–5. The degree of ionization of 0.05M acid solution will be:

1. $\mathrm{\alpha }$ = 0.63 × 10^–2

2. $\mathrm{\alpha }$ = 1.63 × 10^–4

3. $\mathrm{\alpha }$ = 1.63 × 10^–2

4. $\mathrm{\alpha }$ = 0.05 × 10^–2

The salt that gives a neutral solution in water is: 

The ionization constant of benzoic acid is 6.46×10⁵ and K_sp for silver benzoate is 2.5×10^–13. Silver benzoate is x times more soluble in a buffer of pH 3.19 compared to its solubility in pure water. The value of x will be:

1. 6.8 

2. 16.8 

3. 33.3 

4.  3.3 

Consider the following reaction:
\(\mathrm{Cu}\left(\mathrm{NO}_3\right)_2(\mathrm{~s}) \rightleftharpoons 2 \mathrm{CuO}(\mathrm{~s})+4 \mathrm{NO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g})\)

What is the equilibrium constant \(K_c\)​ expression for the above reaction?

$1. {\mathrm{K}}_{\mathrm{C}}= \frac{{\left[{\mathrm{NO}}_2\right]}^4\left[{\mathrm{O}}_2\right]}{\left[\mathrm{Cu}{\left({\mathrm{NO}}_3\right)}_2\right]}$
$2. {\mathrm{K}}_{\mathrm{C}}= {\left[{\mathrm{NO}}_2\right]}^4\left[{\mathrm{O}}_2\right]$
$3. {\mathrm{K}}_{\mathrm{C}} =\frac{{\left[\mathrm{CuO}\right]}^2{\left[{\mathrm{NO}}_2\right]}^4\left[{\mathrm{O}}_2\right]}{\left[\mathrm{Cu}{\left({\mathrm{NO}}_3\right)}_2\right]}$
$4. {\mathrm{K}}_{\mathrm{C}} =\frac{{\left[{\mathrm{NO}}_2\right]}^4\left[{\mathrm{O}}_2\right]}{\left[\mathrm{Cu}{\left({\mathrm{NO}}_3\right)}_2\right]}$

${{\mathrm{I}}_2}_{\left(\mathrm{s}\right)}$ $+$ $5{{\mathrm{F}}_2}_{\left(\mathrm{g}\right)}$ $$ $\to 2{\mathrm{IF}}_{5\left(g\right)}$ $$

The solution that has the lowest pH is: 

(assuming 100% dissociation)

The degree of ionization of a 0.1 M bromoacetic acid solution is 0.132. The pK_a of bromacetic acid will be: 

1. 1.98

2. 2.75

3. 4.56

4. 7.15

The species that can act as Bronsted acids as well as bases is/are:

1.  ${\mathrm{H}}_2\mathrm{O}$

2.  ${\mathrm{HCO}}_3^{-},$ ${\mathrm{HSO}}_4^{-}$ $$

3.  ${\mathrm{NH}}_3$

4.  All of the above.